front 1 A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4. A)3.63 B)3.34 C)3.46 D)2.89 E)3.57 | back 1 Answer: E |
front 2 Which of the following acids is the WEAKEST? The acid is followed by its Ka value. A)H COOH, 1.8 × 10-4 B)HNO2, 4.6 × 10-4 C)HClO2, 1.1 × 10-2 D)HF, 3.5 × 10-4 E)HCN, 4.9 × 10-10 | back 2 Answer E |
front 3 Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C. A)5.15 B)7.15 C)6.15 D)8.15 E)4.15 | back 3 Answer C |
front 4 The pH of an aqueous solution at 25.0°C is 10.66. What is the molarity of H+ in this solution? A)4.6 × 1010 B)4.6 × 10-4 C)2.2 × 10-11 D)1.1 × 10-13 E)3.3 | back 4 Answer C |
front 5 Consider a reaction that has a negative ΔH and a negative ΔS. Which of the following statements is TRUE? A)This reaction will be nonspontaneous only at high temperatures. B)This reaction will be nonspontaneous at all temperatures. C)This reaction will be spontaneous at all temperatures. D)This reaction will be spontaneous only at high temperatures. E)It is not possible to determine without more information. | back 5 Answer A |
front 6 Calculate the concentration of H3O+ in a solution that contains 5.5 × 10-5 M OH- at 25°C. Identify the solution as acidic, basic, or neutral. A)5.5 × 10-10 M,neutral B)1.8 × 10-10 M,basic C)9.2 × 10-1 M, basic D)1.8 × 10-10 M, acidic E)9.2 × 10-1 M, acidic | back 6 Answer B |
front 7 A buffer solution is 0.100 M in both HC7H5O2 and LiC7H5O2 and has a pH of 4.19. Which of the following pH values would you expect from the addition of a small amount of a dilute solution of a strong base? A)5.69 B)4.49 C)3.69 D)3.89 E)There is not enough information to determine. | back 7 Answer B |
front 8 Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2. The Ka for HC7H5O2 is 6.5 × 10-5. A)4.31 B)9.69 C)4.19 D)10.51 E)4.49 | back 8 Answer E |
front 9 Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO. The Ka for HClO is 2.9 × 10-8. A)3.77 B)7.54 C)6.67 D)6.46 E)7.33 | back 9 Answer E |
front 10 A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 100.0 mL of LiOH. A)0.87 B)12.6 5 C)12.95 D)13.13 E)1.35 | back 10 Answer B |
front 11 Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2. The Ka for HCHO2 is 1.8 × 10-4. A)10.13 B)3.87 C)3.47 D)10.53 E)3.74 | back 11 Answer C |
front 12 Calculate the pH of a solution that contains 3.9 x 10-5 M H3O+ at 25°C. A)0.59 B)5.41 C)8.59 D)9.59 E)4.41 | back 12 Answer E |
front 13 Calculate the pH of a buffer that is 0.105 M HC2H3O2 and 0.146 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10-5. A)9.11 B)9.26 C)4.60 D)4.89 E)4.74 | back 13 Answer D |
front 14 Calculate the pOH of a solution that contains 2.4 × 10-5 M H3O+ at 25°C. A)2.40 B)9.38 C)4.62 D)5.62 E)8.38 | back 14 Answer B |
front 15 Which of the following acids will have the strongest conjugate base? A)HClO4 B)HCN C)HNO3 D)HCl E)HI | back 15 Answer B |
front 16 A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 30.0 mL of LiOH. A)1.12 B)2.86 C)1.21 D)2.00 E)0.86 | back 16 Answer A |
front 17 Determine the pH of a 0.023 M HNO3 solution. A)12.36 B)2.30 C)1.64 D)2.49 E)3.68 | back 17 Answer C |
front 18 Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A)6.5 × 10-5 M B)1.4 × 10-10 M C)8.7 × 10-10 M D)7.1 × 10-5 M E)4.2 × 10-10 M | back 18 Answer D |
front 19 Determine the [OH-] concentration of a 0.123 M Sr(OH)2 solution at 25°C. A)0.0615 M B)8.13 x 10-14 M C)0.123 M D)4.06 x 10-14 M E)0.246 M | back 19 Answer E |
front 20 Which of the following is a triprotic acid? A)CCl4 B)H3PO4 C)H2SO4 D)HI E)HC2H3O2 | back 20 Answer B |
front 21 Calculate the pOH of a solution that contains 7.8 x 10-6 M OH- at 25°C. A)8.89 B)9.64 C)1.28 D)5.11 E)12.72 | back 21 Answer D |
front 22 If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE? A)HCHO2] << [NaCHO2] B)[HCHO2] > [NaCHO2] C)[HCHO2] = [NaCHO2] D)[HCHO2] < [NaCHO2] E)It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. | back 22 Answer B |
front 23 Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2)= 4.87 × 10-17. A)2.44 × 10-17 M B)2.30 × 10-6 M C)3.65 × 10-6 M D)1.62 × 10-17 M E)4.03 × 10-9 M | back 23 Answer B |
front 24 Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 M in hydronium ion. A)2.86 × 10-11 M B)2.86 × 10-3 M C)3.50 × 10-11 M D)2.86 × 10-10 M | back 24 Answer A |
