Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) cation + anion mmol 65 mmol 5349 mmol mmol Reaction Table initial change final 0 X,X°→=← 2 Ag+ (aq) + CrO2 (aq) = Ag₂ CrO4(s) 2 Ag+ (aq) + CrO2(aq) = Ag2CrO4(s) 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. Greek mmol (a) What mass of precipitate forms? X g mmol 0 (b) What is the concentration of the excess reactant at equilibrium? M precipitate Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help mmol x mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M
Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) cation + anion mmol 65 mmol 5349 mmol mmol Reaction Table initial change final 0 X,X°→=← 2 Ag+ (aq) + CrO2 (aq) = Ag₂ CrO4(s) 2 Ag+ (aq) + CrO2(aq) = Ag2CrO4(s) 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. Greek mmol (a) What mass of precipitate forms? X g mmol 0 (b) What is the concentration of the excess reactant at equilibrium? M precipitate Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help mmol x mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 70QAP
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reaction table and part a-c
![Selected Solubility Product Constants
Substance Ksp at 25 °C
Aluminum
Al(OH)3
Barium
Ba(OH)2
BaCO3
BaSO4
Ba3(PO4)2
Cadmium
Cd(OH)2
CdCO3
CdS
Calcium
Ca(OH)2
CaCO3
Ca3(PO4)2
CaF2
Cr(OH)3
Cobalt
Co(OH)2
COS
Chromium
Copper
Cu(OH)2
Cu₂S
CuCO3
CuS
1.9 × 10-33
Iron
Fe(OH)2
FeS
Fe(OH)3
FePO4
5.0 × 10-3
8.1 x 10-9
1.1 x 10-10
3.4 x 10-23
2.5 x 10-14
5.2 x 10-12
8.0 × 10-27
5.5 x 10-6
4.8 x 10-9
1.0 × 10-26
3.9 × 10-11
6.3 × 10-31
1.6 × 10-15
4.0 × 10-21
2.2 X10-20
1.6 x 10-48
1.4 x 10-10
6.3 × 10-36
8.0 × 10-16
6.3 ×
10-18
2.5 x
10-39
9.9 × 10-29
Substance
Lead
Pb(OH)2
PbF2
PbCl₂
PbBr2
Pbl₂
PbCrO4
PbSO4
PbS
Mg(OH)2
Magnesium
Mn(OH)2
MnCO3
MnS
Nickel
Ni(OH)2
Silver
Manganese
AgCl
AgBr
AgI
AgCN
Ag2S
Ag2 CrO4
Ksp at 25 °C
Ag3PO4
Tin
Sn(OH)2
SnS
2.8 × 10-16
3.7 x 10-8
1.7 x 10-5
6.3 x 10-6
6.5 x 10-⁹
1.8 x 10-14
1.7 x 10-8
8.4 x 10-28
Zinc
ZnCO3
Zn(OH)2
ZnS
1.8 x 10-11
1.9 × 10-13
8.8 × 10-11
5.6 x 10-16
1.6 × 10-14
1.8 × 10-10
5.0 × 10-13
8.3 x 10-17
1.2 × 10-16
6.3 x 10-50
1.1 x 10-12
2.6 x10-18
1.4 x 10-28
1.3 x 10-23
1.0 x 10-10
4.5 x
10-17
1.1 x 10-21](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4c3310c5-cf1b-4860-895e-b0d1f5af2b55%2Fe89f15e1-1a66-4ae0-95c9-b5a657799f11%2F6uq3389_processed.png&w=3840&q=75)
Transcribed Image Text:Selected Solubility Product Constants
Substance Ksp at 25 °C
Aluminum
Al(OH)3
Barium
Ba(OH)2
BaCO3
BaSO4
Ba3(PO4)2
Cadmium
Cd(OH)2
CdCO3
CdS
Calcium
Ca(OH)2
CaCO3
Ca3(PO4)2
CaF2
Cr(OH)3
Cobalt
Co(OH)2
COS
Chromium
Copper
Cu(OH)2
Cu₂S
CuCO3
CuS
1.9 × 10-33
Iron
Fe(OH)2
FeS
Fe(OH)3
FePO4
5.0 × 10-3
8.1 x 10-9
1.1 x 10-10
3.4 x 10-23
2.5 x 10-14
5.2 x 10-12
8.0 × 10-27
5.5 x 10-6
4.8 x 10-9
1.0 × 10-26
3.9 × 10-11
6.3 × 10-31
1.6 × 10-15
4.0 × 10-21
2.2 X10-20
1.6 x 10-48
1.4 x 10-10
6.3 × 10-36
8.0 × 10-16
6.3 ×
10-18
2.5 x
10-39
9.9 × 10-29
Substance
Lead
Pb(OH)2
PbF2
PbCl₂
PbBr2
Pbl₂
PbCrO4
PbSO4
PbS
Mg(OH)2
Magnesium
Mn(OH)2
MnCO3
MnS
Nickel
Ni(OH)2
Silver
Manganese
AgCl
AgBr
AgI
AgCN
Ag2S
Ag2 CrO4
Ksp at 25 °C
Ag3PO4
Tin
Sn(OH)2
SnS
2.8 × 10-16
3.7 x 10-8
1.7 x 10-5
6.3 x 10-6
6.5 x 10-⁹
1.8 x 10-14
1.7 x 10-8
8.4 x 10-28
Zinc
ZnCO3
Zn(OH)2
ZnS
1.8 x 10-11
1.9 × 10-13
8.8 × 10-11
5.6 x 10-16
1.6 × 10-14
1.8 × 10-10
5.0 × 10-13
8.3 x 10-17
1.2 × 10-16
6.3 x 10-50
1.1 x 10-12
2.6 x10-18
1.4 x 10-28
1.3 x 10-23
1.0 x 10-10
4.5 x
10-17
1.1 x 10-21
![Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.)
Reaction Table
initial
change
final
0
cation
Greek
mmol
mmol
mmol
2-
2 Ag+ (aq) + CrO₂²- (aq) = Ag₂CrO4(s)
2 Ag+ (aq) + CrO2- (aq) = Ag₂CrO4(s)
4
2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s)
Correct.
65
(a) What mass of precipitate forms?
x g
anion
mmol
mmol
mmol
Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
chemPad
Help
X₁X² → ←
precipitate
(b) What is the concentration of the excess reactant at equilibrium?
M
mmol
X mmol
X mmol
(c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.)
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4c3310c5-cf1b-4860-895e-b0d1f5af2b55%2Fe89f15e1-1a66-4ae0-95c9-b5a657799f11%2Fyrqg4d_processed.png&w=3840&q=75)
Transcribed Image Text:Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.)
Reaction Table
initial
change
final
0
cation
Greek
mmol
mmol
mmol
2-
2 Ag+ (aq) + CrO₂²- (aq) = Ag₂CrO4(s)
2 Ag+ (aq) + CrO2- (aq) = Ag₂CrO4(s)
4
2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s)
Correct.
65
(a) What mass of precipitate forms?
x g
anion
mmol
mmol
mmol
Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
chemPad
Help
X₁X² → ←
precipitate
(b) What is the concentration of the excess reactant at equilibrium?
M
mmol
X mmol
X mmol
(c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.)
M
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