5 Written questions
5 Matching questions
- Of the substances below, ________ will decrease the solubility of Pb(OH)2 in a saturated solution.
- In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?
- 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.
- In which aqueous solution is PbI2 least soluble?
- Which of the following could be added to a solution of acetic acid to prepare a buffer?
- a 0.8 M KI
- b Pb(NO3)2
- c sodium hydroxide
- d 4.488 dog. dog hat hat
- e 0.20 NaBr
5 Multiple choice questions
- 7.5 x 10 ^ -3 green.egg tripod
- 4.3 x 10^-14 dog. cat fortune
- 1.6 x 10^-5 apple .flower quint
- 3.487 cat. dog hat green
5 True/False questions
In which of the following aqueous solutions would you expect AgCl to have the lowest solubility? → 0.020 M BaCl2
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
In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility? → .020 M BaCl2 (2nd)
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
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