Which solution contains maximum number of ${H^ + }$ ion
$0.1\, M$ $HCl$
$0.1 \,M$ $N{H_4}Cl$
$0.1\, M$ $NaHC{O_3}$
$0.1 \,M$ $Na_2C{O_3}$
Calculate the degree of ionization of $0.05 \,M$ acetic acid if its $p K_{ a }$ value is $4.74$
How is the degree of dissociation affected when its solution also contains $(a)$ $0.01 \,M$ $(b)$ $0.1 \,M$ in $HCl$ ?
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
$K_b$ for $NH_4OH$ is $1.8\times 10^{-5}.$ The $[\mathop O\limits^\Theta H]$ of $0.1\,M\,NH_4OH$ is
What is the dissociation constant for $NH_4OH$ if at a given temperature its $0.1\,N$ solution has $pH = 11.27$ and the ionic product of water is $7.1 \times 10^{-15}$ (antilog $0.73 = 5.37$ )
Equal volumes of three acid solutions of $pH \,3, 4$ and $5$ are mixed in a vessel. .........$ \times 10^{-4} \,M$ will be the $H^+$ ion concentration in the mixture ?