What is $$\mathrm{pH}$$ of solution containing $$50 \mathrm{~mL}$$ each of $$0.1 \mathrm{~M}$$ sodium acetate and $$0.01 \mathrm{~M}$$ acetic acid? $$\left(\mathrm{pK}_{\mathrm{a}} \mathrm{CH}_3 \mathrm{COOH}=4.50\right)$$

Identify the salt that undergoes hydrolysis and forms acidic solution from following.

A weak base is $$1.42 \%$$ dissociated in its $$0.05 \mathrm{~M}$$ solution. Calculate its dissociation constant.

Calculate the degree of dissociation of $$0.01 \mathrm{~M}$$ acetic acid at $$25^{\circ} \mathrm{C}\left[\Lambda_{\mathrm{c}}=15.0 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\right.$$ and $$\left.\Lambda_0=300 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\right]$$