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5 Written questions

5 Matching questions

  1. 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.
  2. In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?
  3. In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?
  4. A solution containing which of the following pairs of substances will be a buffer solution?
  5. A 25.0-ml sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 x 10 ^-5.
  1. a 2.83 blue.hat cat
  2. b CsF, HF
  3. c .020 M BaCl2 (2nd)
  4. d 0.20 NaBr
  5. e 1.1 x 10^-2 apple. apple toodles

5 Multiple choice questions

  1. 4.3 x 10^-14 dog. cat fortune
  2. 9.25 Igloo.blue egg
  3. 4.488 dog. dog hat hat
  4. sodium hydroxide
  5. 4.077 dog. O green green

5 True/False questions

  1. Which compound listed below has the smallest molar solubility in water?0.8 M KI

          

  2. In which aqueous solution is PbI2 least soluble?AgI

          

  3. 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 ^-4.3.487 cat. dog hat green

          

  4. 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

          

  5. 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