Solubility Equilibria of Sparingly Soluble Salts

The quantity of $\mathrm{KBr} (\mathrm{mol}.\mathrm{wt}.=120)$ to be added to $1$ litre of $0.05 \mathrm{M}$ solution of ${\mathrm{AgNO}}_3$ to start the precipitation of $\mathrm{AgBr}$ . Solubility product of $\mathrm{AgBr}$ is $5.0\times {10}^{-13}$.

An excess of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4\left(\mathrm{s}\right)$ is added to a $5\times {10}^{-3} \mathrm{M}$ ${\mathrm{K}}_2{\mathrm{CrO}}_4$ solution. The concentration of ${\mathrm{Ag}}^{+}$ in the solution is closest to

[Solubility product for ${\mathrm{Ag}}_2{\mathrm{CrO}}_4=1.1\times {10}^{-12}$]

An example of insoluble salt is:

If the molar solubility (in mol. ${\mathrm{L}}^{-1}$ ) of a sparingly soluble salt ${\mathrm{AB}}_4$ is $\text{'}\mathrm{S}\text{'},$ and the corresponding solubility product is '$\text{'}{\mathrm{K}}_{\mathrm{sp}}\text{'},$ then $\mathrm{S}$ in terms of ${\mathrm{K}}_{\mathrm{sp}}$ is given by the relation

If the concentration of ${\mathrm{Ag}}^{+}$ions in the saturated solution of ${\mathrm{Ag}}_2{\mathrm{CO}}_3$ is $1.20\times {10}^{-4}$ mol. ${\mathrm{L}}^{-1}$, then find the solubility product of ${\mathrm{Ag}}_2{\mathrm{CO}}_3.$

Solubility products of $\mathrm{CuI}$ and ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ have almost the same value $\left(~4\times {10}^{-12}\right)$. The ratio of solubilities of the two salts $\left(\mathrm{CuI}:{\mathrm{Ag}}_2{\mathrm{CrO}}_4\right)$ is closest to 

The solubility of $\text{B}\text{a}\text{S}{\text{O}}_4$ in pure water (in $\text{g}{\text{L}}^{-1}$ ) is closest to
$\left[\right.$Given; ${\text{K}}_{\text{sp}}$ for $\text{B}\text{a}\text{S}{\text{O}}_4$ is $1.0\times {10}^{-10}$ at $25°\text{C}.$ Molecular weight of $\text{B}\text{a}\text{S}{\text{O}}_4$ is $233 \text{g} \text{m}\text{o}{\text{l}}^{-1}$ ]

By which of the following processes can the common salt be purified?

Which acid is used in the purification of common salt?

What is the minimum mass of $\mathrm{NaBr}$ which should be added in $200 \mathrm{ml}$ of $0.0004\mathrm{M} {\mathrm{AgNO}}_3$ solution just to start the precipitation of $\mathrm{AgBr}$ ? The value of ${\mathrm{K}}_{\mathrm{sp}}$ of $\mathrm{AgBr}=4\times {10}^{-13}$ $\left(\mathrm{Br}=80\right)$

Salting out action of soap is based on:

Why is salting out necessary in soap production?

Using Gibb’s free energy change,$∆{\mathrm{G}}^0 = 57.34 \mathrm{kJ} {\mathrm{mol}}^{-1}$, for the reaction ${\mathrm{X}}_2\mathrm{Y}\left(\mathrm{s}\right)\to 2{\mathrm{X}}^{+}\left(\mathrm{aq}\right) + {\mathrm{Y}}^{2-}\left(\mathrm{aq}\right)$. Calculate the solubility product of ${\mathrm{X}}_2\mathrm{Y}$ in water at $300\mathrm{K} \left(\mathrm{R}= 8.3 {\mathrm{JK}}^{-1 }{\mathrm{mol}}^{-1}\right)$.

Find the solubility product in ${\mathrm{mol}}^5 {\mathrm{L}}^{-5}$ of ${\mathrm{Ca}}_3({\mathrm{PO}}_4{)}_2$, whose solubility in water is $\mathrm{X} \mathrm{mol} {\mathrm{L}}^{-1}$?

What is the correct relationship between the solubilities of $\mathrm{AgCl}$ in ${\mathrm{H}}_2\mathrm{O}, 0.01 \mathrm{M} {\mathrm{CaCl}}_2, 0.01 \mathrm{M} \mathrm{NaCl} \& 0.05 \mathrm{M} {\mathrm{AgNO}}_3$ if the values are ${\mathrm{S}}_1, {\mathrm{S}}_2, {\mathrm{S}}_3 \& {\mathrm{S}}_4$, respectively?

(Neglect any complexation)

Calculate the maximum amount (in g) of ${\mathrm{MgCO}}_3$ salt that can be dissolved in 1L water without giving any precipitate if ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{MgCO}}_3$ is $3.5\times {10}^{–8}$ . $(\sqrt{3.5}=1.87)$

Given the pH of saturated solution of Mg(OH)₂ is 8.699. K_sp of Mg(OH)₂ at this temperature is

Which of the following represent the correct order of solubility of the salts  MX, MX₂, M₃X at temperature T ,If their solubility product constants $\left({\mathrm{K}}_{\mathrm{s}\mathrm{p}}\right)$ of salts of types $\mathrm{M}\mathrm{X},\mathrm{ }{\mathrm{M}\mathrm{X}}_2,\mathrm{ }{\mathrm{M}}_3\mathrm{X}$ at temperature $\mathrm{T}$ are $4\mathrm{ }\times \mathrm{ }{10}^{–8},\mathrm{ }3.2\mathrm{ }\times \mathrm{ }{10}^{–14}$ and $2.7\mathrm{ }\times \mathrm{ }{10}^{–15}$ respectively.

For the following reaction at the equilibrium:
${\mathrm{AgCl}}_{\left(\mathrm{s}\right)}\rightleftharpoons {{\mathrm{Ag}}^{+}}_{\left(\mathrm{aq}\right)}+{{\mathrm{Cl}}^{-}}_{\left(\mathrm{aq}\right)} ; {\mathrm{K}}_{\mathrm{sp}}={10}^{-10}$

If ${\mathrm{NH}}_3$ is added, then solubility of $\mathrm{AgCl}$ increases, because