Chemistry 30 - Science with Mr. Dan
Chemistry 30
Homework #24
Name: ____________________________ Date: __________________________
Exercises
1. The reaction below produce equilibrium. Write the Equilibrium reaction (using the double arrow) for each of the following chemical systems.
a) Hydrogen gas reacts with chlorine gas to produce hydrogen chloride gas.
b) We decompose ammonium chloride in ammonia and hydrochloric acid by heating at a very high temperature.
2. Are the following system at equilibrium? If yes, write the Equilibrium reaction
a) Yes / No : A mixture of water and ice is left in a fridge at 0°C
If yes, the reaction is represented by: _____________________________________
b) Yes / No : Propane gas is burned in a BBQ.
If yes, the reaction is represented by: _____________________________________
c) Yes / No : A saturated solution of sodium chloride.
If yes, the reaction is represented by: _____________________________________
d) Yes / No : An unsaturated solution of potassium hydroxide.
If yes, the reaction is represented by: _____________________________________
e) Yes / No : The reaction producing carbon dioxide in pop
If yes, the reaction is represented by: _____________________________________
f) Yes / No : You boil water in an open system
If yes, the reaction is represented by: _____________________________________
3. Equilibrium is theoretically defined as
A. constant changes in observed properties
B. constant properties of a closed system
C. a balance between forward and reverse processes
D. two separate reactions occurring simultaneously
4. At equilibrium in a chemical system,
A. both reactants and products are present in constant amounts
B. the amounts of reactants and products is constantly changing
C. macroscopic properties are slowly changing
D. only products are present
Use the following information to answer the next two questions
5. The equation for the equilibrium reaction is
A. N2(g) + 3 H2(g) ( 2 NH3(g) + 92.2 kJ B. N2(g) + 3 H2(g) + 92.2 kJ ( 2 NH3(g)
C. 2 NH3(g) ( N2(g) + 3 H2(g) + 46.1 kJ D. 2 NH3(g) ( N2(g) + 3 H2(g) (H = -46.1 kJ
6. When ethanoic acid is dissolved in water, the following equilibrium exist
CH3COOH(aq) + H2O(aq) ( H3O+(aq) + CH3COO-(aq)
Which of the following statement is true?
A. At equilibrium, the [CH3COOH(aq) ] = [CH3COO-(aq) ]
B. At equilibrium the pH of the solution is higher than 7
C. At equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction
D. At equilibrium, no more vinegar molecules are present.
Chemistry 30
Homework #25
Name: ____________________________ Date: __________________________
Exercises
1. Write the Equilibrium Constant Expression for each of the following reactions.
a) Hydrogen gas reacts with chlorine gas
to produce hydrogen chloride gas.
b) In the Haber Process, nitrogen gas reacts
with hydrogen to produce ammonia gas.
c) We decompose solid ammonium chloride into ammonia
gas and hydrogen chloride gas.
d) CaCO3(s) ( CO2(g) + CaO(s)
e) 3 NO2(g) + H2O(l) ( 2 HNO3(aq) + NO(g)
f) CH3COOH(l) + CH3OH(l) ( CH3COOCH3(l) + H2O(l)
2. Bromine chloride decomposes according to this equation: 2BrCl(g) ( Cl2(g) + Br2(g)
At a certain temperature, the equilibrium constant for this reaction is 11.1. If the concentration of Cl2(g) is 4.00 mol/L, the concentration of BrCl present at equilibrium is __________ mol/L.
3. The following equation represents a chemical equilibrium : N2O4(g) ( 2NO2(g)
If at equilibrium, the [N2O4(g)] is 0.0045 mol/L and [NO2(g)] is 0.030 mol/L.
a) Write the Equilibrium Constant expression:
b) Find the value of Keq : ________ c) Does the reaction favors the products or reactants? _______
d) Find the equilibrium constant for the reverse reaction. ____________________
4. The equilibrium constants for three reactions are Reaction 1: 1.8 x 10-5,
Reaction 2: 2.3, and Reaction 3: 1.0 x 103. Which reaction favours the
products the most? _________________
5. The value of the equilibrium constant for the decomposition of phosphorus pentachloride gas to phosphorus trichloride and chlorine gas if at equilibrium [PCl3(g)] = [Cl2(g)] = 0.014 mol/L and [PCl5(g)] = 4.3 x 10-4 mol/L is _____________.
6. In a container, carbon monoxide and water vapor are reacted to produce carbon dioxide and hydrogen. 2.00 mol of each reactant is placed in a 500 mL reaction flask. Initial concentrations are [CO(g)] = [H2O(g)] = 4.00 mol/L. If at equilibrium, [CO2(g)] = 2.69 mol/L, find the Keq for the reaction.
Keq = __________________
7. The equilibrium 2 NO2(g) ( N2O4(g) is established when 0.734 mol of NO2(g) is placed in a 2.00 L flask.
If the equilibrium concentration of N2O4(g) is 0.125 mol/L. Calculate the equilibrium constant for the reaction.
Keq = __________________
8. After 4.0 mol of C2H4(g) and 2.5 mol of Br2(g) are placed in a sealed 1.0 L container, the reaction
C2H4(g) + Br2(g) ( C2H4Br2(g) establishes an equilibrium in which the [C2H4(g)] is 2.5 mol/L.
Calculate Keq
Keq = __________________
9. At equilibrium, the concentration of the nitrogen dioxide is 0.650 mol/L and the concentration of the dinitrogen tetraoxide is 0.486 mol/L. Calculate the value of the equilibrium constant.
A. 0.748 B. 0.870 C. 1.15 D. 1.34
10. Calculate the equilibrium constant using the following information.
2SO2(g) + O2(g) ( 2SO3(g)
0.33 mol/L 0.17 mol/L 0.27 mol/L
A. 0.25 B. 2.0 C. 3.9 D. 4.8
11. Consider the reaction : 2NOCl(g) ( 2NO(g) + Cl2(g)
At 25°C, a particular experiment showed the concentrations of the gases to be
[NOCl(g)] = 1.20 mmol/L [NO(g)] = 1.25 x 10-2 mmol/L [Cl2(g)] = 3.00 x 10-1 mmol/L
The equilibrium constant for the reaction is
A. 3.25 x 10-5 mmol/L B. 5.20 x 10-4 mmol/L C. 3.13 x 10-3 mmol/L D. 2.60 x 10-3 mmol/L
12. For the following equilibrium law expression:
Keq = [CO2(g)] [H2(g) ] 4
[CH4(g)] [H2O(g)] ²
The reaction described by this equilibrium is
A. CH4(g) + 2 H2O(g) ( CO2(g) + 4 H2(g) B. CO2(g) + 4 H2(g) ( CH4(g) + 2 H2O(g)
C. CH4(g) + H2O(g) ( CO2(g) + H2(g) D. CO2(g) + H2(g) ( CH4(g) + H2O(g)
13. At a specific temperature, a chemist measured the equilibrium concentrations of all the species for the reaction H2(g) + F2(g) ( 2 HF(g).
The measured concentration at equilibrium were: [H2(g)]= 0.471 mol/L, [F2(g)] = 0.471 mol/L,
[HF(g)] = 0.506 mol/L. The equilibrium constant for this system at the specified temperature is ___________.
Chemistry 30
Homework #26
Name: ____________________________ Date: __________________________
Exercises
1. What would happen to these systems if we add the underlined reactant or product?
a) H2(g) + I2(g) ( 2HI(g) : ______________________________________________
b) NH4Cl(s) ( NH3(g)+ HCl(g) : _____________________________________________
2. What would happen to these systems if we remove the underlined reactant or product?
a) CaCO3(s) ( CO2(g) + CaO(s) : _______________________________________
b) AgCl(s) ( Ag+(aq) + 2 I-(aq) : ___________________________________________
3. For each system, what happen to the equilibrium if you raise the temperature.
a) N2O4(g) + energy ( 2 NO2(g) : _______________________________________
b) 3H2(g) + N2(g) ( 2NH3(g) + energy : ____________________________________
c) CaCO3(s) + energy ( CaO + CO2(g) : _________________________________
d) 2 C(s) + 2 H2(g) + 53 kJ ( C2H4(g) : ____________________________________
4. For the reaction, C2H6(g) ( H2(g) + C2H4(g) , what would be the effect on the system if
a) the pressure were increased? ______________________________________________
b) H2(g) was added to the system? ______________________________________________
5. For the reaction, CO(g) + ½ O2(g) ( CO2(g) + energy, what would be the effect on the system if
a) the pressure was increased? ______________________________________________
b) heat was added to the system? ____________________________________________
6. For the reaction, 2Cu2+(aq) + 4NH3(aq) ( Cu2(NH3)4(aq), what would be
the effect on the system if some CuSO4(s) were added to it? ___________________________
7. For the reaction, CO(g) + NO2(g) ( CO2(g) + NO(g) + 227 kJ, what would be the effect on the system if
a) temperature is increased? __________________ b) volume is decreased? ___________________
8. Suggest three ways to increase the percent yield of SO3(g) (other than increasing the concentration of the reactants) in the following equilibrium reaction: 2 SO2(g) + O2(g) ( 2SO3(g) + 96 kJ.
___________________________ __________________________ _________________________
9. The following equilibrium is important in the production of sulfuric acid: 2SO2(g) + O2(g) ( 2SO3(g)
The yield of sulfur trioxide product can be increased by
A. removing oxygen from the system B. adding oxygen to the system
C. removing sulfur dioxide from the system D. decreasing the pressure in the system
10. Water gas (carbon monoxide and hydrogen) is an important industrial fuel mixture and is prepared by the following equilibrium reaction.
H2O(g) + C(s) + energy ( CO(g) + H2(g)
To maximize the amount of both products, a chemical engineer could
A. use low temperatures B. use high temperatures
C. increase the concentration of the CO(g) D. decrease the concentration of the H2O(g)
Use the following information to answer the next two questions.
|2NO2(g) ( N2O4(g) |
|brown colourless |
11. If the equilibrium mixture is heated, the colour becomes darker brown. The correct interpretation is that the forward reaction is
A. exothermic and the equilibrium shifts to the left B. exothermic and the equilibrium shifts to the right
C. endothermic and the equilibrium shifts to the right D. endothermic and the equilibrium shifts to the left
Use the following information to answer the next question
12. In order to reduce the amount of nitrogen oxide pollutants in the air resulting from the combustion of fossil fuels, a design engineer would like to shift the equilibrium to the left. This could be accomplished by
A. a decrease in temperature B. a decrease in the [NO(g)] in the combustion chamber
C. decreasing the volume D. an increase in the [O2(g) ] in the combustion mixture
Use the following information to answer the next question
|Natural gas can be decomposed at 1300°C in a reaction chamber. |
|The reaction is represented by the equation: CH4(g) ( C(s) + 2 H2(g) |
13. The condition that should maximize the amount of product formed are
A. low pressure and low temperature B. low pressure and high temperature
C. low temperature and high pressure D. high temperature and high pressure
Chemistry 30
Homework #27
Name: ____________________________ Date: __________________________
Exercises
1. After 4.0 mol of C2H4(g) and 2.50 mol of Br2(g) are placed in a sealed 1L container, the reaction
C2H4(g) + Br2(g) ( C2H4Br2(g)
established an equilibrium. The diagram shows the concentration of C2H4(g) as it changes over time at a fixed temperature until the equilibrium is reached.
Concentration (mol/L)
4.0
3.0
2.0
1.0
Time
a) Create an ICE table and calculate the concentration of the other two substances at equilibrium.
[Br2(l) ] = ______________ [C2H4Br2(g) ] = _____________
b) Draw the change of concentration for both substances on the graph above.
c) Calculate the equilibrium constant for this system. ___________________
2. In a solution of CuCl2 , the following equilibrium exists: CuCl42-(aq) + 4 H2O(l) ( Cu(H2O)42+(aq) + 4 Cl-(aq)
For the following stresses put on the equilibrium, predict the shift in the equilibrium. Show the shift and the response on the graph for CuCl42-(aq) and Cl-(aq). CuCl42-(aq) is the top line and Cl-(aq) is the bottom line
a) Hydrochloric acid is added.
Shift: ____________________
b) Hydrochloric acid is removed.
Shift: ____________________
3. Identify the nature of the stress imposed on the following equilibrium system at the five times indicated by coordinates A, B, C, D and E.
C2H4(g) + H2(g) ( C2H6(g) + energy
[pic]
Stress at A: _____________________ Stress at B: ________________________
Stress at C: _____________________ Stress at D: ________________________
Stress at E: _____________________
4. The production of Freon-12, involves the following equilibrium: CCl4(l) + 2 HF(g) ( CCl2F2(g) + 2 HCl(g)
The reaction established an equilibrium, which is disturbed at the time indicated by the vertical dotted line on the graphs on the next page.
