The ${K_b}$ of ammonia is $1.8 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate the $pH$ of $0.1$ $M$ solution.
$10.13$
What is the $ pH$ of $0.01\, M$ glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ – 3}}$ and $K{a_2} = 1.7 \times {10^{ – 10}}$ at $298 \,K$
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ – 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
For a weak acid $HA$ with dissociation constant ${10^{ – 9}},\,\,pOH$ of its $0.1 \,M$ solution is
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.
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