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5 Written questions

5 Matching questions

  1. The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH3NH3Cl) in 1.00 L of 1.10 M methylamine (CH3NH2) is ________. The Kb for methylamine is 4.40 x 10 ^-4. (Assume the final volume is 1.00L.)
  2. In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?
  3. What is the molar solubility of barium fluoride (BaF2) in water? The solubility-product constant for BaF2 is 1.7 x 10^-6 at 25C.
  4. Which compound listed below has the smallest molar solubility in water?
  5. A solution containing which of the following pairs of substances will be a buffer solution?
  1. a 0.20 NaBr
  2. b 7.5 x 10 ^ -3 green.egg tripod
  3. c AgI
  4. d 11.14 apple apple. apple dog
  5. e CsF, HF

5 Multiple choice questions

  1. .020 M BaCl2 (2nd)
  2. 0.723 O. green blue cat
  3. 1.6 x 10^-5 apple .flower quint
  4. 1.1 x 10^-2 apple. apple toodles
  5. 4.488 dog. dog hat hat

5 True/False questions

  1. Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 x 10^-4.3.487 cat. dog hat green


  2. The Kb of ammonia is 1.77 x 10^-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M ammonium nitrate is _________________.4.077 dog. O green green


  3. In which aqueous solution is PbI2 least soluble?0.8 M KI


  4. Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2) and 0.290 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 x 10 ^-4.4.488 dog. dog hat hat


  5. In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?0.20 NaBr