Graph #1: Graph #2
[pic] [pic]
a) From graph #1, what stress was applied to the system: _____________________________
b) From graph #2, what stress was applied to the system: _____________________________
5. The production of sulfur trioxide involves the following equilibrium: 2 SO2(g) + O2(g) ( 2 SO3(g) + energy
The reaction established an equilibrium which is disturbed at the time indicated by the vertical dotted line on the graphs below.
Graph #1: Graph #2
[pic] [pic]
a) From graph #1, what stress was applied to the system: _____________________________
b) From graph #2, what stress was applied to the system: _____________________________
Chemistry 30
Homework #28
Name: ____________________________ Date: __________________________
Exercises
1. Find [H30+(aq)] in a cleaning solution that is 0.00400 mol/L KOH : ________________________
2. Find [OH-(aq)] of a solution of apple juice which [H30+(aq)] = 6.00 x 10-3 mol/L: ___________________
3. Calculate the [H30+(aq)] in milk of magnesia that has [OH-(aq)] = 1.43 x 10-4 mol/L: _______________
4. The hydroxide ion concentration in pure water at 25°C is
A. 1.00 x 10-14 mol/L B. 1.00 x 10-7 mol/L C. 1.00 x 107 mol/L D. 1.00 x 1014 mol/L
5. Boric acid is used to maintain a pH level in a electroplating bath:
H3BO3(aq) + SO42-(aq) ( H2BO3-(aq) + HSO4-(aq)
The addition of more NiSO4(aq) would
A. increase the [H3BO3(aq)]and the [SO42-(aq)]
B. decrease the [H2BO3-(aq)] and increase the [HSO4-(aq)]
C. increase the [HSO4-(aq)] and the [H2BO3-(aq)]
D. decrease the [H2BO3-(aq)] and the [HSO4-(aq)]
6. The value for Kw
A. is equal to the [H3O+(aq)] [OH-(aq)]
B. changes depending on the pH
C. shows that adding OH-(aq) increases the[H3O+(aq)]
D. shows that the [OH-(aq)] can never be less than 1.00 x 10-14 mol/L
7. Hydrogen is produced when magnesium reacts with
A. CH3OH(aq) B. C2H5OH(aq) C. CH3COOH(aq) D. C6H12O6(aq)
8. A student wants to clean the spill of a car battery. Which household substance should be used?
A. Water B. Vinegar C. Lemon juice D. Baking soda
9. An acidic solution
A. does not conduct electricity B. reacts with zinc
C. neutralizes CH3COOH(aq) D. taste bitter
10. A student tested two solutions with different indicators. The results were:
Solution Orange IV Phenolphtalein Bromothymol blue
X yellow pink blue
Y yellow colorless yellow
A correct interpretation of these data is that
A. both solution are basic B. both solutions are acidic
C. solution X is basic and solution Y is acidic D. solution X is acidic and solution Y is basic
11. If we add a base to a solution,
A. [H3O+(aq)] decreases and pH increases B. [H3O+(aq)] decreases and pH decreases
C. [H3O+(aq)] increases and pH increases D. [H3O+(aq)] increases and pH decreases
12. If 10.0 g of NaOH are used to make 1.00 L of solution, the [H3O+(aq)] in this solution would be
A. 2.50 x 10-15 mol/L B. 1.00 x 10-14 mol/L C. 2.50 x 10-14 mol/L D. 4.00 x 10-14 mol/L
13. What is the [OH-(aq)] in a 0.15 mol/L nitric acid solution?
A. 1.5 x 10-1 mol/L B. 1.5 x 10-13 mol/L C. 6.7 x 10-13 mol/L D. 6.7 x 10-14 mol/L
14. Which substance increases [H3O+(aq)] ?
A. NH 3(aq) B. CH3OH (aq) C. Ba(OH) 2(aq) D. HCOOH (aq)
15. Arrhenius described acids as substances that
A. turn blue litmus red B. is pink in phenolphtalein
C. produce hydroxide ions in solution D. produce hydrogen ions in solution
16. Find the pH of blood if [OH-(aq) ] = 2.6 x 10-7 mol/L? pH = ____________________
|Colors of an acid with different indicators. |
| |
|Test tubes Indicator Color |
|1 Orange IV Yellow |
|2 Methyl orange Yellow |
|3 Bromocresol green Blue |
|4 Methyl red Orange |
|5 Bromothymol blue Yellow |
17. The approximate pH of the solution is between ______________________
18. We dissolve 2.0 x 10-3 mole of KOH in 100 mL of water. The pH of this solution is ___________.
19. We dissolve 2.0 g of barium hydroxide in 1.00 L of water. The pH of this solution is ___________.
20. A student make a solution in which [H3O+(aq)] = 1.0 x 10-3 mol/L. This solution would
A. be yellow in methylorange B. be pink in phenolphtalein
C. turned litmus red D. be red in alazarin yellow
21. Four unknown solutions labelled I, II, III and IV were tested and these data were obtained:
Indicator I II III IV
Thymol blue green yellow green orange
Methyl orange yellow orange yellow red
Thymolphtalein colorless colorless blue colorless
The acidic solution(s) is/are _________________
22 . An apple was analyzed and found to have a pH of 3.30. The [OH-(aq)] for this sample is ___________
Chemistry 30
Homework #29
Name: ____________________________ Date: __________________________
Exercises
1. Label each species in the following equations as Bronsted-Lowry acid or base. Show the transfer of protons
a) HSO3-(aq) + H2O(l) ( H3O+(aq) + SO32-(aq)
b) H2SO3(aq) + HS-(aq) ( H2S(aq) + HSO3-(aq)
c) HIO3(aq) + HCO3-(aq) ( H2CO3(aq) + IO3-(aq)
d) HCH(aq) + H2O(l) ( H3O+(aq) + CH-(aq)
2. Determine the products for each of the following reactions and label the reactant species in each equation as an acid or a base.
