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Acid and Bases Exam ReviewAcid and Base PropertiesList five general properties of aqueous acids and basesProperties of AcidsProperties of BasesName common binary acids and oxyacids, given their chemical formulasHCl = H2SO4 =Name 2 more examplesNaming rules? (you will not be provided with an ion sheet for the exam)Binary Acids =Oxyacids =List acids commonly used in industry and the laboratory and give examples of eachRemember Strong Acids = HI, HClO4, HBr, HCl, H2SO4, HClO3** Strong Bases are metal hydroxides, ammonia is not strongWhat are some acids you have used in lab?Name at least one example of a weak acid.Define acid and base according to Arrhenius’s theory of ionization. List an example of each.Arrhenius Acid = Arrhenius Base = Explain the difference between strong and weak acids and bases. List an example of each.Strong Acid =Weak Acid = Strong Base =Weak Base =Acid and Base TheoriesDefine and recognize Br?nsted-Lowry acids and bases and give an example of each.Br?nsted-Lowry acid = Br?nsted-Lowry base = Define a Lewis acid and a Lewis base and give an example of each.Lewis acid = Lewis base = Name compounds that are acids under the Lewis definition but not under the Br?nsted-Lowry definitionAcid and Base ReactionsDescribe a conjugate acid, a conjugate base, and an amphoteric compound. Give an example of each.Conjugate acid = Conjugate base = Amphoteric compound = Explain the process of neutralization and write an example balanced equation.Define acid rain, give examples of compounds that can cause acid rain, and describe the effects of acid rainThe pH scaleDescribe the self-ionization of water & write the chemical reaction out.Define pH, and give the pH of a neutral solution at 25°C.pH = A neutral solution has a pH of ____.An example of neutral solution is __________ __________ .Explain and use the pH scale. 3429000-114300The pH scale ranges from ____ to ____.It is a ________________ scale (based on 10).The most acidic solution has a pH of _____.The most basic solution has a pH of _____.A neutral solution has a pH of _____.What is the formula to calculate pH?What is the formula to calculate pOH?pH + pOH = _____.What is the Kw of water?In pure water, [H3O+] = ___________.In pure water, [OH-] = ___________.Kw = [H3O+]x[OH-] = ______________.00The pH scale ranges from ____ to ____.It is a ________________ scale (based on 10).The most acidic solution has a pH of _____.The most basic solution has a pH of _____.A neutral solution has a pH of _____.What is the formula to calculate pH?What is the formula to calculate pOH?pH + pOH = _____.What is the Kw of water?In pure water, [H3O+] = ___________.In pure water, [OH-] = ___________.Kw = [H3O+]x[OH-] = ______________.Given [H3O+] or [OH-], find pH.Given pH, find [H3O+] or [OH-].Be able to use logs on your (non-programmable) calculator.TitrationsDescribe how an acid-base indicator functions. Give an example of an indicator that you used.Explain how to carry out an acid-base titration.What is a titration? (definition)What is the purpose of performing a titration?How do you perform a titration? (started in lab yesterday, you will be titrating vinegar on Monday, sketch the lab set-up and explain)Buret = Standard Solution = Unknown Solution = Indicator = Equivalence Point = Sketch:Distinguish between Molarity and Normality.Molarity = Normality = Describe a way you could determine if an unknown solution is acidic or basic (inquiry lab).Describe how you could rank acidic or basic solutions in order of increasing concentration. (inquiry lab).Problems:Identify the acid, base, conjugate acid, and conjugate base in the following reactions.HCN(aq) + SO42-(aq) HSO4-(aq) + CN-(aq) CH3COO-(aq) + H2S(aq) CH3COOH(aq) + HS-(aq) Identify the Lewis acid and Lewis base in the following reactions.Al3+ + 6H2O Al(H2O)63+2NH3 + Ag+ Ag(NH3)2+Calculate the pH if the hydrogen ion concentration is 4.73 x 10-5 M.Calculate the hydroxide ion of a solution with a pH of 8.25.Problems continued:A 0.130 M solution of acetic acid has a hydronium ion concentration of 1.53 x 10-3 M. Calculate the pH of the acid.A 50.0 mL sample of nitric acid is titrated to it end point with 25.2 mL of 2.50 M KOH. What is the concentration of the acid?What is the molarity of a NaOH solution if 38.0 mL of the solution is titrated to its end point with 14.0 mL of 0.750 M sulfuric acid?What volume of 0.12 barium hydroxide is needed to neutralize 12.2 mL of 0.25 M HCl?A cleaner containing NaOH with a volume of 35.2 m: was neutralized with 25.4 mL of 2.50 mL sulfuric acid. Calculate the molarity of NaOH in the cleaner.What is the molarity of 55.3 mL of sulfuric acid if it is titrated to its end point with 122.7 mL of 0.75 M calcium hydroxide?1.An aqueous solution of which of the following reacts with magnesium metal?A.AmmoniaB.Hydrogen chlorideC.Potassium hydroxideD.Sodium hydrogencarbonate2.Which is a buffer solution?I.0.01 mol dm–3 HCl, 0.01 mol dm–3 NaClII.0.01 mol dm–3 CH3COOH, 0.01 mol dm–3 CH3COONaA.I onlyB.II onlyC.Both I and IID.Neither I nor II3.Define the terms strong acid and weak acid. Using hydrochloric and ethanoic acid as examples, write equations to show the dissociation of each acid in aqueous solution.(4)4.(i)Calcium carbonate is added to separate solutions of hydrochloric acid and ethanoic acid of the same concentration. State one similarity and one difference in the observations you could make. (2) (ii)Write an equation for the reaction between hydrochloric acid and calcium carbonate. (2) (iii)Determine the volume of 1.50 mol dm–3 hydrochloric acid that would react with exactly 1.25 g of calcium carbonate. (3)(iv)Calculate the volume of carbon dioxide, measured at 273 K and1.01×105 Pa, which would be produced when 1.25 g of calcium carbonate reacts completely with the hydrochloric acid.(2)5.The graph below shows the change in pH when aqueous sodium hydroxide is added to 20 cm3 of aqueous hydrochloric acid.By reference to the graph(i)state the [H+] before any alkali is added. (1) (ii)state by how much the [H+] changes after the addition of 20 cm3 of aqueous sodium hydroxide. (1) (iii)determine the volume of the same sodium hydroxide solution needed to neutralize?20 cm3 of aqueous ethanoic acid of the same concentration as the hydrochloric acid. (1)6.Propanoic acid, CH3CH2COOH is a weak acid.(a)Give the equation for the ionization of propanoic acid in water and deduce the expression for the ionization constant, Ka, of propanoic acid.(2) (b)Calculate the Ka value of propanoic acid using the pKa value in the Data Booklet.(1) (c)Use your answer from (b) to calculate the [H+] in an aqueous solution of propanoic acid of concentration 0.0500 mol dm–3, and hence the pH of this solution.(3)7.Which one of the following species can act as both a Br?nsted-Lowry acid and base in aqueous solution?A.CH3COOHB.NO3–C.H2PO4–D.OH–8.The Ka value for an acid is 1.0×10–2. What is the Kb value for its conjugate base?A.1.0×10–2B.1.0×10–6C.1.0×10–10D.1.0×10–129.Separate 20.0 cm3 solutions of a weak acid and a strong acid of the same concentration are titrated with NaOH solution. Which will be the same for these two titrations?I.Initial pHII.pH at equivalence pointIII.Volume of NaOH required to reach the equivalence point A.I onlyB.III onlyC.I and II onlyD.II and III only10.Predict whether each of the following solutions would be acidic, alkaline or neutral. In each case explain your reasoning.(i) 0.1 mol dm–3 FeCl3(aq)…………………………………………………………………………………………..…………………………………………………………………………………………..………………………………………………………………………………………….. (ii)0.1 mol dm–3 NaNO3(aq)…………………………………………………………………………………………..…………………………………………………………………………………………..………………………………………………………………………………………….. (iii)0.1 mol dm–3 Na2CO3(aq)…………………………………………………………………………………………..…………………………………………………………………………………………..…………………………………………………………………………………………..(6)20.Which is a conjugate acid-base pair in the following reaction?HNO3 + H2SO4 H2NO3+ + HSO4–A.HNO3 and H2SO4B.HNO3 and H2NO3+C.HNO3 and HSO4–D.H2NO3+ and HSO4–21.Which equation represents an acid-base reaction according to the Lewis theory but not the Br?nsted-Lowry theory?A.NH3 + HCl NH4ClB.2H2O H3O+ + OH–C.NaOH + HCl NaCl + H2OD.CrCl3 + 6NH3 [Cr(NH3)6]3+ + 3Cl–23.An acid-base indicator, HIn, dissociates according to the following equation.HIn(aq) H+(aq) + In–(aq)colour Acolour B Which statement about this indicator is correct?I.In a strongly acidic solution colour B would be seen.II.In a neutral solution the concentrations of HIn(aq) and In–(aq) must be equal.III.It is suitable for use in titrations involving weak acids and weak bases.A.I onlyB.II onlyC.III onlyD.None of the above ................
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