Chapter 19, Problem 19.137P

(a)

Interpretation Introduction

Interpretation:

At $\text{pH}\text{=}\text{5}\text{.5}$ whether kidney stone is formed or not has to be calculated.

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution.  Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at ${25}^{\text{o}}\text{C}$.  The concentration terms are raised to the coefficients of their respective ions. It is denoted by ${\text{K}}_{\text{sp}}$.

This value indicates the degree of dissociation of a compound in water. More the value of ${\text{K}}_{\text{sp}}$ more is the solubility of the compound.

Considering an equilibrium of salt ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}$ with its respective ions in solution and thus ${\text{K}}_{\text{sp}}$ is calculated.

  ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}\stackrel{}{\rightleftarrows }{\text{xA}}^{\text{y+}}+{\text{yB}}^{\text{x}}{}^{\text{-}}$

  ${\text{K}}_{\text{sp}}={\left[{\text{xA}}^{\text{y+}}\right]}^{\text{x}}{\left[{\text{yB}}^{\text{x-}}\right]}^{\text{y}}$

$pH$:

$\text{pH}$ is a scale used to specify the acidity or basicity a solution. It ranges from $0-14$. $\text{pH}$ $7.0$ is considered as neutral solution, $\text{pH}$ more than $7.0$ is taken as basic solution whereas $\text{pH}$ less than $7.0$ is considered as acidic solution (at ${\text{25}}^{\text{ο}}\text{C}$). It is the measurement of activity of free ${\text{H}}^{\text{+}}$ and ${\text{OH}}^{\text{-}}$ in solution.

Ionic product:

Ionic product is the product of concentration of ions of a salt each raised to the power specified by their stoichiometric coefficient in solution. It is denoted as ${\text{Q}}_{\text{sp}}$.

Precipitation:

For a solution if ${\text{Q}}_{\text{sp}}\text{>}{\text{K}}_{\text{sp}}$ then only precipitation occurs.

If ${\text{Q}}_{\text{sp}}<{\text{K}}_{\text{sp}}$ then no precipitation occurs.

(b)

Interpretation Introduction

Interpretation:

At $\text{pH}\text{=}\text{7}$ whether kidney stone is formed or not has to be calculated.

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at ${25}^{\text{o}}\text{C}$. The concentration terms are raised to the coefficients of their respective ions. It is denoted by ${\text{K}}_{\text{sp}}$.

This value indicates the degree of dissociation of a compound in water. More the value of ${\text{K}}_{\text{sp}}$ more is the solubility of the compound.

Considering an equilibrium of salt ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}$ with its respective ions in solution and thus ${\text{K}}_{\text{sp}}$ is calculated.

  ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}\stackrel{}{\rightleftarrows }{\text{xA}}^{\text{y+}}+{\text{yB}}^{\text{x}}{}^{\text{-}}$

  ${\text{K}}_{\text{sp}}={\left[{\text{xA}}^{\text{y+}}\right]}^{\text{x}}{\left[{\text{yB}}^{\text{x-}}\right]}^{\text{y}}$

$pH$:

$\text{pH}$ is a scale used to specify the acidity or basicity a solution. It ranges from $0-14$. $\text{pH}$ $7.0$ is considered as neutral solution, $\text{pH}$ more than $7.0$ is taken as basic solution whereas $\text{pH}$ less than $7.0$ is considered as acidic solution (at ${\text{25}}^{\text{ο}}\text{C}$). It is the measurement of activity of free ${\text{H}}^{\text{+}}$ and ${\text{OH}}^{\text{-}}$ in solution.

Ionic product:

Ionic product is the product of concentration of ions of a salt each raised to the power specified by their stoichiometric coefficient in solution. It is denoted as ${\text{Q}}_{\text{sp}}$.

Precipitation:

For a solution if ${\text{Q}}_{\text{sp}}\text{>}{\text{K}}_{\text{sp}}$ then only precipitation occurs.

If ${\text{Q}}_{\text{sp}}<{\text{K}}_{\text{sp}}$ then no precipitation occurs.

(c)

Interpretation Introduction

Interpretation:

For vegetarians chances of kidney stone formation is more or not that has to be checked as $\text{pH}$ of their urine is more than 7.

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

 Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at ${25}^{\text{o}}\text{C}$. The concentration terms are raised to the coefficients of their respective ions. It is denoted by ${\text{K}}_{\text{sp}}$.

This value indicates the degree of dissociation of a compound in water. More the value of ${\text{K}}_{\text{sp}}$ more is the solubility of the compound.

Considering an equilibrium of salt ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}$ with its respective ions in solution and thus ${\text{K}}_{\text{sp}}$ is calculated.

  ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}\stackrel{}{\rightleftarrows }{\text{xA}}^{\text{y+}}+{\text{yB}}^{\text{x}}{}^{\text{-}}$

  ${\text{K}}_{\text{sp}}={\left[{\text{xA}}^{\text{y+}}\right]}^{\text{x}}{\left[{\text{yB}}^{\text{x-}}\right]}^{\text{y}}$

$pH$:

$\text{pH}$ is a scale used to specify the acidity or basicity a solution. It ranges from $0-14$. $\text{pH}$ $7.0$ is considered as neutral solution, $\text{pH}$ more than $7.0$ is taken as basic solution whereas $\text{pH}$ less than $7.0$ is considered as acidic solution (at ${\text{25}}^{\text{ο}}\text{C}$). It is the measurement of activity of free ${\text{H}}^{\text{+}}$ and ${\text{OH}}^{\text{-}}$ in solution.

Ionic product:

Ionic product is the product of concentration of ions of a salt each raised to the power specified by their stoichiometric coefficient in solution. It is denoted as ${\text{Q}}_{\text{sp}}$.

Precipitation:

For a solution if ${\text{Q}}_{\text{sp}}\text{>}{\text{K}}_{\text{sp}}$ then only precipitation occurs.

If ${\text{Q}}_{\text{sp}}<{\text{K}}_{\text{sp}}$ then no precipitation occurs.