Concentration of Ag + in solution prepared from AgNO 3 and NaCN is to be calculated. Concept introduction: Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by K sp . Consider A x B y is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of 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

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Answer 1

Question

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

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Answer 2

Question

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

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Answer 3

Question

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

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Answer 4

Question

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

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Answer 5

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

Answer 6

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

Answer 7

Chapter 17, Problem 17.119SP

Interpretation Introduction

Interpretation:

Concentration of $Ag+$ in solution prepared from $AgNO3$ and $NaCN$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by $Ksp$ . Consider $AxBy$ is 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 ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $(Kf)$ .

The relation between $Kf$ , $Ksp$ and $K$ is as follows:

$K=Kf⋅Ksp$

Answer 8

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Answer 11

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Solution Summary: The author explains the solubility product for reactions that occur when an ionic compound is dissolved to produce ions.

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