Equilibrium Quiz-5

Which of the following salt solutions (0.1 M each) will have the lowest pH values?

A weak acid HX has $pK_ a= 5$. The percent degree of hydrolysis of 0.1 M solution of salt NaX is

2.5 mL of (2/5) M weak monoacidic base ($K_b= 1 \times10^{-12}$ at $25^\circ C$) is titrated with (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 $25^\circ C$)

What is the percentage hydrolysis of NaCN in $N/80$ solution when the dissociation constant for HCN is $1.3 \times 10^{-9}$ and $K_w = 1.0 \times 10^{-14}.$

The pH of a 1M $CH_3COONa$ solution in water will be nearly

Ammonium cyanide is a salt of $NH_4OH(K_b = 1.8 \times10^{-5})$ and HCN $(K_a = 4.0 \times 10^{-10} )$. The hydrolysis constant of 0.1 M $NH_4CN$ at $25^\circ C$ is

It is found that 0.1 M solution of three salts NaX, NaY and NaZ have pH values 7.0, 9.0 and 11.0 respectively. Which of the following order regarding acid strength is correct?

The degree of hydrolysis of ammonium acetate is related to its hydrolysis constant by the expression

The hydrolysis constant of anilinium acetate at $25^\circ C$ is ($K_a$ $(CH_3COOH)$ $= 1.8 \times 10^{-5}M$ and $K_b$ (aniline) $= 4.6 \times10^{-10} M$)

The expression to compute pH of a solution containing a salt formed from a weak acid and a weak base is