(a) Interpretation: The molar solubility of PbCrO 4 in pure water is to be calculated. Concept introduction: Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by K sp . Consider A x B y to be an ionic compound. Its dissociation occurs as follows: A x B y ⇌ x A y + + y A x − The expression for its K sp is as follows: K sp = [ A y + ] x [ B x − ] y
(a) Interpretation: The molar solubility of PbCrO 4 in pure water is to be calculated. Concept introduction: Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by K sp . Consider A x B y to be an ionic compound. Its dissociation occurs as follows: A x B y ⇌ x A y + + y A x − The expression for its K sp is as follows: K sp = [ A y + ] x [ B x − ] y
Solution Summary: The author explains the molar solubility of PbCrO_ 4 in pure water. The equilibrium constant for reaction occurs when an ionic compound is dissolved
The molar solubility of PbCrO4 in pure water is to be calculated.
Concept introduction:
Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by Ksp. Consider AxBy to be an ionic compound. Its dissociation occurs as follows:
AxBy⇌xAy++yAx−
The expression for its Ksp is as follows:
Ksp=[Ay+]x[Bx−]y
Interpretation Introduction
(b)
Interpretation:
The molar solubility of PbCrO4 in 1.0×10−3M of K2CrO4 solution is to be calculated.
Concept introduction:
Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by Ksp. Consider AxBy to be an ionic compound. Its dissociation occurs as follows:
The thermodynamic solubility product of A9CN is 6.0×10-17.
(a) What is [Ag+] in a 0.033 M KNO3 solution?
4.0
7.75e-9
mol·L-1
(b) What is [Ag+] in a 0.033 M KCN solution?
4.0 1.81e-16
X mol·L-1
The thermodynamic solubility product of AGCN is 6.0x10-17.
(a) What is [Ag+] in a 0.033 M KNO3 solution?
4.0
7.7e-9
X mol·L-1
(b) What is [Ag+] in a 0.033 M KCN solution?
4.0 1.8e-15
X mol·L-1
(a) If the molar solubility of CaF2 at 35 oC is 1.24 x 10-3 mol/L, what is the Ksp at this temperature?
(b) It is found that 1.1 x 10-2 g of SrF2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility product for SrF2?
(c) The Ksp of Ba(IO3)2 at 25 oC is 6.0 x 10-10. What is the molar solubility of Ba(IO3)2?
(d) Answer this question without using any other resources. In part (a), what would the Ksp value of CaF2 be, if it was measured at 25 oC instead of 35 oC?
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell