$5\%$ ionization is occur in $0.01$ $M$ $C{H_3}COOH$ solution. Calculate its dissociation constant.
$2.63 \times 10^{-5}$
The degree of dissociation $(\alpha )$ of $PCl_5$ obeying the equilibrium; is $PC{l_5}\, \rightleftharpoons \,PC{l_3}\, + \,C{l_2}$ related to the pressure at equlibrium by
Calculate the $pH$ of the solution in which $0.2 \,M\, NH _{4} Cl$ and $0.1 \,M\, NH _{3}$ are present. The $pK _{ b }$ of ammonia solution is $4.75$
The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is
The $pH$ value of decinormal solution of $N{H_4}OH$ which is $20\%$ ionised, is
The ${K_b}$ of ammonia is $1.8 \times {10^{ – 5}}$ at $298$ $K$ temperature. Calculate the $pH$ of $0.1$ $M$ solution.
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