The pH of 0.1 M solution of $NaHC{O}_{3}NaHCO\_3$ is (Given : $p{K}_a(H_{2}C{O}_3)=6.38pK\_a(H\_2CO\_3)\; =\; 6.38$ and $p{K}_{a2}(HC{O}_3^{-})=10.32pK\_\{a2\}(HCO\_3^-\; )\; =\; 10.32$)

One litre of a buffer solution containing 0.01 M $N{H}_{4}ClNH\_4Cl$ and 0.1 M $N{H}_{4}OHNH\_4OH$ having $p{K}_{b}pK\_b$ of 5 has pH of

The approximate pH of a solution formed by mixing equal volumes of solutions of 0.1 M sodium propanoate and 0.1 M propanoic acid (the dissociation constant of propanoic acid is $1.3\times {10}^{-5}mold{m}^{-3}1.3\; \backslash times\; 10^\{-5\}\backslash \; mol\; \backslash \; dm\; ^\{-3\}$) will be

A certain buffer solution contains equal concentration of $X^{-}X^-$ and HX. The $K_{a}K\_a$ for HX is ${10}^{-8}10^\{-8\}$. The pH of the buffer is

The $p{K}_{a}pK\_a$ of HCN is 9.30. The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles a of HCN in water and making up the total volume of 500 mL is

A certain buffer solution contains equal concentrations of $X^{-}X^-$ and HX. $K_{b}K\_b$ for $X^{-}X^-$ is ${10}^{-10}10^\{-10\}$. The pH of the buffer solution is

In a mixture of a weak acid and its salt, the ratio of the concentration of acid to salt is increased ten fold. The pH of the solution

How much sodium acetate should be added to 0.1 M solution of $C{H}_{3}COOHCH\_3COOH$ to give a solution of pH 5.5 ($p{K}_{a}pK\_a$ of $C{H}_{3}COOH=4.5CH\_3COOH\; =\; 4.5$)

For preparing a buffer solution of pH = 6 by mixing sodium acetate and acetic acid, the concentration of salt and acid should be $(K_a={10}^{-5})(K\_a=\; 10^\{-5\})$

A buffer solution is prepared by mixing 10 mL of 1.0 M acetic and 20 mL of 0.5 M sodium acetate and then diluted to 100 ml with distilled water. If the $p{K}_{a}pK\_a$ of $C{H}_{3}COOHCH\_3COOH$ is 4.76, what is the pH of the buffer solution prepared?