front 25 A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4. A)4.24 B)4.06 C)3.46 D)3.63 E)2.85 | back 25 Answer B |
front 26 Calculate the pH of a buffer that is 0.058 M HF and 0.058 M LiF. The Ka for HF is 3.5 × 10-4. A)10.54 B)9.31 C)4.69 D)3.46 E)2.86 | back 26 Answer D |
front 27 Which of the following is a polyprotic acid? A)H2SO4 B)CCl4 C)HCN D)HI E)HC2H3O2 | back 27 Answer A |
front 28 Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4 A)HBrO2 < HBrO4 < HBrO < HBrO3 B)HBrO < HBrO2 < HBrO3 < HBrO4 C)HBrO4 < HBrO2 < HBrO3 < HBrO D)HBrO2 < HBrO3 < HBrO4 < HBrO E)HBrO < HBrO4 < HBrO3 < HBrO2 | back 28 Answer B |
front 29 What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with ka=3.5 x 10-8. The equation for the dissociation of hypochlorous acid is: HOCl (aq)+ H2O (l)--> <-- H3O + (aq) + OCl- (aq) A)7.2 × 10-4 M B)1.9 × 10-4 M C)7.2 × 10-5 M D)2.8 × 10-5 M | back 29 Answer C |
front 30 A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer? A)adding 0.050 moles of LiC2H3O2 B)adding 0.050 moles of HC2H3O2 C)adding 0.050 moles of NaOH D)adding 0.050 moles of HCl E)None of the above will destroy the buffer. | back 30 Answer D |
front 31 Identify the weak diprotic acid. A)HCOOH B)CH3COOH C)H2CO3 D)H3PO4 E)H2SO4 | back 31 Answer C |
front 32 Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. A)5.4 × 10-3 B)8.5 × 10-6 C)1.2 × 10-5 D)4.9 × 10-7 E)2.7 | back 32 Answer B |
front 33 Identify the weakest acid. A)HF B)HI C)HCl D)HBr E)not enough information is available | back 33 Answer A |
front 34 Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00. A)9.0 × 10-14 B)5.0 × 10-14 C)9.00 D)1.0 × 10-9 E)1.0 × 10-5 | back 34 Answer E |
front 35 Calculate the pH of a buffer that is 0.040 M HF and 0.020 M LiF. The Ka for HF is 3.5 × 10-4. A)3.16 B)3.76 C)4.86 D)2.06 E)3.46 | back 35 Answer A |
front 36 A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 400.0 mL HBr. A)2.11 B)1.22 C)1.00 D)1.40 E)1.30 | back 36 Answer D |
front 37 Identify the weak diprotic acid. A)H3PO4 B)HClO4 C)H2SO3 D)H2SO4 E)HNO3 | back 37 Answer C |
front 38 You wish to prepare an HC2H3O2 buffer with a pH of 4.24. If the pKa of is 4.74, what ratio of C2H3O2 -/HC2H3O2 must you use? A)0.32 B)2.8 C)0.10 D)0.50 E)2.0 | back 38 Answer A |
front 39 A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of ________. A)1.85 B)12.15 C)11.85 D)1.4 × 10-2 E)7.1 × 10-13 | back 39 Answer B |
front 40 A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH. Determine the pH of the solution after the addition of 75.0 mL of LiOH. A)2.65 B)1.89 C)12.1 D)13.06 E)11.35 | back 40 Answer C |
front 41 Calculate the pH for an aqueous solution of pyridine that contains 2.15 x 10-4 M hydroxide ion. A)3.67 B)2.15 × 10-4 C)10.33 D)4.65 × 10-11 | back 41 Answer C |
front 42 Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6. A)8.5 × 10-7 M B)3.0 × 10-4 M C)1.2 × 10-2 M D)2.3 × 10-5 M E)0.0750 M | back 42 Answer B |
front 43 Determine the pOH of a 0.00598 M HClO4 solution. A)11.777 B)2.223 C)6.434 D)7.566 E)3.558 | back 43 Answer A |
front 44 A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10-4. A)9.62 B)7.00 C)3.46 D)10.54 E)8.14 | back 44 Answer E |
front 45 The molar solubility of Ag2S is 1.26 × 10-16 M in pure water. Calculate the Ksp for Ag2S. A)6.81 × 10-63 B)3.78 × 10-12 C)8.00 × 10-48 D)1.12 × 10-8 E)1.59 × 10-32 | back 45 Answer C |
front 46 Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO. The Ka for HClO is 2.9 × 10-8. A)7.06 B)6.46 C)5.99 D)8.01 E)7.54 | back 46 Answer D |
front 47 A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point). A)7.00 B)2.76 C)11.24 D)13.03 E)0.97 | back 47 Answer A |
front 48 Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10-5. A)4.74 B)4.89 C)9.26 D)9.11 E)4.60 | back 48 Answer E |
front 49 What is the hydronium ion concentration of a 0.500 M acetic acid solution with K a = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq)+H2O (l) <-- ---> H3O+(aq)+ CH3CO2 -(aq) A)3.0 × 10-2 M B)3.0 × 10-3 M C)4.2 × 10-3 M D)4.2 × 10-2 M | back 49 Answer B |
front 50 Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 M in hydroxide ion. A)4.00 × 10-7 M B)4.00 × 10-8 M C)4.00 × 10-9 M D)5.00 × 10-9 M | back 50 Answer C |