a) CH3COOH(aq) + OH-(aq) ( ___________________________
b) CO3-2(aq) + H2O(l) ( ________________________
a) H2CO3(aq) + S-2(aq) ( ______________________
b) d) H2S(aq) + OH-(aq) ( ________________________
3. For the following acids, write the formula of the conjugate base .
a) HF: __________ b) HCO3- : ___________ c) H2PO4- : __________
d) NH4+ : ___________ e) H2CO3 : ___________ f) H2O: ____________
4. For the following bases, write the formula of the conjugate acid .
a) NH3 : ___________ b) HCOO- : ____________ c) HCO3- : __________
d) SO42- : ____________ e) I- : _______________ f) S2- : _____________
g) H2O : ______________
5. Find the products of the following acid-base reactions. Give the conjugate acid-base pairs
a) NH3(aq) + H2O(l) ( _____________________
b) HF(aq) + CH3COO-(aq) ( _______________________
c) CO32-(aq) + H3O+(aq) ( __________________________
d) HCO3-(aq) + S2-(aq) ( __________________________
6. A conjugate acid-base pair in this system: HSO3-(aq) + H2BO3-(aq) ( SO32-(aq) + H3BO3(aq) is
A. HSO3-(aq) and H3BO3(aq) B. HSO3-(aq) and H2BO3-(aq)
C. H2BO3-(aq) and H3BO3(aq) D. HSO3-(aq) and H2O(l)
7. Choose the equation in which HSO3 -(aq) exibits the behavior of a Bronsted-Lowry base
A. HSO3-(aq) + HClO4(aq) ( HSO4-(aq) + HClO3(aq)
B. HSO3-(aq) + H2PO4-(aq) ( H2SO3(aq) + HPO42- (aq)
C. HSO3-(aq) + H2O(l) ( H3O+(aq) + SO32- (aq)
D. HSO3-(aq) + HCO3- (aq) ( SO32-(aq) + H2CO3(aq)
8. “A substance that increases the hydrogen ion concentration" is the
A. Arrhenius definition of an acid B. Bronsted-Lowry definition of an acid
C. Arrhenius definition of a base D. Bronsted-Lowry definition of a base
9. Which statement is true for a solution with a pH of 7.8?
A. The solution will react with a metal B. [OH-(aq)] > [H3O+(aq)]
C. The solution will not conduct electricity D. The addition of bromothymol blue results in a yellow
10. A pH meter immersed in a solution displays a reading of 4.21. The [OH-(aq)] of the solution is
A. 1.6x 10-10 mol/L B. 6.2 x 10-5 mol/L C. 1.6 x 104 mol/L D. 6.2 x 109 mol/L
11. A worker in the lime plant accidentally inhaled some lime dust (CaO(s)). The taste in his mouth is expected to be
A. sour B. bitter C. sweet D. salty
12. A solution was tested and found to have a pOH of 3.2. This solution would most likely
A. be a proton donor B. react violently with zinc
C. cause thymolphtalein to be blue D. cause bromocresol green to be yellow
Chemistry 30
Homework #30
Name: ____________________________ Date: __________________________
Exercises
1. What is the Kb for the following ions?
a) carbonate ion: ______________________ b) sulfite ion: ________________________
c) acetate ion: ________________________ d) fluoride ion: ________________________
2. Find the pH of the following solutions.
A) 0.100 mol/L Methanoic acid
B) 0.152 mol/L NaHS(aq)
C) 0.18 mol/L NaCN(aq)
D) Hydrogen sulphite ion
E) Nitrous acid
G) 2.3 mmol/L nitric acid
3. An unknown acid is a weak acid. In a 0.10 mol/L solution, the pH of this acid is 1.58. Find Ka and the identity of the acid.
4. A student prepares a 0.20 mol/L solution of ascorbic acid, measures its pH, and finds it to be 2.40. Based on this evidence, what is the Ka for ascorbic acid?
5. Codeine has a Kb of 1.73 x 10-6. Calculate the pH of a 0.020 mol/L codeine solution.
6. The hydroxide ion concentration in a 0.157 mol/L solution of sodium propanoate (NaC2H5COO(aq)) is found to be 1.1 x 10-5 mol/L. Calculate the Kb for the propanoate ion.
7. A student dissolves 0.50 g of barium hydroxide in 1.00 L of water. What is the pH of the solution?
8. The property that acids and bases have in common is that they
A. conduct electricity B. turn red litmus blue C. turn blue litmus red D. taste sour
9. Which anion is the weakest base?
A. F-(aq) B. OH-(aq) C. SO42-(aq) D. HSO4-(aq)
10. 1.80 g of CH3COOH(aq) are dissolved in enough water to make 300 mL of solution. If the indicator dropped into the solution is
A. orange IV, the color of the solution will be orange
B. bromothymol blue, the color of the solution will be blue
C. methyl violet, the color of the solution will be yellow
D. thymol blue, the color of the solution will be yellow
11. A 0.10 mol/L solution containing a single dissolved substance is a very good conductor of electricity and turns blue litmus paper red. The pH of this solution could be approximately
A. 1.4 B. 5.6 C. 7.0 D. 12.3
12. The weakest electrolyte (does not ionize very well) would be a 0.10 mol/L solution of
A. HCl(aq) B. NaCl(aq) C. NaOH(aq) D. HOCl(aq)
13. An unknown 0.10 mol/L acid solution turns bromocresol green to yellow, orange IV to yellow and methyl orange to red. The unknown solutioncould be
A. ammonium chloride B. carbonic acid C. ethanoic acid D. nitric acid
Use the following information to answer the following question
| |
|[pic] |
14. The [H3O+(aq)] in the two solutions
A. is the same and is less than 1.0 x 10-7 mol/L B. is greater in I than in II
C. is greater in II than in I D. is the same and is greater than 1.0 x 10-7 mol/L
15. Container #1 contains an acid with a Ka = 1.0 x 107 and container #2 contains an acid with a Ka = 2.2 x 10-6. If equal volumes and concentrations of the two acid solutions are compared, the acidic solution in container #1 has
A. a higher pH B. more solvent molecules present
C. fewer hydronium ions in solution D. fewer undissociated acid molecules
16. In order to maintain the pH in an electroplating bath, strong acids are added. If a 10 L sample of 1.0 mol/L HCl(aq) is added to 990 L of water, the pH of the acidic solution
A. increased by 2 pH units B. increased by 1 pH unit
C. decreased by 2 pH units D. decreased by 1 pH unit
17. A 0.100 mol/L propanoic acid solution, C2H5COOH(aq), has a pH of 2.95. From these data, the Kb for the propanoate ion, C2H5COO-(aq), is
A. 1.1 x 10-3 B. 1.3 x 10-5 C. 7.9 x 10-10 D. 8.7 x 10-12
18. Which of the following is not associated with a 0.10 mol/L solution of a weak acid?
A. [H3O+(aq] < 0.10 mol/L B. pH = 1.00
C. A small Ka value. D. A relatively strong conjugate base.
Chemistry 30
Homework #31
Name: ____________________________ Date: __________________________
Exercises
1. For each of the following mixtures, write a balanced acid-base equilibrium equation.
A) Solutions of sodium sulfate and hydrofluoric acid are mixed in a beaker.
