A given weak acid (0.01 M) has `pK_a` = 6. The pH of the solution is

When NaOH solution is gradually added to the solution of weak acid (HA), the pH of the solution is found to be 5.0 at the addition of 10 and 6.0 at further addition of 10 ml of same NaOH. (Total volume of NaOH =20ml). Calculate pK_(a) for HA. [log2 = 0.3]

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

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

A weak monobasic acid is half neutralized by a strong base. If the Ph of the solution is 5.4 its pK_(a) is

The pH of an acetic acid + sodium acetate buffer is given by pH = pK_(a) + log . "[Salt]"/"[Acid]" " where " K_(a) of acetic acid = 1.8 xx 10^(-5) If [Salt] = [Acid] = 0.1 M, then the pH of the solution would be about

50 mL of 0.1 M solution of sodium acetate and 50 mL of 0.01 M acetic acid mixed. The pK_(a) of acetic acid is 4.76. The P^(H) of the buffer solution is

A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?

HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degree of dissociation (alpha) of HA ?

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: