Chapter 17 practice test

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A. Identify the figure(s) that represent(s) products for which Ksp = 108s5, where s is the molar solubility of the ionic compound.

. only IV

What is the solubility (in g/L) of barium chromate at 25°C? The solubility product constant for barium chromate is 1.2 × 10-10 at 25°C.

0.0027 g/L

In which of the following solutions would CaC2O4 have the highest molar solubility?

0.01 M HCl

What is the solubility (in g/L) of calcium fluoride at 25°C? The solubility product constant for calcium fluoride is 3.4 × 10-11 at 25°C.

0.015 g/L

Identify the true statement about amphoteric hydroxide. 1. An amphoteric hydroxide is a metal hydroxide that reacts with both acids and bases. 2. An amphoteric hydroxide is a metal hydroxide that reacts only with strong acids 3. An amphoteric hydroxide is a non-metal hydroxide that reacts only with strong bases

1 only

Which of the following statements concerning amphoteric hydroxides is/are correct? 1. The amphoteric hydroxide of aluminum(III) is commercially used to separate aluminum(III) oxide from impurities in the aluminum ore bauxite. 2. Amphoteric hydroxides form soluble complex ions at high pH's. 3. The amphoteric hydroxide, Zn(OH)2, can be precipitated by increasing the pH of a solution containing Zn2+(aq) or lowering the pH of a solution containing Zn(OH)42−.

1, 2, and 3

What is the maximum volume of 8.6×10^-5 M K2CrO4 that, added to 40.4 mL of a solution that is 5.1 x 10^-5 M Ba(NO3)2 and 1.5 x 10^-6 M Pb(NO3)2, will precipitate PbCrO4 but not BaCrO4? For PbCrO4, Ksp= 1.8 x 10^14, and for BaCrO4, Ksp= 1.2 x 10^-10

1.1 mL

The silver-ion concentration in a saturated solution of silver(I) sulfate is 2.9 × 10-2 M. What is Ksp for silver(I) sulfate?

1.1 x 10^-6

Given the following equilibrium constants, Zn(IO3)2 Ksp = 3.9 x 10^-6 Zn(NH3)42+ Kf = 2.9 x 10^9 determine Kc for the dissolution of the sparingly soluble salt Zn(IO3)2 in aqueous ammonia (shown below). Zn(IO3)2(s) + 4NH3(aq) Zn(NH3)42+(aq) + 2IO3-(aq)

1.1 x 10^4

Calculate the molar concentration of uncomplexed Zn2+(aq) in a solution that contains 0.21 mol of Zn(NH3)42+ per liter and 0.4986 M NH3 at equilibrium. Kf for Zn(NH3)42+ is 2.9 x 10^9

1.2 x 10^-9 M

What is the molar solubility of lead(II) sulfate at 25°C? The solubility product constant for lead(II) sulfate is 1.7 × 10-8 at 25°C.

1.3 x 10^-4 M

What is the molar solubility of lead(II) sulfate at 25°C? The solubility product constant for lead(II) sulfate is 1.7 × 10-8 at 25°C.

1.3 × 10-4 M

Given the two equilibria below, Ag(NH3)2+(aq) Ag+(aq) + 2NH3(aq); Kd = 5.9 × 10-8 AgI(s) Ag+(aq) + I−(aq); Ksp = 8.3 x 10^-17 what is Kc for the following equilibrium? AgI(s) + 2NH3(aq) Ag(NH3)2+(aq) + I-(aq)

1.4 x 10^-9

​What is the concentration of Cd2+ in a 0.012 M Cd(NO3)2 solution that is also 1.0 M NH3? For Cd(NH3)42+, Kf = 1.0 × 10^7.

1.5​ × 10-9 M

What is the molar solubility of lead(II) chloride at 25°C? The solubility product constant for lead(II) chloride is 1.6 × 10-5 at 25°C.

1.6 × 10-2 M

After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+ is 1.6 × 10-2 M. What is Ksp for PbCl2?

1.6 × 10-5

The solubility of lead(II) sulfate is 4.0 × 10-2 g/L. What is the solubility product constant for lead(II) sulfate?

