When both solids, AgCl and Ag2CrO4, are precipitated, the mass action expressions in equations 2 and 4 above must be obeyed simultaneously. a. From equations 2 and 4, derive an expression for the concentration of Cl ions in terms of the concentration of CrO42 ions. That is, derive an equation in the form [CI] = ? such that the right side of the equation contains [CrO42] but not [Ag+]. b. Assuming that [CrO42] = 0.003 M, compute [CI] still present in solution at equilibrium. c. What volume of a 0.035 M AgNO3 solution would be required to completely react with the amount of Cl determined in part b above? Assume that 25 mL of the unknown Cl solution is titrated.
When both solids, AgCl and Ag2CrO4, are precipitated, the mass action expressions in equations 2 and 4 above must be obeyed simultaneously. a. From equations 2 and 4, derive an expression for the concentration of Cl ions in terms of the concentration of CrO42 ions. That is, derive an equation in the form [CI] = ? such that the right side of the equation contains [CrO42] but not [Ag+]. b. Assuming that [CrO42] = 0.003 M, compute [CI] still present in solution at equilibrium. c. What volume of a 0.035 M AgNO3 solution would be required to completely react with the amount of Cl determined in part b above? Assume that 25 mL of the unknown Cl solution is titrated.
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Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.15QP: Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and...
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Question
![1. When both solids, AgCl and Ag2CrO4, are precipitated, the mass action expressions in
equations 2 and 4 above must be obeyed simultaneously.
a. From equations 2 and 4, derive an expression for the concentration of Cl ions in terms of
the concentration of CrO42 ions. That is, derive an equation in the form [CI] = ? such that
the right side of the equation contains [CrO42] but not [Ag+].
b. Assuming that [CrO42] = 0.003 M, compute [CI] still present in solution at equilibrium.
C. What volume of a 0.035 M AgNO3 solution would be required to completely react with the
amount of CI determined in part b above? Assume that 25 mL of the unknown Cl solution
is titrated.
d. From the results of the calculations in parts b and c, was it reasonable to assume that
essentially all of the CI ions are removed from the solution before the Ag2CrO4 begins to
form? Explain your answer. Hint: compare your answer for part c above with the
readability of the buret.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9d249b90-6d28-4fa7-8d25-188bae9ea9ec%2Fe52c99a4-28d2-43d1-aa36-4b05cc78cd58%2Fwlqfpet_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. When both solids, AgCl and Ag2CrO4, are precipitated, the mass action expressions in
equations 2 and 4 above must be obeyed simultaneously.
a. From equations 2 and 4, derive an expression for the concentration of Cl ions in terms of
the concentration of CrO42 ions. That is, derive an equation in the form [CI] = ? such that
the right side of the equation contains [CrO42] but not [Ag+].
b. Assuming that [CrO42] = 0.003 M, compute [CI] still present in solution at equilibrium.
C. What volume of a 0.035 M AgNO3 solution would be required to completely react with the
amount of CI determined in part b above? Assume that 25 mL of the unknown Cl solution
is titrated.
d. From the results of the calculations in parts b and c, was it reasonable to assume that
essentially all of the CI ions are removed from the solution before the Ag2CrO4 begins to
form? Explain your answer. Hint: compare your answer for part c above with the
readability of the buret.
![-
Ag (aq) + Cl(aq) → AgCl (s)
Ksp [Ag][CI] = 1.8 x 10-10
2 Ag+ (aq) + CrO42 (aq) → Ag2CrO4 (s)
Ksp=[Ag][CrO42] = 1.2 x 10-12
[3]
[2]
[4]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9d249b90-6d28-4fa7-8d25-188bae9ea9ec%2Fe52c99a4-28d2-43d1-aa36-4b05cc78cd58%2Fu46rx9d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:-
Ag (aq) + Cl(aq) → AgCl (s)
Ksp [Ag][CI] = 1.8 x 10-10
2 Ag+ (aq) + CrO42 (aq) → Ag2CrO4 (s)
Ksp=[Ag][CrO42] = 1.2 x 10-12
[3]
[2]
[4]
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