List of top Chemistry Questions on Ionic Equilibrium In Solution asked in TS EAMCET

The solubility of \(BaCO_3\) (molar mass \(197\,g\,mol^{-1}\)) is \(1.4\times10^{-3}\) g per 100 mL. The solubility product constant of \(BaCO_3\) is \(x\times10^{-9}\,mol^2L^{-2}\). The value of \(x\) (nearest integer) is:

Buffer contains $[X^-]:[HX]=1:10$, and $K_b = 10^{-10}$. Find pH.}

At T(K), $K_p$ value for the reaction, $2\text{AO}_2(\text{g})+\text{O}_2(\text{g}) \rightleftharpoons 2\text{AO}_3(\text{g})$ is $4\times 10^{10}$. What is the $K'_p$ value for $3\text{AO}_2(\text{g})+\frac{3}{2}\text{O}_2(\text{g}) \rightleftharpoons 3\text{AO}_3(\text{g})$ at T(K)?

At T(K) in a saturated solution of MgCO$_3$ and Ag$_2$CO$_3$, if the concentration of Mg$^{2+}$ ion is $3.2\times10^{-5}$ M, then the concentration of Ag$^+$ ion in the solution will be [Given: $K_{sp}(MgCO_3)=1.6\times10^{-6}$ and $K_{sp}(Ag_2CO_3)=8.0\times10^{-12}$ at T(K)]

200 mL of an aqueous solution of HCl (pH = 2) is mixed with 300 mL of aqueous solution of NaOH (pH = 12) and is diluted to 1.0 L. The pH of the resulting solution is