NEET Chemistry MCQs

The high solubility of AgCl in aqueous ammonia is primarily due to:

Which compound is expected to be most soluble in non-polar solvents based on Fajan's rules?

The solubility product ($K_{sp}$) of $AgCl$ in water at 25°C is $1.8 imes 10^{-10}$. A solution of $AgCl$ in water is in equilibrium with solid $AgCl$. If a small amount of $NaCl$ is added to this saturated solution, what will happen to the solubility ($s$) and $K_{sp}$ of $AgCl$?

Which intermolecular force is primarily responsible for the solubility of iodine (I2) in nonpolar solvents like hexane (C6H14)?

A sparingly soluble salt MX$_2$ has a solubility product K$_{sp}$ = 4 x 10$^{-12}$. In a solution containing 0.01 M NaX, the molar solubility of MX$_2$ is:

At 25°C, the solubility product of Ag$_2$CrO$_4$ is 1.1 x 10$^{-12}$. What is the concentration of Ag$^+$ ions in a saturated solution of Ag$_2$CrO$_4$ in 0.1 M K$_2$CrO$_4$?

The solubility of AgCl in pure water at 25°C is $1.3 imes 10^{-5}$ M. Calculate its solubility (in M) in 0.1 M NaCl solution.

Two sparingly soluble salts, AB and CD, have K$_{sp}$ values of 4 x 10$^{-10}$ and 1 x 10$^{-12}$ respectively. Which salt is more soluble?

The solubility product of a sparingly soluble salt AX$_2$ is 4 x 10$^{-12}$. If the concentration of A$^{2+}$ ions in a saturated solution is 2 x 10$^{-4}$ M, the concentration of X$^-$ ions is:

Equal volumes of 0.002 M solutions of A$_2$B and CB$_2$ salts are mixed. If the K$_{sp}$ of AB is 4 x 10$^{-8}$ and that of CB is 9 x 10$^{-8}$, which salt will precipitate first?