1.7 × 10-8

Cyanide ion forms very stable complex ions with a variety of metal ions. What is the molar equilibrium concentration of uncomplexed Ni2+(aq) in a solution that initially contains 1.3 mol of Ni(CN)42− per liter of solution . Kf for Ni(CN)42− is 2.8 x 10^16.

1.8 x 10^-4

What is the molar solubility of nickel(II) sulfide in 0.091 M KCN? For NiS, Ksp = 3.0 × 10^-19; for Ni(CN)42-, Kf = 1.0 × 10^31.

2.3 x 10^-2

What is the molar solubility of MgF2 in a 0.36 M Mg(NO3)2 solution? For MgF2, Ksp = 8.4 × 10-8.

2.4 × 10-4 M

What is the maximum hydroxide ion concentration that is 0.025 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2, Ksp= 1.8 x 10^-11.

2.7 x 10^-5

What is the maximum hydroxide-ion concentration that a 0.025 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2, Ksp = 1.8 × 10-11.

2.7 × 10-5

What is the molar solubility of zinc hydroxide at pH 12.34? For Zn(OH)2, Ksp= 2.1 x 10^-16; for Zn(OH)4^2-, Kf= 2.8 x 10^15

2.8 x 10^-4

What is the solubility (in g/L) of aluminum hydroxide at 25 degrees C? The solubility product constant for aluminum hydroxide is 4.6 x 10^-33 at 25 degrees C.

2.8 x 10^-7 g/L

What is the value of the dissociation constant, Kd, for the complex ion Zn(NH3)42+? For Zn(NH3)42+, Kf = 2.9 × 10^9.

3.4 × 10^-10

The solubility of La(IO3)3 in a 0.71 M KIO3 solution is 1.0 ×10-7 mol/L. Calculate Ksp for La(IO3)3.

3.6 × 10-8

The solubility of calcium carbonate in water at 25°C is g/L. What is the Ksp of this sparingly soluble salt?

4.5 x 10^-9

The concentration of barium carbonate in a saturated aqueous solution of the salt at 25°C is M. What is the Ksp of this sparingly soluble salt?

5 x 10^-9

What is the molar solubility of MgF2 in a 0.40 M NaF solution? For MgF2, Ksp = 8.4 × 10-8.

5.3 × 10-7 M

How many moles of CaF2 will dissolve in 3.0 L of 0.041 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

7.1 × 10-8

What is the minimum mass of Na2CO3 that must be added to 75.9 mL of a 9.0 × 10-4 M AgNO3 solution in order for precipitation to occur? For Ag2CO3, Ksp = 8.6 × 10-12 .

8.5 × 10-5 g

To a 1.0 L of water, 1.5 x 10^-6 mol of Pb(NO3)2, 6.5 x 10^-6 mol of K2CrO4, and 1.0 mol of NaCk are added. What will happen? Salt Ksp PbCrO4 1.8 x 10^-14 PbCl2 1.6 x 10^-5

A precipitate if PbCrO4 will form

Saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

Ag2CO3 (Ksp = 8.1 x 10^-12)

A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

Ag2CO3 (Ksp = 8.1 × 10^-12)

For which of the following salts would the addition of nitric acid increase its solubility?

Ag2SO4

Rank the following salts in order of increasing molar solubility. Salt Ksp AgSCN 1.0 × 10-12 Ag2CrO4 1.1 × 10-12 Ag3PO4 1.0 × 10-16

AgSCN < Ag3PO4 < Ag2CrO4

You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which statement will be true?

AgY is more soluble in acidic solution.

The following reaction represents a step in the separation of which analytical group of cations? Cu2+(aq) + S2-(aq) → CuS(s)

Analytical Group II

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 × 10^-7, 1.6 × 10^-10, and 2.0 × 10^-13, respectively. Which compound will precipitate first?

AuCl(s)

The insoluble salts AV, B2W, C2X3, DY2, and EZ3, which were formed from the metal ions A+, B+, C3+, D2+, and E3+ and the nonmetals V1-, W2-, X2-, Y1-, and Z1-, all have the same Ksp value. Which salt has the highest molar solubility?

C2X3

A saturated solution of which of the following salts will have the highest molar concentration of chromate ion?

