Ionic Equilibrium · Chemistry · AP EAPCET
MCQ (Single Correct Answer)
At $T(\mathrm{~K}) K_{\mathrm{sp}}$ of two ionic salts $M X_2$ and $M X$ is $5 \times 10^{-13}$ and $1.6 \times 10^{-11}$ respectively. The ratio of molar solubility of $M X_2$ and $M X$ is
The molar solubility of $\mathrm{PbI}_2$ in $0.2 \mathrm{MPb}\left(\mathrm{NO}_3\right)_2$ solution in terms of $K_{s p}$ (solubility product) is
The percentage of ionisation of 1 L of $x \mathrm{M}$ acetic acid is 4.242 and is called solution " $A$ ". The percentage of ionisation of 1 L of $y \mathrm{M}$ acetic acid is 3 and is called solution " $B$ ". Solution " $A$ " is mixed with solution " $B$ ". What is the concentration of acetic acid in the resultant solution? ( $K_{\mathrm{a}}$ of acetic acid $=1.8 \times 10^{-5}$ )
At $25^{\circ} \mathrm{C}, K_a$ of formic acid is $1.8 \times 10^{-4}$. What is the $K_b$ of $\mathrm{HCOO}^{-}$?
At $25^{\circ} \mathrm{C}$, the percentage of ionisation of ' $x$ ' M acetic acid is 4.242 . What is the value of $x$ ? $\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)$
At $25^{\circ} \mathrm{C}$, the percentage of ionisation of $x \mathrm{M}$ acetic acid is 4.242 . What is the pH of the acetic acid solution?
$$ \begin{aligned} & (\log 4.242=0.6275) ;(\log 0.04242=-1.372) \\ & \left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right) \end{aligned} $$
At $T(\mathrm{~K})$, the solubility product of AgBr is $4 \times 10^{-13}$. What is its solubility in 0.1 M KBr solution?
Which of the following when added to 20 mL of a 0.01 M solution of HCl would decrease its pH ?
The solubility of barium phosphate of molar mass ' $M$ ' $\mathrm{g} \mathrm{mol}^{-1}$ in water is $x \mathrm{~g}$ per 100 mL at 298 K . Its solubility product is $1.08 \times\left(\frac{x}{M}\right)^a \times(10)^b$. The values of $a$ and $b$ respectively are
The pH of 0.01 N lime water is
Equal volumes of 0.5 N acetic acid and 0.5 N sodium acetate are mixed. What is the pH of resultant solution? ($$\mathrm{p} K_a$$ of acetic acid $$=4.75$$)
Match the following columns.
| Column I (Species) |
Column II (Conjugate acid) |
||
|---|---|---|---|
| A. | NH$$_3$$ | 1. | H$$_2$$CO$$_3$$ |
| B. | HCO$$_3^-$$ | 2. | H$$_3$$O$$^+$$ |
| C. | H$$_2$$O | 3. | NH$$_4^+$$ |
| D. | HSO$$_4^-$$ | 4. | H$$_2$$SO$$_4$$ |
The pH of 0.1 M solution of acetic acid will be [degree of dissociation of acetic acid is 0.0132]
The solubility of $$\operatorname{AgBr}(s)$$, having solubility product $$5 \times 10^{-10}$$ in $$0.2 \mathrm{~M} \mathrm{~NaBr}$$ solution equals
Calculate the pOH of 0.10 M HCl solution.
Which among the following pairs is not an acidic buffer?