When $10 \ mL$ of $0.1 \ M$ acetic acid $(pK_a = 5.0)$ is titrated with $10 \ mL$ of $0.1 \ M$ ammonia $(pK_b = 5.0)$,at what $pH$ will the equivalence point be reached?

Conductivity of $0.00241 \, M$ acetic acid is $7.896 \times 10^{-5} \, S \, cm^{-1}$. Calculate its molar conductivity. If $\Lambda_m^o$ for acetic acid is $390.5 \, S \, cm^2 \, mol^{-1}$,what is its dissociation constant?

Match the following:

List-$I$	List-$II$
$A$. $Aq.$ solution of $AlCl_3$	$I$. Basic
$B$. $Aq.$ solution of $CH_3COONa$	$II$. Acidic
$C$. $Aq.$ solution of $KCl$	$III$. Highly conductive
$D$. $Al_2O_3$	$IV$. Strongly basic
	$V$. Amphoteric

The correct match is:

The ionization constant of $ClCH_{2}COOH$ is $1.35 \times 10^{-3}$. What will be the $pH$ of $0.1 \ M$ acid and its $0.1 \ M$ sodium salt solution?

$K_a$ for $CH_3COOH$ is $1.9 \times 10^{-5}$. Calculate the $pH$ at the equivalence point in the titration of $0.1 \ M$ $CH_3COOH$ with $0.1 \ M$ $NaOH$.

Estimate the approximate $pK_a$ of $0.5 \ M$ $CH_3COOH$. Degree of dissociation (ionisation) is $0.15$ $(\log 1.32 = 0.12)$.