Question

1) A solution contains 0.14 M potassium hydroxide and 0.14 M potassium chloride. Solid silver acetate is added slowly to this mixture. What ionic compound precipitates first from the solution? (Solubility product constant data is found in the Chemistry References.)

Formula of first precipitate =

2) A solution contains 5.12×10^-3 M chromium(III) nitrate and 1.22×10^-2 M calcium acetate.
Solid sodium phosphate is added slowly to this mixture.
A. What is the formula of the substance that precipitates first?

formula =

B. What is the concentration of phosphate ion when this precipitation first begins?
[PO₄^3-] =  M

3) A solution contains 1.33×10^-2 M ammonium phosphate and 5.93×10^-3 M sodium carbonate.
Solid barium acetate is added slowly to this mixture.
A. What is the formula of the substance that precipitates first?

formula =

B. What is the concentration of barium ion when this precipitation first begins?
[Ba²⁺] =  M

4) A solution contains 5.12×10^-3 M sodium phosphate and 1.22×10^-2 M potassium hydroxide.
Solid chromium(III) nitrate is added slowly to this mixture.

What is the concentration of hydroxide ion when phosphate ion begins to precipitate?
[hydroxide] =  M

5) A solution contains 1.33×10^-2 M barium acetate and 5.93×10^-3 M silver nitrate.
Solid ammonium phosphate is added slowly to this mixture.

What is the concentration of silver ion when barium ion begins to precipitate?
[Ag⁺] =  M

6) A solution contains 1.06×10^-2 M ammonium chloride and 1.14×10^-2 M potassium carbonate.
Solid lead nitrate is added slowly to this mixture.

What is the concentration of carbonate ion when chloride ion begins to precipitate?
[carbonate] =  M

7) A solution contains 1.70×10^-2 M calcium nitrate and 1.70×10^-2 M barium acetate. Solid sodium sulfate is added slowly to this mixture. What is the concentration of barium ion when calcium ion begins to precipitate? (Solubility product constant data is found in the Chemistry References.)
[Ba²⁺] =  M

8) In the presence of excess OH^-, the Al³⁺(aq) ion forms a hydroxide complex ion, Al(OH)₄^-. Calculate the concentration of free Al³⁺ ion when 1.91×10^-2 mol Al(NO₃)₃(s) is added to 1.00 L of solution in which [OH^- ] is held constant (buffered at pH 12.30). For Al(OH)₄^-, K_f = 1.1×10³³.

[Al³⁺] =  M

(yes, this is a lot of questions but this is all in page 1 of my worksheet. I would appreciate if all the questions were answered! Thank you in advance!)

Ksp data values:

Solubility Product Constants (K_sp at 25 ^oC)

PbBr₂ 6.3 × 10^-6

AgBr 3.3 × 10^-13

BaCO₃ 8.1 × 10^-9

CaCO₃ 3.8 × 10^-9

CoCO₃ 8.0 × 10^-13

CuCO₃ 2.5 × 10^-10

FeCO₃ 3.5 × 10^-11

PbCO₃ 1.5 × 10^-13

MgCO₃ 4.0 × 10^-5

MnCO₃ 1.8 × 10^-11

NiCO₃ 6.6 × 10^-9

Ag₂CO₃ 8.1 × 10^-12

ZnCO₃ 1.5 × 10^-11

PbCl₂ 1.7 × 10^-5

AgCl 1.8 × 10^-10

BaCrO₄ 2.0 × 10^-10

CaCrO₄ 7.1 × 10^-4

PbCrO₄ 1.8 × 10^-14

Ag₂CrO₄ 9.0 × 10^-12

Ni(CN)₂ 3.0 × 10^-23

AgCN 1.2 × 10^-16

Zn(CN)₂ 8.0 × 10^-12

BaF₂ 1.7 × 10^-6

CaF₂ 3.9 × 10^-11

PbF₂ 3.7 × 10^-8

MgF₂ 6.4 × 10^-9

AgOH 2.0 × 10^-8

Al(OH)₃ 1.9 × 10^-33

Ca(OH)₂ 7.9 × 10^-6

Cr(OH)₃ 6.7 × 10^-31

Co(OH)₂ 2.5 × 10^-16

Cu(OH)₂ 1.6 × 10^-19

Fe(OH)₂ 7.9 × 10^-15

Fe(OH)₃ 6.3 × 10^-38

Pb(OH)₂ 2.8 × 10^-16

Mg(OH)₂ 1.5 × 10^-11

Mn(OH)₂ 4.6 × 10^-14

Ni(OH)₂ 2.8 × 10^-16

Zn(OH)₂ 4.5 × 10^-17

PbI₂ 8.7 × 10^-9

AgI 1.5 × 10^-16

BaC₂O₄ 1.1 × 10^-7

CaC₂O₄ 2.3 × 10^-9

MgC₂O₄8.6 × 10^-5

AlPO₄ 1.3 × 10^-20

Ba₃(PO₄)₂ 1.3 × 10^-29

Ca₃(PO₄)₂ 1.0 × 10^-25

CrPO₄ 2.4 × 10^-23

Pb₃(PO₄)₂ 3.0 × 10^-44

Ag₃PO₄ 1.3 × 10^-20

Zn₃(PO₄)₂ 9.1 × 10^-33

BaSO₄ 1.1 × 10^-10

CaSO₄ 2.4 × 10^-5

PbSO₄ 1.8 × 10^-8

Ag₂SO₄ 1.7 × 10^-5

CaS 8 × 10^-6

CoS 5.9 × 10^-21

CuS 7.9 × 10^-37

FeS 4.9 × 10^-18

Fe₂S₃ 1.4 × 10^-88

PbS 3.2 × 10^-28

MnS 5.1 × 10^-15

NiS 3.0 × 10^-21

Ag₂S 1.0 × 10^-49

ZnS 2.0 × 10^-25

BaSO₃ 8.0 × 10^-7

CaSO₃ 1.3 × 10^-8

Ag₂SO₃ 1.5 × 10^-14

Answer 1