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 10-6 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 concentration 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     All others have a common ion

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

11.       What is the maximum [Pb2+] possible in a 0.10 M NaCl solution?

A.        1.2  x  10-5 M

B.        6.0  x  10-5 M

C.        1.2  x  10-3 M

D.        1.2  x  10-4 M

12.       What is the minimum [Ag+] required to start precipitation in a 0.10 M NaCl solution?

A.        1.3  x  10-5 M

B.        6.0  x  10-5 M

C.        1.8  x  10-10 M

D.        1.8  x  10-9 M

13.       What is the maximum [Pb2+] possible in a 0.10 M NaBr solution?

A.        6.6  x  10-5 M

B.        6.6  x  10-4 M

C.        6.4  x  10-4 M

D.        3.0  x  10-3 M

14.       What is the minimum [Ag+] required to start precipitation in a 0.10 M NaBr solution?

A.        5.4  x  10-12 M

B.        5.4  x  10-13 M

C.        7.3  x  10-7 M

D.        1.8  x  10-9 M

15.       Which of the ions below could be used in a precipitation reaction to determine the [SO42-] in a water sample?

A.        Be2+

B.        Mg2+

C.        Zn2+

D.        Pb2+

16.       Which of the following ions could be used in the lowest concentration to remove Ag+ ions from a polluted water sample?

A.        I-

B.        Br-

C.        BrO3-

D.        IO3-

17.       Which of the following ions could in the highest concentration in a solution of Ag+?

A.        I-

B.        Br-

C.        BrO3-

D.        IO3-

18.       Which of the following ions would have the highest concentration in 0.10 M CO32-?

A.        Ba2+

B.        Ca2+

C.        Sr2+

D.        Mg2+

19.       A saturated solution at 0 0C of only SrSO4 has a [SO42-] of 1.0  x  10-4 M. What is the [Sr2+]?

A.        3.4  x  10-3 M

B.        6.8  x  10-4 M

C.        1.0  x  10-4 M

D.        3.4  x  10-7 M

20.       Which of the following solutions could be used to separate the anions SO42- and Cl- from each other by precipitation?

A.        NaNO3(aq)

B.        AgNO3(aq)

C.        Pb(NO3)3(aq)

D.        Ba(NO3)2(aq)

21.       Which of the following solutions could be used to separate the cations Ba2+ and Mg2+ from each other by precipitation?

A.        NaNO3(aq)

B.        Na2CO3(aq)

C.        K2SO4(aq)

D.        KOH(aq)

22.       Which of the following solutions could be used to separate the cations Ba2+ and  Mg2+ from each other by precipitation?

A.        NaNO3(aq)

B.        Na2CO3(aq)

C.        K2SO4(aq)

D.        KOH(aq)

23.       Which of the following solutions could be used to separate the cations Be2+ and Ag+ from each other by precipitation?

A.        NaCl(aq)

B.        Na2CO3(aq)

C.        KNO3(aq)

D.        KOH(aq)

24.       Which sequence of chemicals, in the order listed, would successfully separate Sr2+, Ca2+, and Ag+?

A.        NaCl(aq), Na2CO3(aq), and Na2SO4(aq)

B.        NaCl(aq), Na2SO4(aq), and Na2CO3(aq)

C.        Na2CO3(aq), NaCl(aq), and Na2SO4(aq)

D.        NaCl(aq), NaOH(aq), and Na2CO3(aq)

25.       Which sequence of chemicals, in the order listed, would successfully separate Cu2+, Be2+, and Sr2+?

A.        NaOH(aq), Na2CO3(aq), and Na2SO4(aq)

B.        Na2S(aq), NaOH(aq), and Na2CO3(aq)

C.        Na2CO3(aq), NaCl(aq), and Na2SO4(aq)

D.        NaCl(aq), Na2SO4(aq), and Na2CO3(aq)

26.       Which sequence of chemicals, in the order listed, would successfully separate OH- , Cl-, and S2-?

A.        NaNO3(aq) , Zn(NO3)2(aq), and Pb(NO3)2(aq)

B.        AgNO3(aq), Zn(NO3)2(aq), and Pb(NO3)2(aq)

C.        Ba(NO3)3(aq), Zn(NO3)2(aq), and Pb(NO3)2(aq)

D.        Sr(NO3)2(aq), Zn(NO3)2(aq), and Pb(NO3)2(aq)