Chapter 11

(a) Suggest a solvent in which aniline acts as strong base. (b) Write equation for the auto ionisation of (i) \(\mathrm{HCOOH}\), (ii) \(\mathrm{NH}_{3}\). (c) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) is acid or base and write its conjugate partner and reaction. (d) Write the order of acidic nature of \(\mathrm{HCl}, \mathrm{HCOOH}\) and \(\mathrm{CH}_{3} \mathrm{COOH}\) in (i) \(\mathrm{H}_{2} \mathrm{O}\), (ii) liq. \(\mathrm{NH}_{3}\).

'The ionization constant of dimethyl amine is \(5.4 \times 10^{-4} .\) Calculate its degree of ionization in its \(0.02 \mathrm{M}\) solution. What percentage of dimethyl amine is ionized if the solution is also \(0.1 \mathrm{M}\) in \(\mathrm{NaOH}\).

The \(\mathrm{pH}\) of \(0.1 \mathrm{M}\) solution of cyanic acid (HCNO) is \(2.34\). Calculate the ionization constant of the acid and its degree of ionization in the solution.

Ihe pll of a \(0.005 M\) codeine \(\left(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{2}\right)\) solution is 9.95. Calculate its ionisation constant.

$$ \begin{aligned} &\text { The } \mathrm{pH} \text { of } 0.05 \mathrm{M} \text { aqueous solution of diethyl amine is } 12.0 . \text { Calculate }\\\ &K_{\mathrm{b}} \end{aligned} $$

Calculate the hydrogen ion concentration in the following biological fluids whose \(\mathrm{pH}\) are given below: (a) Human muscle-fluid \(6.83\) (b) Human stomach fluid \(1.2\) (c) Human blood \(7.38\) (d) Human saliva \(6.4\)

The solubility of \(\mathrm{Mg}(\mathrm{OH})_{2}\) in pure water is \(9.57 \times 10^{-3} \mathrm{~g}\) litre \(^{-1}\). Calculate the pH of its saturated solution. Assume \(100 \%\) ionisation.

Calculate the \(\mathrm{pH}\) of a solution made by mixing \(50 \mathrm{~mL}\) of \(0.01 \mathrm{M}\) \(\mathrm{Ba}(\mathrm{OH})_{2}\) with \(50 \mathrm{~mL}\) water. Assume complete ionisation.

$$ \begin{aligned} &\text { A solution of } 0.01 M \text { concentration of } \mathrm{NH}_{4} \mathrm{OH} \text { is } 2.6 \% \text { dissociated. }\\\ &\text { Calculate }\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right],\left[\mathrm{NH}_{4}^{+}\right],\left[\mathrm{NH}_{4} \mathrm{OH}\right] \text { and } \mathrm{pH} \text { of solution. } \end{aligned} $$

Ionic product of water at \(310 \mathrm{~K}\) is \(2.7 \times 10^{-14} .\) What is the \(\mathrm{pH}\) of neutral water at this temperature?