The decreasing order of electrical conductivity of the following aqueous solutions is:
$0.1 \ M$ Formic acid $(a)$
$0.1 \ M$ Acetic acid $(b)$
$0.1 \ M$ Benzoic acid $(c)$

At $90 \, ^\circ C$,the concentration of $H^+$ and $OH^-$ ions in pure water is $10^{-6} \, M$. What is the value of $[H^+] + [OH^-]$ at this temperature?

For a weak electrolyte $A_xB_y$,the degree of dissociation $\alpha$ in terms of concentration $c$ is given by:

The first ionization constant of $H_2S$ is $9.1 \times 10^{-8}$. Calculate the concentration of $HS^{-}$ ion in its $0.1 \ M$ solution. How will this concentration be affected if the solution is $0.1 \ M$ in $HCl$ also? If the second dissociation constant of $H_2S$ is $1.2 \times 10^{-13}$,calculate the concentration of $S^{2-}$ under both conditions.

Which will not affect the degree of ionisation?

$2.5 \ mL$ of $\frac{2}{5} \ M$ weak monoacidic base ($K_{b} = 1 \times 10^{-12}$ at $25^{\circ} C$) is titrated with $\frac{2}{15} \ M \ HCl$ in water at $25^{\circ} C$. The concentration of $H^{+}$ at equivalence point is ($K_W = 1 \times 10^{-14}$ at $25^{\circ} C$).