SCH3U - Acids & Bases Worksheet



SCH3U - Acids & Bases Worksheet

|1.    |Explain the meaning of the terms "strong" and "weak" when applied to acids and bases. |

|2. |Give illustrations of a strong acid, a strong base, a weak acid and a weak base. |

|3. |Phosphoric acid is the active ingredient in many commercial rust-removing solutions.  Calculate the volume of concentrated phosphoric |

| |acid (14.6 M) that must be diluted to prepare 500 mL of a 1.25 M solution? |

|4. |How did Arrhenius define and acid and a base? |

|5. |Pure HClO4 is molecular.  Write an equation for its dissolution in water. |

|6. |What is the difference between a strong electrolyte and a weak electrolyte. |

|7. |If a substance is a weak electrolyte, what does this mean in terms of the tendency of the ions to react to form the molecular compound? |

| |How does this compare with strong electrolytes? |

|8.  |Nitrous acid, HNO2, is a weak acid.  Write an equation showing its reaction with water. |

|9. |Hydrazine is a toxic substance that can be formed when household ammonia is mixed with a bleach such as CloroxTM.  Its formula is |

| |N2H4 and it is a weak base.  Write a chemical equation showing its reaction with water. |

|10. |HClO3 is a strong acid.  Write an equation for its reaction with water. |

|11.   |Formic acid, HCHO2, is the substance that is responsible for the painful bites of fire ants.  It is a weak electrolyte and reacts with |

| |water in the same manner as acetic acid.  Write a chemical equation that shows its ionization in water. |

|12. |Write the formula for the conjugate bases for each of these acids: |

| |a) HCl;   b) CH4;    c) HSO3-1;     d)   H2SO4;     e) NH3;    f) HClO4 |

|13. |Show how each of these acids react with water and forms a conjugate acid-base pair: |

| |a)  HCl;    b)  HNO3;    c) H2SO4;   d) HClO4;   e) H2S;    f)   H3PO4 |

|14. |Calculate the molarity of a solution that contains 10 grams of HCl in 100 mL of solution. |

|15. |A solution contains 0.1 mole of HC2H3O2 dissolved in 0.5 L of solution. Calculate the molarity of the solution. |

|16. |500 mL of a solution contain 0.1 mole of HC2H3O2. The solution is diluted with water to the 1 L mark. Calculate the molarity of the |

| |resulting solution. |

|17. |A 250 mL solution of H2SO4 has a strength of 0.2 M. The solution is diluted with water to the 1 L mark. What is the molarity of the |

| |solution so formed? |

|18. |If 0.3 mole of acetic acid is present in 150 mL of solution, calculate the molarity of the acid solution. |

|19. |How many moles of acetic acid are required to make 125 ml of a 0.5 M solution. |

|20. |To what volume must 125 mL of a 2 M solution of HCl  be diluted to make the solution 0.05M? |

|21. |What is the concentration of a solution formed by diluting 300 mL of a solution containing 0.1 mole of HCl to 6 L? |

|22. |Give directions for preparing 2.0 L of 0.250 mol/L HCl using 11.7 M HCl. |

|23. |Give directions for preparing 5.00 L of 0.15 mol/L H2SO4 using 18.0 M H2SO4. |

|24. |What volume of 2.00 mol/L HNO3 is needed to yield 10.00 grams of HNO3? |

SCH3U - pH Calculations

|1. |What is the pH of a 0.0010 M HCl solution? |

| |a)  0.0       b)  1.0         c)  2.0         d)  3.0         e)   4.0 |

|2. |What is the molar concentration of hydronium ions in a solution of pH 5.50? |

| |a)   5.50 M     b)   3.2 X 10-5 M      c)   5.0 X 10-5 M     |

| |d)   3.2 X 10-6 M      e)    3.2 X 10-1 M |

|3. |What hydrogen ion concentration corresponds to a pH of 8.64? |

| |a)    0.94 M      b)   4.4 X 10-6 M      c)   2.3 X 10-6 M     |

| |d)   4.4 X 10-9 M      e)    2.3 X 10-9 M |

|4. |What is the hydrogen ion concentration in a solution of pH 5.76? |

| |a)  1.74 X 10-6 M       b)   5.76 X 10-6 M      c)   2.40 X 10-6 M    |

| |d)   5.76 X 10-5 M      e)   7.64 X 10-5 M |

|5.  |What is the  [H+] in a 0.15 molar solution of acetic acid in water at 25oC?  Acetic acid is 1.3% dissociated. |

| |a)  1.10 X 10-2 M       b)   1.95 X 10-3 M      c)   1.20 X 10-4 M    |

| |d)   1.80 X 10-5 M      e)   2.75 X 10-6 M |

|6.  |What is the H+ ion concentration of an aqueous solution that has a pH of 11? |

| |a)  1.0 X 10-11 M       b)   1.00 X 10-3 M      c)   3.0 X 10-1 M    d)   11 X 10-1 M |

|7. |If an aqueous solution has a [OH-1] = 3.0 X 10-11, the solution would be |

| |a) an acidic solution    b) a basic solution   c) a neutral solution   d) a salty solution |

|8. |The pH of a solution in which the hydroxide ion concentration is 2.00 X 10-3 mol/L is |

| |a) 1.70        b)  2.70        c)  11.0       d) 11.3 |

|9. |The pH of a solution is 5.  The hydrogen ion and hydroxide ion concentrations are: |

| |a)   [H+1] = 1.0 X 10-9 M;  [OH-1] = 1.0 X 10-5 M |

| |b)   [H+1] = 1.0 X 10-5 M;  [OH-1] = 1.0 X 10-5 M |

| |c)   [H+1] = 1.0 X 10-5 M;  [OH-1] = 1.0 X 10-9 M |

| |d)   [H+1] = 1.0 X 10-7 M;  [OH-1] = 1.0 X 10-9 M |

|10.  |The pOH of 0.00010 M nitric acid solution is |

| |a)   1.0 X 10-10     b)   1.0 X 10-4      c)   10          d)   4.0  |

|11. |How are acidic, basic, and neutral solutions in water defined; |

| |a)  in terms of [H+1] and [OH-1] |

| |b)  in terms of pH |

|12. |A sodium hydroxide solution is prepared by dissolving 6.0 g of NaOH in 1.00 L of water.  What is the pOH and pH of this solution? |

|13. |A solution was made by dissolving 0.837 grams of Ba(OH)2 in 100 mL of water.  If Ba(OH)2 is fully dissociated into ions what is the pOH |

| |and pH of the resulting solution? |

|14. |What is the pH and pOH of a solution made by adding 400 mL of distilled water to 10 mL of 0.010 M HNO3?  You may assume that volumes are |

| |additive. |

|15. |  What is the [OH-1] and pH of these solutions: |

| |a)    5.6 mg of KOH dissolved in 100 mL of solution. |

| |b)    74 mg of Ca(OH)2 dissolved in 2.0 litres of solution. |

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