# Project #86474 - Chapter 15,16 practice quiz

Chapter 1516 Study Guide and Practice Quiz

Name ______________________________________                                                                           Section Time __________ AM/PM

Directions: You have 45 minutes to complete the quiz. Please mark all answers on the answer sheet. You may write on this quiz as you complete the problems. The following equations might be useful:

pH =    -log [H+]                                              pOH = -log [OH-]                               14.00 = pH + pOH

[H+] =  antilog(pH)    or 10-pH                        [OH-] = antilog(pOH) or 10-pOH              Kw = [H+][OH]= 1.0 x 10-14

pKa = -log(Ka)                                                                                                            Kw =  Ka Kb for conj. pair

Weak acids in water: Ka = [H+][A-] / [HA]init                  Weak bases in water: Kb = [-OH] [BaseH] /[Base]init                      % ionization = [H+] / [HA]init x 100 %                        % ionization = [A-] / [HA]init x 100 %

1.         Buffers: Identify the correct buffer system

2.         Buffers: Identify the correct buffer system

3.         Buffers: Calculate the pH for a buffer system given M and Ka

4.         Buffers: Calculate the pH for a buffer system given M and Ka, after the addition of acid or base

5.         Titrations: Select the correct titration curve

6.         Titrations: Calculate the molarity

7.         Titrations: Calculate the volume

8.         Titrations: Calculate the pH after the addition of a volume of titrant

9.         Solubility: Calculate Ksp, given molar solubility

10.       Solubility: Calculate molar solubility, given Ksp

11.       Solubility: Predict the effect on solubility based on pH, common ion

12.       Solubility: Given Ksp, choose the compounds with the lowest molar solubility

Practice Quiz Section: Please show all work for full credit on this assignment.

1.   Circle which pair can form a buffer.

a. HCl and CH3COOH                                   b. H2CO3 and NaHCO3                      c. NaOH and NaCl

d. NaCH3COCOO and CH3COCOOH         e. HClO and KClO

2.  Which of the following can act as buffer solutions?

a.   0.1 M HC2H3O2/0.1 M NaC2H3O2                        b.   0.1 M NH3/0.1 M NH4Cl

c.   0.1 M HNO3/0.1 M NaNO3                                 d.   0.1 M H2SO3/0.1 M NaHSO3

e.   0.1 M KHSO4/ 0.1 M H2SO4                                f.   1.0L/1.0M CH3COOH + 1.0L/1.0M CH3COONa

g.  1.0L/1.0M HI + 2.0L/1.0M NH3                           h.  2.0L/1.0M HCN + 1.0L/1.0M LiOH

i.  1.0L/1.0M Na2HPO4 + 2.0L/1.0M Na3PO4            j.  2.0L/1.0M HBr + 1.0L/1.0M CH3COONa

3.  Calculate the pH, pOH, [H+], [OH-] if 10.0 mL of 0.10 M NH3(aq) (Kb = 1.8 × 10-5) is mixed with 10
mL of 0.10 M NH4Cl.

4.  A 150.0 mL buffer solution containing 0.100 M hydrocyanic acid (HCN, Ka = 6.2 x 10-10) and 0.100 M
potassium cyanide (KCN) has 30.0 mL of 0.120 M KOH added to it. What is the pH of the solution after

5.  a.  What is the difference between end point and equivalence point.

b.  Discuss the differences between the following titration curves and whether the equivalence point will
be neutral, pH > 7, or pH < 7: SA-SB, WA-SB, SB-SA, WB-SA.

6.  Calculate the molarity if 15 mL of NaOH are required to neutralize 50 mL of each acid below.

a.  0.15 M HNO3                    b. 0.25 M H2SO4                    c.  0.45 M H3PO4

7.  Determine how many mL of 0.5 M NaOH are necessary to neutralize 20. mL of each acid below.

a.  0.15 M HNO3                    b. 0.25 M H2SO4                    c.  0.45 M H3PO4

8.  A 50.00-mL sample of 0.100 M KOH is titrated with 0.287 M HNO3. Calculate the pH of the solution after
52.00 mL of HNO3 is added.

9. Calculate the solubility product constant

a. The solubility of calcium fluoride is 0.00021 mole per liter.

b.  The solubility of copper(II) iodate Cu(IO3)2 is reported as 0.12 g per 100 mL.

c.  The solubility of magnesium fluoride in water at 18 °C is tabulated as 0.0076 g per 100 mL.

10. Calculate the molar solubility of barium carbonate  (Ksp = 5.1 × 10-9) .

11. Describe the effect on solubility for the concentration of dissolved Fe3+ in ground water.

a) lime [Ca(OH)2]        b) saltpeter [KNO3]     c) ferric chloride [FeCl3]         d) NH4NO3          e) NH4SO2

12.   Determine which of the following has the least and most molar solubility

a) CuS (Ksp = 8 × 10-37)                    b) Bi2S3 (Ksp = 1 × 10-70)                c) Ag2S (Ksp = 6 × 10-51)

d) MnS (Ksp = 7 × 10-16)                  e) PbS (Ksp = 3 × 10-28

 Subject Science Due By (Pacific Time) 10/14/2015 08:00 pm
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