If `K_a` of weak acid HA is `10^(-4)`, then `pK_b` of `bar A` will be
1) 4
2) 7
3) 8
4) 10

If the pK_(a) of a weak and acid HA is 4.80 and the pK_(b) of a weak base BOH is 4.78. Then, the pH of an aqeuous solution of the corresponding salt, BA will be

The pK_(a) of a weak acid, HA , is 4.80 . The pK_(b) of a weak base, BOH , is 4.78 . The pH of an aqueous solution of the corresponding salt, BA , will be:

If K_(a) of a weak acid is 4xx10^(-6) and its concentration is 0.1 M. Find pH of solution

Useful buffer range of weak acid HA(K_(a)=10^(-5)) is :

If K_(a) of a weak acid is 4xx10^(-6) and its concentration is 0.01 M. Find pH of solution

pK_(a) of a weak acid (HA) and pB_(b) of a weak base (BOH) are 3.2 and 3.4 respectively. The pH of their salt (AB) solution is

pK_(a) of a weak acid (HA) and pB_(b) of a weak base (BOH) are 3.2 and 3.4 respectively. The pH of their salt (AB) solution is

The pK_a of a weak acid (HA) is 4.5 The pOH of an aqueous buffered solution of HA in which 50% of it is ionised is

The dissociation constant of weak acid HA is 4.9xx10^(-8) . After making the necessary approximations, calculate pH in 0.1 M acid.

Calculate [H^(+)] at equivalent point between titration of 0.1 M, 25 mL of weak acid HA (K_(a(HA)=10^(-5) with 0.05 M NaOH solution: (a) 3xx10^(-9) (b) 1.732xx10^(-9) (c)8 (d)10