___________________________________________________________
B) A solution of ammonium nitrate and a solution of NaCH3COO(aq) are mixed.
___________________________________________________________
C) NaC6H5COO(s) is dissolved in a solution of NaHSO4(aq).
___________________________________________________________
D) A household ammonia solution is mixed with a solution of nitrous acid
___________________________________________________________
E) Nitric acid and potassium hydroxide solutions are mixed.
___________________________________________________________
F) Sodium sulfite is dissolved into a solution of sulfurous acid.
___________________________________________________________
G) Bleach (sodium hypochlorite) and vinegar are mixed.
___________________________________________________________
2. Which statement for the system: H2PO4-(aq) + CH3COO-(aq) ( CH3COOH(aq) + HPO42-(aq) is correct
A. H2PO4-(aq) acts as a base B. CH3COOH(aq) acts as a base
C. CH3COO-(aq) acts as an acid D. HPO42-(aq) acts as a base
3. Which solution can neutralize or partially neutralize both acidic and basic solutions?
A. HCOO-(aq) B. CH3COO-(aq) C. HCO3-(aq) D. S2-(aq)
4. A species that could behave as either an acid or a base is
A. sodium carbonate B. Methanol (CH3OH(l)) C. Sodium hydrogen sulfide D. Na3PO4(aq)
5. Which ion is the least capable of acting as either an acid or a base in aqueous solution?
A. HPO42-(aq) B. HCO3- (aq) C. H3O+(aq) D. H2PO4- (aq)
6. In which 0.10 mol/L solution would bromothymol blue turn green?
A. NaOH(aq) B. K2CO3(aq) C. NaCl(aq) D. HOOCCOOH(aq)
Use the following information to answer the following question
| |
|H2(g) + Cl2(g) ( 2HCl(g) (H = -184.6 kJ |
7. If the hydrogen chloride produce when 9.23 kJ of energy are released is dissolved to form 1.5 L of solution, the pH will be _______________.
Use the following information to answer the following question
|1. 0.10 mol/L H2S(aq) |
|2. 0.10 mol/L NaOH(aq) |
|3. 0.10 mol/L H2SO4(aq) |
|4. 0.10 mol/L HOOCCOOH(aq) |
8. When the solutions are listed in order of increasing pH, the order is ______________.
9. Solutions of HCl(aq) acid and sodium hypochlorite are combined. The net ionic equation for the reaction that occurs is
A. HCl(aq) + NaOCl(aq) ( NaCl(aq) + HOCl(aq) B. H+(aq) + NaOCl(aq) ( Na+ (aq) + HOCl(aq)
C. HCl(aq) + OCl- (aq) ( HOCl(aq) + Cl- (aq) D. H3O+ (aq) + OCl- (aq) ( H2O(l) + HOCl(aq)
10. The net ionic equation for the neutralization of ammonia with hydrobromic acid is
A. HBr(aq) + NH3(aq) ( Br-(aq) + NH4+(aq) B. H3O+(aq) + NH3(aq) ( H2O (l) + NH4+(aq)
C. HBr(aq) + NH4OH (aq) ( H2O(l) + NH4Br (aq) D. H3O+ (aq) + NH4OH (aq) ( 2 H2O(l) + NH4+(aq)
11. In the reaction HCl(aq) + H2O(l) ( H3O+(aq) + Cl-(aq) water is
A. an acid B. a proton donor C. an electron acceptor D. a proton acceptor
Chemistry 30
Homework #32
Name: ____________________________ Date: __________________________
Exercises
1. A student adds 250 mL of 0.100 mol/L NaOH(aq) to 249 mL of 0.100 mol/L HNO3(aq). The pH of the mixture is _______.
2. Find the pH of a solution made with 100 mL of 0.250 mol/L HCl(aq) and 100 mL of 0.150 mol/L Ba(OH)2(aq) .
3. A solution is made by mixing 30.0 mL of 0.200 mol/L HCl(aq) with 20.0 mL of 0.300 mol/L HCl(aq) Find the pH of the solution?
4. A solution is made by mixing 30.0 mL of 0.0200 mol/L NaOH(aq) with 20.0 mL of 0.0300 mol/L Ba(OH)2(aq) Find the pH of the solution?
5. 10.0 mL of 0.400 mol/L KOH solution was required to neutralize 40.0 mL of gastric juice (HCl(aq)). The concentration of the acid in the gastric juice _______ mol/L.
6. A student neutralize 10.0 mL of vinegar using a 0.100 mol/L Ba(OH)2 solution. The following data were recorded : Initial buret reading : 0.4 mL and final buret reading : 25.4 mL . The concentration of ethanoic acid in vinegar is _________ mol/L.
7. A sample of Sani-Flush containing 81.0 g of NaHSO4 is dissolved in 4.00 L of water and titrated with 2.00 mol/L KOH. What volume of KOH solution is required for complete reaction?
8. A student uses 0.200 mol/L NaOH(aq) to titrate a sample of H3PO4(aq) . A 10.0 mL sample of the H3PO4(aq) required 45.0 mL of base for complete neutralization Calculate the concentration of H3PO4(aq).
9. 1.59 g of sodium carbonate solid was added to an Erlenmayer flask and titrated with diluted HCl(aq). The titration evidence collected is shown below
Trial 1 2 3 4
Final buret reading 13.3 26.0 38.8 13.4
Initial buret reading 0.2 13.3 26.0 0.6
The concentration of the diluted HCl(aq) Is ___________ mo/L.
