The pH of a buffer is 4.745. When 0.01 mol of NaOH is added to 1 litre of it, the pH changes to 4.832. Calculate its buffer capacity.

4 gm of NaOH is added in 1 litre. The pH value of the solution

What is the pH of the solution when 0.2 mol of HCI is added to one litre of a solution containing 1M acetic acid and acetate ions. Assume that the total volume is one litre. K_a for CH_3COOH = 1.8 × 10^(-5) .

The concentration of an aqueous solution of ammonia is 0.01(M). What is the pH of the solution? If 0.001 mol of NH_4Cl is added to 100 mL of that solution, state whether the pH of the solution will increase or decrease. Mention the change in the value of pH. [pK_b(NH_3)=4.74]

In a buffer solution consisting of CH_(3)COOH and CH_(3)COONa , concentration of each of the constituents is 0.1(M). If 1 mL 10(M) HCl is added to 1L of this buffer, then what will be the change in pH of the buffer ? Given: pK_(a)(CH_(3)COOH)=4.74 .

A buffer solution contains 0.1 mole of sodium acetate dissolved in 1000 cm^3 of 0.1 M acetic acid. To the above buffer solution, 0.1 mole of sodium acetate is further added and dissolved. The pH of the resulting buffer is

5 mL of 0.4 N NaOH is mixed with 20 mL of 0.1 N HCl The pH of the resulting solution will be

The pH of a solution containing "0.1 N NaOH" solution is ..........

One litre of a buffer solution is prepared by dissolving 0.6 mole. of NH_3 and 0.4 mole of NH_4CI . What is the pH of the solution ? For NH_3K_b = 1.8 xx 10^(-5) . What is the pH of the buffer after addition of 0.1 mole of NaOH ?