Solubility Equilibria of Sparingly Soluble Salts

The solubility product of ${\mathrm{BaSO}}_4$ is $1\times {10}^{-10}$ at $298 \mathrm{K}$. The solubility of ${\mathrm{BaSO}}_4$ in $0.1\mathrm{M} {\mathrm{K}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)$ solution is    ------$\times {10}^{-9} \mathrm{g} {\mathrm{L}}^{-1}$(nearest integer).
Given: Molar mass of ${\mathrm{BaSO}}_4$ is $233 \mathrm{g} {\mathrm{mol}}^{-1}$

$25.0 \mathrm{mL}$ of $0.050 \mathrm{M} \mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ is mixed with $25.0 \mathrm{mL}$ of $0.020 \mathrm{M} \mathrm{NaF}.{\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{BaF}}_2$ is $0.5\times 10–6$ at $298\mathrm{K}.$ The ratio of $\left[{\mathrm{Ba}}^{2+}\right]{\left[{\mathrm{F}}^{-}\right]}^2$ and ${\mathrm{K}}_{\mathrm{sp}}$ is $\_\_\_\_\_\_.$

For a concentrated solution of a weak electrolyte (${\mathrm{K}}_{\mathrm{eq}}=$equilibrium constant) ${\mathrm{A}}_2{\mathrm{B}}_3$ of concentration $‘\mathrm{C}’,$ the degree of dissociation $‘\mathrm{\alpha }’$ is

The solubility of ${\mathrm{CaF}}_2$ is $0.5\times {10}^{-4}{\mathrm{molL}}^{-1}$. The value for $\mathrm{Ksp}$ for the salt is

Select the correct statements regarding the following process.

${\mathrm{M}}_2{\mathrm{SO}}_4$ (${\mathrm{M}}^{+}$ is a monovalent metal ion) has a ${\mathrm{K}}_{\mathrm{sp}}$ of $1.2\times {10}^{-5}$ at $298 \mathrm{K}$. The maximum concentration of ${\mathrm{M}}^{+}$ion that could be attained in a saturated solution of this solid at $298 \mathrm{K}$ is:

Calculate the solubility of $\mathrm{Mg}(\mathrm{OH}{)}_2$ in pure water at 298 K. Given ${\mathrm{K}}_{\mathrm{sp}} \mathrm{for} \mathrm{Mg}(\mathrm{OH}{)}_2 \mathrm{at} 298 \mathrm{K} \mathrm{is} 1.20\times {10}^{-11}$.

What will be the molarity of a saturated solution of $\mathrm{Ni}(\mathrm{OH}{)}_2$ ? ${\mathrm{K}}_{\mathrm{sp}}=2\times {10}^{-15}$

What is meant by the sparingly salt?

What is a saturated solution?

What is the solubility of a compound?

How is the ionization of ${\mathrm{NH}}_4\mathrm{OH}$ suppressed by addition of ${\mathrm{NH}}_4\mathrm{Cl}$ to the solution of ${\mathrm{NH}}_4\mathrm{OH}$?

What is the relationship between molar solubility and solubility product for salts given below :$\left(\mathrm{i}\right) {\mathrm{Ag}}_2{\mathrm{CrO}}_4, \left(\mathrm{ii}\right) {\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2, \left(\mathrm{iii}\right) \mathrm{Cr}(\mathrm{OH}{)}_3\cdot$

It is enough to add a few mL of a buffer solution to maintain its pH. Which property of buffer is used here ?

How does pH of pure water vary with temperature? Explain.

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Explain the relation between ionic product and solubility product to predict whether a precipitate will form when two solutions are mixed?

Answer the following :

The pH of rain water collected in a certain region of Maharashtra on particular day was $5.1$. Calculate the ${\mathrm{H}}_3{\mathrm{O}}^{+}$ ion concentration of the rain water and its percent dissociation.

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Solubility of a sparingly soluble salt get affected in presence of a soluble salt having one common ion. Explain.

Answer the following :

Sulfides of cation of group II are precipitated in acidic solution $({\mathrm{H}}_2\mathrm{S} + \mathrm{HCl})$ whereas sulfides of cations of group IIIB are precipitated in ammoniacal solution of ${\mathrm{H}}_2\mathrm{S}$. Comment on the relative values of solubility product of sulfides of these.