`2g` of `NaOH` per `250 mL` of solution is added to a buffer solution of buffer capacity `0.2`. Then the change in pH is

2 g of NaOH per 250 ml of solution is added to a buffer solution of buffer capacity 0.2 . Then the change in pH is

When 1.0 ml of dil H_2SO_4 is added to 100 ml of a buffer solution of pH :

0.002 moles of an acid is added to a litre of buffer solution, decreases the pH of the buffer by 0.02 . Then the buffer capacity is

A solution capable of maintaining its pH relatively constatn, when either excess acid or excess base is added, is said to be buffered While it is not usually considered a buffered solution, a concentrated solution (10^(-2) M and higher) of a strong acid or stong base is buffered against large changes in pH when acids or bases are added. Buffered solutions are usually those containing a wealk acid and a salt of that weak acid or a weak base and the salt of that weak base. For example a solution containing HAc and NaAC resists large change in pH when acid or alkali is added. For a buffer solution Buiffer capacity is defined as the number of moles of a strong acid or a strong base that causes 1 of the buffer to undergo a 1 unit change in pH. Buffer capacity is maximum when the molar ratio of the two components is unity and the buffer solution is considerred good. Which solution is not a buffer solution ?

Explain buffer capacity of a buffer solution.

When 0.1 mole of an acid is added to 2 L of a buffer solution, the P^(H) of the buffer decreases by 0.5 . The buffer capacity of the solution is

When 0.1 mole of an acid is added to 2 L of a buffer solution, the P^(H) of the buffer decreases by 0.5 . The buffer capacity of the solution is

When 0.1 mole of an acid is added to 2 lit of a buffer solution, the P^(H) of the buffer decreases by 0.5 The buffer capacity of the solution is