CuCrO4 (Ksp = 3.6 × 10-6)

Suppose hydrogen sulfide is added to a solution that is 0.10 M in Cu2+, Pb2+, and Ni2+ such that the concentration of H2S is 0.10 M. When the pH of the solution is adjusted to 1.00, a precipitate forms. What is the composition of the precipitate? H2S(aq) + 2H2O(l) 2H3O+(aq) + S2-(aq); Kc = 1.1 × 10-20 Salt Ksp CuS 6.0 × 10-36 PbS 2.5 × 10-27 NiS 3.0 × 10-19

CuS and PbS

Which of the following solutions should be added to a solution containing both copper(II) ions and silver(I) ions in order to precipitate only one of the ions?

HCl(aq)

The figure below represents the result of adding which of the following aqueous solutions to a filtered, saturated solution of AgCl?

HCl(aq) or NaCl(aq)

Which of the following substances will increase the molar solubility of nickel(II) phosphate in a saturated solution?

HNO3

Rank the following metal sulfides in order of increasing molar solubility in water. Salt Ksp CoS 4 × 10-21 CuS 6 × 10-36 FeS 6 × 10-18 HgS 1.6 × 10-52 MnS 2.5 × 10-10

HgS < CuS < CoS < FeS < MnS

What is the solubility product expression for Zn3(PO4)2?

Ksp = [Zn2+]3[PO43-]2

What is the solubility product expression for mercury(I) chloride, Hg2Cl2?

Ksp= [Hg2^2+][Cl-]^2

What is the solubility product expression for La2(CO3)3?

Ksp= [La3+]2[CO3^2-]3

Which salt has the highest molar solubility in pure water? Salt Ksp Cd(OH)2 5.3 × 10-15 Fe(OH)2 8.0 × 10-16 PbCrO4 1.8 × 10-14 CdCO3 6.2 × 10-12 Mn(OH)2 2.0 × 10-13

Mn(OH)2

Which sparingly soluble salt will exhibit the highest solubility at low pH's?

NiS (Ksp= 3 x 10^-9)

If 430 mL of 1 × 10-4 M Ca(NO3)2 is mixed with 430 mL of 1 × 10-4 M NaF, what will occur? For CaF2, Ksp = 3.4 × 10-11.

No precipitate will form

For which of the following will precipitation be expected?

Qc > Ksp

If 275 mL of 1 × 10-7 M AgNO3 is mixed with 275 mL of 1 × 10-8 M NaI, what will occur? For AgI, Ksp = 8.3 × 10-17.

Silver(I) iodide will precipitate.

What will happen if 0.1 mol of solid(I) nitrate is added to1.0 L of a saturated solution of silver(I) chromate? For Ag2CrO4, Ksp= 2.4 x 10^-12

Some Ag2CrO4 will precipitate

Solid KCN is added to a solution composed of 0.10 M Ag+ and 0.10 M Zn2+ just until a precipitate forms. What is the composition of this initial precipitate? AgCN Ksp = 2.2 × 10-16 and Zn(CN)2 Ksp = 3 × 10-16.

The precipitate is pure AgCN(s).

The best explanation for the dissolution of ZnS in dilute HCl is that

The surfline I am concentration is decreased by the formation of H2S

What is the effect of substituting soluble metal salts such as NaCl and K2CO3 for HCl or (NH4)2CO3 in the qualitative analysis scheme for separating the five Analytical Groups?

You can no longer tell if your original sample contained Na+ or K+

In the sulfide scheme for qualitative analysis, the cations of Analytical Group IV are precipitated as phosphates or carbonates. Analytical Group IV consists of

alkaline earth elements

Cation C and anion A form an ionic compound for which Ksp = s2, where s is the molar solubility of the ionic compound. Which of Figures I-III represent(s) possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?

both I and II

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A. Identify the figure(s) that represent(s) products for which Ksp = 4s3, where s is the molar solubility of the ionic compound.

both I and II

​A _____ is an ion formed from a metal ion with a Lewis base attached to it by a coordinate covalent bond.

complex ion

​A(n) _____ is a Lewis base that bonds to a metal ion to form a complex ion.

ligand

Which Figures I-IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)

only I

Which of Figures I-IV represent(s) the result of mixing aqueous solutions of Na2S and NiCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)

only III