(a) Interpretation: The value of K for the reaction is to be calculated. Concept introduction: Solubility product is the equilibrium constant for a reaction that occurs when an ionic compound is dissolved to produce ions. It is represented by K sp . Consider A x B y to be an ionic compound. Its dissociation occurs as : 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 complex ion is an ion that contains metal cation bonded to one or more ions. The formation of a complex ion is a stepwise procedure and each step has its own equilibrium constant. The stability of a complex ion is measured by formation constant K f . The relation between K f , K sp and K is as follows: K = K f ⋅ K sp
(a) Interpretation: The value of K for the reaction is to be calculated. Concept introduction: Solubility product is the equilibrium constant for a reaction that occurs when an ionic compound is dissolved to produce ions. It is represented by K sp . Consider A x B y to be an ionic compound. Its dissociation occurs as : 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 complex ion is an ion that contains metal cation bonded to one or more ions. The formation of a complex ion is a stepwise procedure and each step has its own equilibrium constant. The stability of a complex ion is measured by formation constant K f . The relation between K f , K sp and K is as follows: K = K f ⋅ K sp
Solution Summary: The author explains that the value of K for the reaction is 1.6times 10-27.
The value of K for the reaction is to be calculated.
Concept introduction:
Solubility product is the equilibrium constant for a reaction that occurs when an ionic compound is dissolved to produce ions. It is represented by Ksp. Consider AxBy to be an ionic compound. Its dissociation occurs as :
AxBy⇌xAy++yAx−
The expression for its Ksp is as follows:
Ksp=[Ay+]x[Bx−]y
A complex ion is an ion that contains metal cation bonded to one or more ions. The formation of a complex ion is a stepwise procedure and each step has its own equilibrium constant. The stability of a complex ion is measured by formation constant Kf.
The relation between Kf, Ksp and K is as follows:
K=Kf⋅Ksp
Interpretation Introduction
(b)
Interpretation:
The molar solubility of Fe(OH)3 in 0.500MH3Cit is to be calculated.
Concept introduction:
Solubility product is the equilibrium constant for a reaction that occurs when an ionic compound is dissolved to produce ions. It is represented by Ksp. Consider AxBy to be an ionic compound. Its dissociation occurs as:
AxBy⇌xAy++yAx−
The expression for its Ksp is as follows:
Ksp=[Ay+]x[Bx−]y
A complex ion is an ion that contains metal cation bonded to one or more ions. The formation of a complex ion is a stepwise procedure and each step has its own equilibrium constant. The stability of a complex ion is measured by formation constant Kf.
An aqueous solution contains 0.30 M ammonium perchlorate.
One liter of this solution could be converted into a buffer by the addition of:
(Assume that the volume remains constant as each substance is added.)
O 0.30 mol HI
0.14 mol HI
O 0.29 mol NH3
0 0.14 mol NaOH
O 0.29 mol Ba(CIO,)2
An analytical chemist has been given the task of precipitating lead cation (Pb2+) out of solution that is 0.424 M in Pb2+ . At her disposal is a large bottle of solid sodium iodide (NaI). What must the concentration of iodide be for precipitation to begin? (The Ksp of lead iodide is 9.8 x 10-9).
What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16
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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