10. Which equation is the first step in a reaction of a polyprotic species?
A. OH-(aq) + HCl(aq) ( H2O(l) + Cl-(aq) B. HOOCCOOH(aq) + 2 OH-(aq) ( H2O(l) + OOCCOO2-(aq)
C. HMo(aq) + OH-(aq) ( H2O(l) + Mo-(aq) D. H2CO3(aq) + OH-(aq) ( H2O(l) + HCO3-(aq)
11. The strongest base listed is
A. H3X(aq) b. HX-(aq) C. HX2- (aq) D. X3- (aq)
12. The [OH-(aq)] in a solution made by mixing 50.0 mL of 0.200 mol/L HCl(aq) with 200 mL of 0.300 mol/L HCl(aq) is
A. 2.80 x 10-1 mol/L B. 2.80 x 10-4 mol/L C. 3.57 x 10-11 mol/L D. 3.57 x 10-14 mol/L
13. If 0.10 mol/L solutions of HOCl(aq) and KCH3COO(aq) are mixed together, the following equilibrium is established:
HOCl(aq) + CH3COO-(aq) ( OCl-(aq) + CH3COOH(aq)
This equilibrium
A. favors the reactants B. favors neither side because all concentrations are equal
C. favors the products D. is impossible to predict, given the information available
14. Which 50.0 mL solution requires the greatest volume of 0.100 mol/L HCl(aq) to completely react with it?
A. 0.100 mol/L NaOH(aq) B. 0.100 mol/L NH3(aq)
C. 0.100 mol/L Ba(OH) 2(aq) D. 0.100 mol/L HOOCCOOH(aq)
15. In which reaction would the reactants be the favored species?
A. H2CO3(aq) + OH-(aq) ( HCO3-(aq) + H2O(l) B. HSO3-(aq) + PO43-(aq) ( HPO4-(aq) + SO32-(aq)
C. H3O+(aq) + CH3COO-(aq) ( CH3COOH(aq) + H2O(l) D. H2S(aq) + OOCCOO2-(aq) ( HOOCCOO-(aq) + HS-aq)
Chemistry 30
Homework #33
Name: ____________________________ Date: __________________________
Exercises
1. Sketch the pH curve of the following titration. The concentration of each substance is 0.100 mol/L.
Predict whether the pH endpoint is (=7) (7).
a) Hydrobromic acid + sodium phosphate b) Oxalic acid + sodium hydroxide.
c) Perchloric acid and potassium hydroxide d) Carbonic acid + KOH(aq) .
e) Sodium sulfate + nitric acid. f) Hydrocyanic acid + NaOH(aq) .
2. For the following titrations, answer the following questions:
- How many endpoints would you see on the pH curve of the titrations?
- For each endpoint, write the approximate value.
a) Titration of HNO3(aq) with NaOH(aq) Number of endpoints values: ____________
b) Titration of H2SO3(aq) with NaOH(aq) Number of endpoints values: ____________
c) Titration of H3PO4(aq) with KOH(aq) Number of endpoints values: ____________
d) Titration of HCN(aq) with NaOH(aq) Number of endpoints values: ____________
e) Titration of Ba(OH)2(aq) with HCl(aq) Number of endpoints values: ____________
f) Titration of S2-(aq) with HCl(aq) Number of endpoints values: ____________
g) Titration of PO43-(aq) with HCl(aq) Number of endpoints values: ____________
3. Will the following solution pairs form an effective buffer?
a) HNO3(aq) and NaNO3(aq) : _______________
b) NH3(aq) and NH4Cl(aq) : _______________
c) HCl(aq) and NaOH(aq) : _______________
d) C6H5COOH(aq) and NaC6H5COO(aq) : _______________
4. An important part of the buffer in blood is the
A. hydrogen carbonate ions B. acetate ion C. ethanoate ion D. ammonium ion
5. A buffer system of CH3COOH3(aq) / NaCH3COO (aq) works best if
A. the solution to be buffered has a pH greater than 7
B. the amount of CH3COOH3(aq) and CH3COO-(aq) are large compared to the amount of acid or base added
C. large amounts of acid or base are added to the buffered system
D. the concentration of CH3COO-(aq) is small compared to the concentration of CH3COOH(aq).
6. The buffering region on this graph occurs at point (circle your answer on the graph)
[pic]
7. The true statement about the reaction between carbonate ions and the buffer system is that the equilibrium favors
A. products because HCO3-(aq is a weaker acid than H2PO4-(aq
B. products because H2PO4-(aq is a weaker acid than HCO3-(aq
C. reactants because HCO3-(aq is a weaker acid than H2PO4-(aq
D. reactants because H2PO4-(aq is a stronger acid than CO32-(aq
Use the following information to answer the next two questions
8. The most likely reaction between this buffer system and a solution containing the carbonate ion is
A. CO32-(aq) + H3PO4(aq) ( H2PO4-(aq + HCO3-(aq) B. CO32-(aq) + HPO42-(aq ( PO43-(aq + HCO3-(aq) C. CO32-(aq) + H2PO4-(aq) ( HPO42-(aq + HCO3-(aq) D. HCO3-(aq) + H2PO4-(aq ( H2CO3(aq + HPO42-(aq)
9. Blood maintains a nearly constant pH because it contains
A. sodium ions and chloride ions that keep the pH of the blood at 7
B. hemoglobin that maintains the oxygen levels in the blood
C. catalysts (enzymes) that control the equilibrium in the blood
D. buffers that regulate the hydronium ion concentration in the blood
10. The conjugate base of N2H5+(aq) is
A. HOH(l) B. OH-(aq) C. N2H6+2(aq) D. N2H4(aq)
11. Which of the following solutions could act as a buffer system?
A. KH2PO4(aq) / H3PO4(aq) B. KCl(aq) / HCl(aq) C. KClO4(aq) / HClO4(aq) D. KNO3(aq) / HNO3(aq)
Use the following information to answer the next question
12. When equal concentrations of HOCl(aq) and OCl-(aq) are present, the pH of the swimming pool water is ___________
Chemistry 30
REVISION
Name: ____________________________ Date: __________________________
Exercices
1. The equivalence point of this titration occurs at point
[pic]
2. The equivalence point in an acid-base titration will have a pH of 7 for the titration of
A. OH-(aq) with vinegar B. ammonia with hydrochloric acid
C. acetic acid with potassium hydroxide D. hydrochloric acid with sodium hydroxide
3. The ion H2AsO4-(aq) has both a conjugate acid and a conjugate base. These are, respectively
A. H3AsO4(aq) and AsO43-(aq) B. HAsO42-(aq) and AsO43-(aq)
C. H3AsO4(aq) and HAsO42-(aq) D. H4AsO4+(aq) and AsO43-(aq)
Use the following graph to answer the next question
[pic]
4. The acid in the titration is
A. HOOCCOOH(aq) B. CH3COOH(aq) C. HNO3(aq) D. HCl(aq)
5. A student mixed 100.0 mL of 0.50 mol/L acid samples with 100.0 mL of 0.50 mol/L base samples and measured the heat released by each mixture. The results are tabulated below:
Heat released
HCl(aq) + NaOH(aq) 50 kJ/mol
HNO3(aq) + KOH(aq) 49 kJ/mol
HBr(aq) + NaOH(aq) 52 kJ/mol
HCl(aq) + KOH(aq) 49 kJ/mol
The heats of reaction are all nearly the same because
A. each acid is monoprotic.
B. these acids and bases are all soluble electrolytes.
C. the same net ionic reaction occurs in each case
D. solutions of KOH(aq) and NaOH(aq) of equal concentration have the same [OH-(aq)]
6. A student did four acid-base titrations and plotted them on the same graph. Which of the four curves best represents the neutralization of a weak acid by a strong base?
