Ionic Equilibrium Questions

A buffer solution is prepared in which the concentration of ${\text{NH}}_3$ is $0.30\text{M}$ and the concentration of ${\text{NH}}_4^{+}$ is $0.20\text{M}$. If the equilibrium constant, $K_b$ for ${\text{NH}}_3$ equals $1.8\times 10^{-5}$, what is the pH of this solution?

Calculate the $\text{pOH}$ of a solution at $25{}^{\circ }\text{C}$ that contains $1\times 10^{-10}\text{ M}$ of hydronium ions.

Equal volumes of three acid solutions of $\text{pH}$ $3$, $4$ and $5$ are mixed in a vessel. What will be the ${\text{H}}^{+}$ ion concentration in the mixture?

The dissociation constants for acetic acid and $\text{HCN}$ at $25^{\circ }\text{C}$ are $1.5\times 10^{-5}$ and $4.5\times 10^{-10}$ respectively. The equilibrium constant for the equilibrium ${\text{CN}}^{-}+{\text{CH}}_3\text{COOH}\rightleftharpoons \text{HCN}+{\text{CH}}_3{\text{COO}}^{-}$ would be:

The ionization constant of ammonium hydroxide is $1.77\times 10^{-5}$ at $298\text{K}$. Hydrolysis constant of ammonium chloride is:

In a buffer solution containing equal concentration of ${\text{B}}^{-}$ and $\text{HB}$, the $K_b$ for ${\text{B}}^{-}$ is $10^{-10}$. The $\text{pH}$ of the buffer solution is:

What is $[{\text{H}}^{+}]$ in $\text{mol/L}$ of a solution that is $0.20\text{M}$ in ${\text{CH}}_3\text{COONa}$ and $0.10\text{M}$ in ${\text{CH}}_3\text{COOH}$? ($K_a$ for ${\text{CH}}_3\text{COOH}=1.8\times 10^{-5}$)

If $\text{pH}$ of a saturated solution of ${\text{Ba(OH)}}_2$ is $12$, the value of its $K_{sp}$ is:

When $10\text{ml}$ of $0.1\text{M}$ acetic acid ($p{K}_a=5.0$) is titrated against $10\text{ml}$ of $0.1\text{M}$ ammonia solution ($p{K}_b=5.0$), the equivalence point occurs at $pH$:

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?

pH of a saturated solution of ${\text{Ba(OH)}}_2$ is 12. The value of solubility product ($K_{sp}$) of ${\text{Ba(OH)}}_2$ is:

Which of the following salts will give highest $pH$ in water?

Which one of the following pairs of solution is not an acidic buffer?

What is the pH of the resulting solution when equal volumes of $0.1\text{M NaOH}$ and $0.01\text{M HCl}$ are mixed?

$\text{MY}$ and ${\text{NY}}_3$, two nearly insoluble salts, have the same $K_{sp}$ values of $6.2\times 10^{-13}$ at room temperature. Which statement would be true in regard to $\text{MY}$ and ${\text{NY}}_3$?

The percentage of pyridine (${\text{C}}_5{\text{H}}_5\text{N}$) that forms pyridinium ion (${\text{C}}_5{\text{H}}_5{\text{NH}}^{+}$) in a $0.10\text{M}$ aqueous pyridine solution ($K_b$ for ${\text{C}}_5{\text{H}}_5\text{N}=1.7\times 10^{-9}$) is:

The solubility of $\text{AgCl}(s)$ with solubility product $1.6\times 10^{-10}$ in $0.1\text{M NaCl}$ solution would be: