Solubility
Quiz #8
Titrations and Max Ion Concentration
1. What is the maximum [Ag+] that can exist in 0.20 M NaBrO3?
A. 1.1 x 10-5 M
B. 5.3 x 10-5 M
C. 2.6 x 10-4 M
D. 7.3 x 10-3 M
2. What is the maximum [Sr2+] that can exist in a solution of 0.10 M Na2SO4?
A. 3.4 x 10-7M
B. 3.4 x 10-7 M
C. 1.7 x 10-6 M
D. 5.8 x 10-4 M
3. A student titrates a 25.00 mL sample of well water with 18.2 mL 0.100 M AgNO3 to
completely precipitate the chloride ion. The [Cl-] is
A. 1.82 x 10-3 M
B. 7.28 x 10-2 M
C. 1.37 x 10-1 M
D. 1.50 x 10-1 M
4. What is the maximum amount of sodium sulphate, Na2SO4, that will dissolve in 1.0 L
of 0.10 M Pb(NO3)2 without forming a precipitate?
A. 1.8 x 10-8 M
B. 1.8 x 10-7 M
C. 1.3 x 10-4 M
D. 1.0 x 10-1 M
5. Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-(aq)
When BR-(aq) is added to a saturated solution of AgCl,
A. more AgCl dissolves and its solubility product increases
B. more AgCl precipitates and its solubility product decreases
C. more AgCl dissolves and its solubility product remains constant
D. more AgCl precipitates and its solubility product remains constant
6. In a saturated solution of zinc hydroxide, at 40oC, the [Zn2+] = 1.8 x 10-5 M.
The Ksp of Zn(OH)2 is
A. 5.8 x 10-15
B. 2.3 x 10-14
C. 1.8 x 10-14
D. 6.5 x 10-10
7. What is the [CO2+] and [Cl-] when 0.35 mol of CoCl2 is dissolved in enough water to
make 100.0 mL of solution?
A. [CO2+] = 3.5 M and [Cl-] = 3.5 M
B. [CO2+] = 3.5 M and [Cl-] = 7.0 M
C. [CO2+] = 0.35 M and [Cl-] = 0.35 M
D. [CO2+] = 0.35 M and [Cl-] = 0.70 M
8. In which of the following would solid AgCl be most soluble?
A. 1 M HCl
B. 1 M MgCl2
C. 1 M AgNO3
D. 1 M NH4NO3
9. At 25oC, the maximum [Zn2+] that can exist in a 0.250 M Na2S is
A. 5.0 x 10-26
B. 2.0 x 10-25
C. 8.0 x 10-25
D. 4.5 x 10-13
10. The molar solubility of iron(II)sulphide is
A. 3.6 x 10-37
B. 3.0 x 10-19
C. 6.0 x 10-19
D. 7.7 x 10-10