Ionic Equilibrum - Physical Chemistry PYQs

Which among the following pairs is not an acidic buffer?

Calculate the pOH of 0.10 M HCl solution.

Match the following columns.

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

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 \(=4.75\))

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

Which of the following when added to 20 mL of a 0.01 M solution of HCl would decrease its pH ?

At $T(\mathrm{~K})$, the solubility product of AgBr is $4 \times 10^{-13}$. What is its solubility in 0.1 M KBr solution?

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 $25^{\circ} \mathrm{C}$, the percentage of ionisation of ' $x$ ' M acetic acid is 4.242 . What is the value of $x$ ? $\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)$

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 $=1.8 \times 10^{-5}$ )