Practice problems for Chapter 16 5 Determine the pH of a a 0 40 M CH3COOH solution b a solution that is 0 40 M CH3COOH and 0 20 M CH3COONa 6 Determine the pH of a a 0 20 M NH3 solution b a solution that is 0 20 M in NH3 and 0 30 M NH4Cl 9 Which of the following solutions can act as a buffer a KCl HCl b KHSO4 H2SO4 c Na2HPO4 NaH2PO4 d KNO2 HNO2 10 Which of the following solutions can act as a buffer a KCN HCN b Na2SO4 NaHSO4 c NH3 NH4NO3 d NaI HI 11 Calculate the pH of the buffer system made up of 0 15 M NH3 0 35 M NH4Cl 12 Calculate the pH of the following two buffer solutions a 2 0 M CH3COONa 2 0 CH3COOH b 0 20 M CH3COONa 0 20 M CH3COOH Which is the more effective buffer Why 13 The pH of a bicarbonate carbonic acid buffer is 8 00 Calculate the ratio of the concentration of carbonic acid H2CO3 to that of the bicarbonate ion HCO3 14 What is the pH of the buffer 0 10 M Na2HPO4 0 15 M KH2PO4 15 The pH of a sodium acetate acetic acid buffer is 4 50 Calculate the ratio CH3COO CH3COOH 16 The pH of blood plasma is 7 40 Assuming the principal buffer system is HCO3 H2CO3 calculate the ratio HCO3 H2CO3 Is this buffer more effective against an added acid or an added base 17 Calculate the pH of the 0 20 M NH3 0 20 M NH4Cl buffer What is the pH of the buffer after the addition of 10 0 mL of 0 10 M HCl to 65 0 mL of the buffer 18 Calculate the pH of 1 00 L of the buffer 1 00 M CH3COONa 1 00 M CH3COOH before and after the addition of a 0 080 mol NaOH b 0 12 mol HCL Assume there is no change in volume 19 A diprotic acid H2A has the following ionization constants Ka1 1 1 x 10 3 and Ka2 2 5 x 10 6 In order to make up a buffer solution of pH 5 80 which combination would you choose NaHA H2A or Na2A NaHA 21 The diagrams shown contain one or more compounds H2A NaHA and Na2A where H2A is a weak diprotic acid 1 Which of the solutions can act as buffer solutions 2 Which solution is the most effective buffer solution What molecules and Na ions have been omitted 22 The diagrams shown represent solutions containing a weak acid HA pKa 5 00 and its soldium salt NaA 1 Calculate the pH of the solutions 2 What is the pH after the addition of 0 1 mol H ions to solution a 3 What is the pH after the addition of 0 1 mol OH ions to solution d Treat each sphere as 0 1 mol 27 A 0 2688 gram sample of a monoprotic acid neutralizes 16 4 mL of 0 08133 M KOH solution Calculate the molar mass of the acid 28 A 5 00 gram quantity of a diprotic acid was dissolved in water and made up to exactly 250 mL Calculate the molar mass of the acid if 25 0 mL of this solution required 11 1 mL of 1 00 M KOH for neutralization Assume that both protons of the acid were titrated 29 In a titration experiment 12 5 mL of 0 500 M H2SO4 neutralize 50 0 mL of NaOH What is the concentration of the NaOH solution 32 A solution is made by mixing 5 00 x 10 2 mL of 0 167 M NaOH with 5 00 x 10 2 mL of 0 100 M CH3COOH Calculate the equilibrium concentrations of H CH3COOH CH3COO OH and Na 33 Calculate the pH at the equivalence point for the following titration 0 20 M HCl versus 0 20 M methylamine CH3NH2 34 Calculate the pH at the equivalence point for the following titration 0 10 M HCOOH versus 0 10 M NaOH 35 A 25 0 mL solution of 0 100 M CH3COOH is titrated with a 0 200 M KOH solution Calculate the pH after the following additions of the KOH solution a 0 0 mL b 5 0 mL c 10 0 mL d 12 5 mL e 40 0 mL 36 A 10 0 mL solution of 0 300 M NH3 is titrated with a 0 100 M HCl solution Calculate the pH after the following additions of the HCl solution a 0 0 mL b 10 0 mL c 20 0 mL d 30 0 mL e 40 0 mL 45 The ionization constant Ka of an indicator Hln is 1 0 x 10 6 The color of the nonionized form is red and that of the ionized form is yellow What is the color of this indicator in a solution whose pH is 4 00 46 The Ka of a certain indicator is 2 0 x 10 6 The color of Hln is green and that of ln is red A few drops of the indicator are added to a HCl solution which is then titrated against a NaOH solution At what pH will the indicator change color 53 Calculate the concentration of ions in the following saturated solutions a I in AgI solution with Ag 9 1 x 10 9 M b Al3 in Al OH 3 solution with OH 2 9 x 10 9 M 55 The molar solubility of MnCO3 is 4 2 x 10 6 M What is Ksp for this compound 56 The solubility of an ionic compound MX molar mass 346 g is 4 63 x 10 3 g L What is Ksp for this compound 57 The solubility of an ionic compound M2X3 molar mass 288 g is 3 6 x 10 17 g L What is Ksp for the compound 59 What is the pH of a saturated zinc hydroxide solution 60 The pH of a saturated solution of a metal hydroxide MOH is 9 68 Calculate the Ksp for the compound 61 If 20 0 mL of 0 10 M Ba NO3 2 are added to 50 0 mL of 0 10 M Na2CO3 will BaCO3 precipitate 63 Solid NaI is slowly added to a solution that is 0 010 M in Cu and 0 010 M in Ag a Which compound will begin to precipitate first b Calculate Ag when CuI just begins to precipitate c What percent of Ag remains in solution at this point 68 The solubility product of PbBr2 is 8 9 x 10 6 Determine the molar solubility a in pure water b in 0 20 M KBr solution c in 0 20 M Pb NO3 2 solution 69 Calculate the molar solubility of AgCl in a 1 00 L solution containing 10 0 g of dissolved CaCl2 70 Calculate the molar solubility of BaSO4 a in water b in a solution containing 1 0 M SO4 2 ions 71 Which of the following ionic compounds will be more soluble in acid solution …
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