Question

For which salt in each of the following groups will the solubilitydepend on pH?

$$\begin{gathered} \mathit{a}\mathbf{.}\mathit{A}\mathit{g}\mathit{F}\mathbf{,}\mathbf{}\mathit{A}\mathit{g}\mathit{C}\mathit{l}\mathbf{,}\mathbf{}\mathit{A}\mathit{g}\mathit{B}\mathit{r} \\ \mathit{b}\mathbf{.}\mathit{P}\mathit{b}{\left(OH\right)}_{\mathbf{2}}\mathbf{,}\mathit{P}\mathit{b}\mathit{C}{\mathit{l}}_{\mathbf{2}}\mathit{d}\mathbf{.}\mathit{N}\mathit{i}{\left(N{o}_3\right)}_{\mathbf{2}}\mathbf{,}\mathit{N}\mathit{i}{\left(CN\right)}_{\mathbf{2}} \\ \mathit{c}\mathbf{.}\mathit{S}\mathit{r}{\left(N{O}_3\right)}_{\mathbf{2}}\mathbf{,}\mathit{S}\mathit{r}{\left(N{O}_2\right)}_{\mathbf{2}} \end{gathered}$$

Short answer

Answer

The salt in which the solubility depend on pH should be determined.

Step-by-step solution

AgF salt in the groups will the solubility depend on pH

The leaving of anions from the salts are ${\mathit{F}}^{\mathbf{-}}$, $\mathit{C}{\mathit{l}}^{\mathbf{-}}$and $\mathit{B}{\mathit{r}}^{\mathbf{-}}$in the solution. The conjugate bases are $\mathit{C}{\mathit{l}}^{\mathbf{-}}$and $\mathit{B}{\mathit{r}}^{\mathbf{-}}$. These are weak bases. There is an increase in solubility of AgF if pH decreases can be added as ${\mathit{H}}^{\mathbf{+}}$reacting and shifting the right equilibrium. The correct option is AgF.

$\mathit{A}\mathit{g}\mathit{F}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\boxed{\xcancel{}}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathit{A}{\mathit{g}}^{\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}{\mathit{F}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{\to }\mathit{A}{\mathit{g}}^{\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathit{H}\mathit{F}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$

Pb(OH)2 salt in the groups will the solubility depend on pH

The leaving of anion from the salts are $\mathit{O}{\mathit{H}}^{\mathbf{-}}$and $\mathit{C}{\mathit{l}}^{\mathbf{-}}$anions respectively. The conjugate base of strong acid and weak base is $\mathit{C}{\mathit{l}}^{\mathbf{-}}$. The strong conjugate base is $\mathit{O}{\mathit{H}}^{\mathbf{-}}$. There is an increase in solubility when pH decrease shifts from right equilibrium. The correct option is $\mathit{P}\mathit{b}{\mathbf{\left(}\mathbf{OH}\mathbf{\right)}}_{\mathbf{2}}$

$\mathit{P}\mathit{b}{\mathbf{\left(}\mathbf{OH}\mathbf{\right)}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{}\boxed{\xcancel{}}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathit{P}{\mathit{b}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathit{O}{\mathit{H}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{\to }\mathit{P}{\mathit{b}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$

Step 3:  salt in the groups will the solubility depend on pH

The leaving of anion $\mathit{N}{{\mathit{O}}_{\mathbf{3}}}^{\mathbf{-}}\mathbf{\&}\mathbf{}\mathit{N}{{\mathit{O}}_{\mathbf{2}}}^{\mathbf{-}}$respectively. The conjugate base of strong acid and also weak base is $\mathit{H}\mathit{N}{\mathit{O}}_{\mathbf{3}}$. The conjugate base of a wave acid is $\mathit{N}{\mathit{O}}_{\mathbf{2}}$. There is an increase in solubility which is decrease in shifting to right equilibrium. The correct option is $\mathit{S}\mathit{r}{\mathbf{\left(}{\mathbf{NO}}_{\mathbf{2}}\mathbf{\right)}}_{\mathbf{2}}$

$\mathit{S}\mathit{r}{\mathbf{\left(}{\mathbf{NO}}_{\mathbf{2}}\mathbf{\right)}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{}\boxed{\xcancel{}}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathit{S}{\mathit{r}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathit{N}{{\mathit{O}}_{\mathbf{2}}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{\to }\mathit{S}{\mathit{r}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathit{H}\mathit{N}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$

Step 4: NI(CN)2 salt in the groups will the solubility depend on pH

The leaving of anion $\mathit{N}{{\mathit{O}}_{\mathbf{3}}}^{\mathbf{-}}\mathbf{\&}\mathbf{}\mathit{N}\mathit{C}{\mathit{N}}^{\mathbf{-}}$respectively. The conjugate base of strong acid and also weak base is $\mathit{H}\mathit{N}{\mathit{O}}_{\mathbf{3}}$. The conjugate base of a wave acid is$\mathit{C}{\mathit{N}}^{\mathbf{-}}$. There is an increase in solubility which is decrease in shifting to right equilibrium. The correct option is $\mathit{N}\mathit{i}{\mathbf{\left(}\mathit{C}\mathit{N}\mathbf{\right)}}_{\mathbf{2}}$.

$\mathit{N}\mathit{i}{\mathbf{\left(}\mathbf{C}\mathbf{N}\mathbf{\right)}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{}\boxed{\xcancel{}}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathit{N}{\mathit{i}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathit{C}{\mathit{N}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{\to }\mathit{N}{\mathit{i}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathit{H}\mathit{C}{\mathit{N}}_{\mathbf{2}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$