[pic]
Volume added
7. The pH at the equivalence point of an acid-base titration is 9.2. This result would be consistent with the titration of a
A. strong acid with a strong base B. weak acid with a strong base
C. strong acid with a weak base D. weak acid with a weak base
Use the following information to answer the next question
8. Which statement explains the low volume of NaOH(aq) used in trial I?
A. The color observed was dark pink B. The buret tip was not filled before titrating
C. The HCl(aq) was diluted by water left in the pipet D. The NaOH(aq) was diluted by water left in the buret
9. A 20.0 mL sample of 0.300 mol/L NaOH(aq) is required to completely react with 30.0 mL of HNO2(aq). What was the concentration of the nitrous acid?
A. 2.56 mol/L b. 1.56 mol/L C. 0.450 mol/L D. 0.200 mol/L
Use the following information to answer the next question
10. A physical characteristic that all these reactions share is a
A. yellow color at the end B. transfer of proton
C. transfer of electrons D. decrease in electricla conductivity
11. Examples of two conjugate acid-base pairs are
A. H3Ct(aq) and H2O(l) , H2Ct- (aq) and H3O+ (aq) B. H2Ct- (aq) and H3O+ (aq) , HCt2- (aq) and H2O(l)
C. H3Ct(aq) and HCt2- (aq) , H3O+ (aq)and H2O(aq) D. HCt2- (aq) and Ct3- (aq) , H3O+ (aq) and H2O(l)
Use the following information to answer the next question
12. On the pH curve showing the titration of a weak base with a strong acid, it can be seen that the pH changes very gradually at I compared to II. The reason for this is that
A. the acid is not as strong at I as at II B. the solution at I is a buffer solution
C. all the base reacted at I D. pH always changes rapidly around pH = 7
13. A 25.0 mL sample of citric acid is titrated to the equivalence point with 0.100 mol/L sodium hydroxide solution in the presence of a phenolphtalein indicator. Which of the following statements is correct?
A. The end-point is reached when the concentration of the acid equals the concentration of the base.
B. The end-point is reached when the concentration of HPh approximately equals the concentration of Ph- .
C. The equivalence point is reached when the volume of base equals the volume of acid.
D. The equivalence point is reached when the pH is equal to 7.00.
14. Equal volumes of an acid and a base solution are mixed. The resulting solution has properties that are not characteristic of either an acidic or a basic solution. This occurs because
A. a strong acid and a weak base were mixed
B. a weak acid and a strong base were mixed
C. a single replacement reaction occurred and hydrogen gas was produced
D. the acid and base contained equivalent amounts of H3O+ (aq) and OH-(aq)
15. Which of the following graphs best represents the neutralization of a diprotic acid by the continuous addition of
0.10 mol/L NaOH(aq)?
[pic]
16. A base is titrated with an acid solution until the indicator changes colour. This change in the colour of the indicator is referred to as the
A. end point B. equivalence point C. equilibrium point D. neutralization point
Use the following information to answer the next question
17. The graph represents the titration of
A. barium hydroxide and hydrochloric acid B. potassium hydroxide with oxalic acid
C. hydrochloric acid with ammonia D. acetic acid with sodium hydroxide
18. An acid that is not polyprotic is
A. HOOCCOOH(aq) B. H2BO2-(aq) C. HCOOH(aq) D. H2SO4(aq)
19. To completely react 50 mL of 0.10 mol/L acid, 150 mL of 0.10 mol/L KOH(aq) was required. The number of protons donated by each acid molecule was
A. 1 B. 2 C. 3 D. 4
Use the following graph to answer the next question
| |
|[pic] |
20. The titration best represented by the graph is
A. HOOCCOOH(aq) titrated with NaOH(aq) B. CH3COOH(aq) titrated with Na2CO3(aq)
C. HCl(aq) titrated with Ba(OH)2(aq) D. H3O+(aq) titrated with NH4OH(aq)
21. One of the buffer systems in the human body is
HCO3-(aq) + H2O(l) ( H2CO3(aq) + OH-(aq)
This buffer system would respond to the addition of vinegar, CH3COOH(aq), by
A. replacing the vinegar with OH-(aq)
B. reacting the vinegar with carbonic acid
C. shifting the equilibrium to the right because [OH(aq)] would decrease
D. shifting the equilibrium to the left, producing more carbonic acid
Use the following equations and key to answer the next question
| |
|Equations |
| |
|HOCN(aq) + C3H5O3-(aq) ( OCN- (aq) + HC3H5O3(aq) (Products favoured) |
|HC3H5O3(aq) + C6H5COO-(aq) ( C3H5O3- (aq) + C6H5COOH(aq) (Products favoured) |
|HOCN(aq) + IO3-(aq) ( OCN- (aq) + HIO3(aq) (Reactants favoured) |
| |
|Key |
| |
|1 C6H5COOH(aq) 4 OCN- (aq) 7 HC3H5O3(aq) |
|2 C6H5COO-(aq) 5 HIO3(aq) 8 C3H5O3- (aq) |
|3 HOCN(aq) 6 IO3-(aq) |
22. The acids, order from the weakest to the strongest, are ________________.
Use the following graph to answer the next question
|pH curve for the titration of 37 mL of |
|0.10 mol/L H3PO4(aq) with NaOH(aq) |
| |
|[pic] |
23. The Bronsted-Lowry equation that occurs between point I and II is
A. H2PO4-(aq) + OH- (aq) ( HPO42-(aq) + H2O(l) B. H3PO4(aq) + OH- (aq) ( H2PO4-(aq) + H2O(l)
C. HPO42-(aq) + OH- (aq) ( PO43-(aq) + H2O(l) D. H3PO4(aq) + 2 OH- (aq) ( HPO42-(aq) + H2O(l)
24. A 10.0 mL sample of CH3COOH(aq) is titrated to the equivalence point with 25.0 mL of 0.0714 mol/L NaOH(aq). The concentration of the CH3COOH(aq) is
A. 2.04 mol/L B. 0.250 mol/L C.125 mol/L D. 0.0200 mol/L
25. If hydrochloric acid is continuously added to a solution that contains both Na2CO3(aq) and Na2SO3(aq), the following reactions will occur:
1. H3O+(aq) + SO32-(aq) ( HSO3-(aq) + H2O(l)
2. H3O+(aq) + CO32-(aq) ( HCO3-(aq) + H2O(l)
3. H3O+(aq) + HSO3-(aq) ( H2SO3(aq) + H2O(l)
4. H3O+(aq) + HCO3-(aq) ( H2CO3(aq) + H2O(l)
The order in which these reactions occur is __________.
