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5 Written questions

5 Matching questions

  1. Of the substances below, ________ will decrease the solubility of Pb(OH)2 in a saturated solution.
  2. In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?
  3. Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid HBz and 0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 x 10^-5.
  4. In which aqueous solution is PbI2 least soluble?
  5. Which of the following could be added to a solution of acetic acid to prepare a buffer?
  1. a 0.8 M KI
  2. b Pb(NO3)2
  3. c sodium hydroxide
  4. d 4.488 dog. dog hat hat
  5. e 0.20 NaBr

5 Multiple choice questions

  1. 7.5 x 10 ^ -3 green.egg tripod
  2. 4.3 x 10^-14 dog. cat fortune
  3. 1.6 x 10^-5 apple .flower quint
  4. AgI
  5. 3.487 cat. dog hat green

5 True/False questions

  1. In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?0.020 M BaCl2

          

  2. A 25 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. What is the [H+] (molarity) before any base is added?2.83 blue.hat cat

          

  3. In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?.020 M BaCl2 (2nd)

          

  4. 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.)4.488 dog. dog hat hat

          

  5. 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 x 10^ -6.4.3 x 10^-14 dog. cat fortune