Chemistry Ch.16
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| 1) Identify a good buffer. | show 🗑
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| 2) Which of the following solutions is a good buffer system? | show 🗑
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| show | B) A solution that is 0.10 M HCN and 0.10 M LiCN
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| show | C) A buffer resists pH change by neutralizing added acids and bases.
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| 5) 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? | show 🗑
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| show | A) [HCHO2] < [NaCHO2]
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| 7) If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74, which of the following is TRUE? | show 🗑
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| show | D) 4.49
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| 28) Which of the following is TRUE? | show 🗑
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| 29) Define buffer capacity. | show 🗑
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| 30) The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid? | show 🗑
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| show | C) HClO, pKa = 7.54
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| show | E) HClO2, Ka = 1.1 x 10-2
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| show | C) adding 0.050 moles of HCl
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| 34) A 1.0 L buffer solution is 0.050 M HC2H3O2 and 0.250 M LiC2H3O2. Which of the following actions will destroy the buffer? | show 🗑
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| show | C) 7.4
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| show | B) MgCO3, Ksp = 6.82 × 10-6
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| show | B) FeS
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| show | A) CaCO3 and MgCO3
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| 68) Which of the following compounds solubility will not be affected by a low pH in solution? | show 🗑
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| 79) Which of the following compounds will have the highest molar solubility in pure water? | show 🗑
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| The Ka of hydrazoic acid is 1.9 × 10-5. | show 🗑
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| The Ka of chloroacetic acid is 1.36 × 10-3. | show 🗑
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| In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C? | show 🗑
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| show | B) 1.6 × 10- 2 M
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| 41) What is the molar solubility of AgCl in 0. 10 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021. | show 🗑
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| show | A) The equivalence point is where the amount of acid equals the amount of base during any acid-base titration.
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| show | D) pH will be equal to 7 at the equivalence point.
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| 38) When titrating a weak monoprotic acid with NaOH at 25°C, the | show 🗑
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| 39) When titrating a monoprotic strong acid with a weak base at 25°C, the | show 🗑
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| 40) Identify the most common indicator. | show 🗑
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| 41) Identify the indicator that can be used at the lowest pH. | show 🗑
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| show | B) thymol blue
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| 43) Identify the indicator that can be used at the highest pH. | show 🗑
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| 86) Give the equation for an unsaturated solution in comparing Q with Ksp. | show 🗑
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| show | C) Q = Ksp
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| 88) Give the equation for a supersaturated solution in comparing Q with Ksp. | show 🗑
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| show | C) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution.
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| 90) A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9. | show 🗑
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| show | D) A precipitate will form since Q > Ksp for calcium oxalate.
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| 94) Identify the compound that is acid-insoluble. | show 🗑
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| 95) Identify the compound that is base-insoluble. | show 🗑
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| 96) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl. | show 🗑
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| 97) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl, then H2S and 0.2 M HCl. | show 🗑
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| show | E) ZnS
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| 99) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. | show 🗑
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| 100) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the soluble ions | show 🗑
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| show | D) Lewis base
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| show | A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
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| 103) Gives what happens at low pH for aluminum hydroxide. | show 🗑
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| show | C) Al(OH)3 precipitates
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| show | B) Al(H2O)2(OH)4- dissolves
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| show | B) 1.9 x 10-26 M
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| 107) A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF. If the Kf for AlF63- is 7 × 1019, how much aluminum ion remains at equilibrium? | show 🗑
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| show | C) 0.1 M CaBr2
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| show | 5) pH = pKa2
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| show | 1)pH = 7
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| C) half-way to equivalence point of a weak acid/strong base titration | show 🗑
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| D) equivalence point of a weak base/strong acid titration | show 🗑
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| show | 3)pH > 7
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| 40) What is the molar solubility of AgCl in 0. 30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1. | show 🗑
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| 41) What is the molar solubility of AgCl in 0. 10 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021. | show 🗑
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| show | D) 6.8 × 10-2 M
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| 43) A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds __________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6. | show 🗑
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Created by:
isha2326