Use the following information to answer the next question
26. Solutions of ammonium chloride and sodium hydroxide are mixed together. The net ionic equation that represents the acid-base reaction that occurs is outlined below. The reactants and products in the order stated, as selected from the above numbered species, would be
__________ + ___________ ( _____________ + ______________
acid base conjugate acid conjugate base
Use the following diagram to answer the next question
27. The code for the color of the solution in the
beaker when
- no HCl(aq) is added is ________
- 5.0 mL of HCl(aq) are added is _______
- 10.0 mL of HCl(aq) are added is ________
- 15.0 mL of HCl(aq) are added is ________
Use the following equation to answer the next question
C(s) + 2 H2(g) ( CH4(g)
28. a) Write the equilibrium constant expression.
b) Calculate the equilibrium constant if at equilibrium, [C(s) ] = [H2(g) ] = 1.00 mol/L and [CH4(g) ] = 1.73 mol/L.
Answer: ________
Use the following equilibrium to answer all the questions below
2 NO2(g) + O2(g) ( 2 NO3(g) + Energy
29. a) Calculate the equilibrium constant if the initial [NO2(g) ] = 2.00 mol/L and the initial [O2(g) ] = 1.00 mol/L (No product is added). After the equilibrium was reached, the [NO3(g) ] was 1.74 mol/L.
Answer: ________
b) Is the equilibrium favoring the products or the reactants? _______________
c) Calculate the Keq for the reverse reaction. _________________
d) How would the equilibrium shift if the temperature is risen: _________________________
e) How would the equilibrium shift the pressure is increased: ______________________________
Use the following information to answer the next question
30. Match each of the stresses identified above with the letter on the graph that indicates the time at which the stress was applied.
Stress applied : ______ ________ _______ _______
Time : W X Y Z
31. What is the pH of the following solutions?
a) A solution made with 4.00 g of Ba(OH)2(s) dissolved in 5000 mL of water? ___________
b) A 0.0500 mol/L HCl solution. ____________
c) A solution made with 15.0 g of sodium carbonate dissolved in 500 mL of water. ____________
d) A 0.0125 mol/L HF solution. ____________
32. The pain-killing ingredient in an aspirin tablet is acetylsalicylic acid, a weak solid monoprotic acid whose molar mass is 180.16 g/mol.
A 1.85 g aspirin tablet is dissolved in water to form 30.0 mL of solution. It is then titrated with 41.9 mL of 0.19 mol/L NaOH(aq) to reach the equivalence point.
Using the abbreviation HASA for acetylsalicylic acid, write the net ionic equation for the reaction between the acid and the base and calculate the mass of acetylsalicylic acid in the tablet.
Net ionic equation: _______________________________________________________
Calculation:
Answer: __________
33. A student recorded data during the titration of a 25.0 mL sample of an unidentified base with 0.100 mol/L HCl(aq).
Volume of acid (mL) pH Volume of acid (mL) pH
0.0 10.1 40.0 5.0
10.0 9.1 45.0 2.2
20.0 8.9 50.0 1.9
30.0 8.3 60.0 1.6
35.0 7.9 70.0 1.5
A) Plot the data from the table. Mark the equivalence point with an X.
B) Calculate the initial concentration of the base.
C) What indicator would be suitable for use in this titration? _________________________
D) What conclusion can you draw about the type of base? ____________________
Use the following information to answer the next question
In a container at 900°C, carbon monoxide and water vapor are reacted to produce carbon dioxide and hydrogen.
2.00 mol of carbon monoxide and 3 moles of water vapour are placed in a 500 mL reaction flask. At equilibrium, the concentration of hydrogen is 2.69 mol/L. It took 30 s for the equilibrium to be reached.
1. Write the equilibrium constant expression for this reaction.
2. Calculate the Keq value for this reaction. (You need to set-up an ICE table)
3. Make a sketch of the graph representing this equilibrium
2. Suggest two ways of increasing the production of hydrogen.
-----------------------
The Haber process uses hydrogen and nitrogen to produce ammonia for use as a feedstock for other processes or as a fertilizer.
N2(g) + O2(g) + 180.4 kJ ( 2 NO(g)
Acid-base reactions are critical to maintain equilibrium within the human body. A constant pH is maintained by the HPO42-(aq) / H2PO4-(aq) buffer system
Municipal swimming pool water is treated with chlorine compounds. To assure safe, appropriate levels of these chlorine compounds, a pH range of 7.2 to 7.8 is essential. Within this pH range, the equilibrium H2O(l) + HOCl(aq) ( H3O+(aq) + OCl-(aq) maintains approximately equal concentration of HOCl(aq) and OCl-(aq)
These titration data were obtained for a 10.0 mL HCl(aq) sample titrated with 0.10 mol/L NaOH(aq).
Trial I II III IV
Final buret volume (mL) 13.3 25.9 38.5 33.3
Final buret volume (mL) 1.2 13.2 25.9 20.6
Volume of NaOH used (mL) 12.1 12.7 12.6 12.7
The indicaor used in all cases was phenolphtalein
Bb-(aq) + H3O+(aq) ( HBb(aq) + H2O(l)
Cr2O72-(aq) + H2O(l) ( 2 CrO42-(aq) + 2 H+(aq)
HMo(aq) + OH-(aq) ( Mo-(aq) + H2O(l)
[pic]
[pic]
1. NH4+(aq) 4 OH-(aq)
2. Cl-(aq) 5 NH3(aq)
3. CO32-(aq) 6 H2O(aq)
[pic]
[pic]
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