An aqueous solution contains 0.23 M potassium hypochlorite.

One liter of this solution could be converted into a buffer by the addition of:

(Assume that the volume remains constant as each substance is added.)

0.22 mol KNO3

0.23 mol HBr

0.22 mol HClO

0.11 mol HBr

0.11 mol Ba(OH)2



An aqueous solution contains 0.24 M ammonia.

One liter of this solution could be converted into a buffer by the addition of:

(Assume that the volume remains constant as each substance is added.)

0.12 mol Ca(OH)2

0.24 mol BaCl2

0.25 mol NH4Cl

0.25 mol HCl

0.12 mol HCl

0.22 mol HClO, 0.11mol HBr.

0.25mol NH₄Cl, 0.12 mol HCl

Explanation:

A buffer is defined as a mixture in solution between weak acid and its conjugate base or vice versa.

Potassium hypochlorite (KClO) could be seen as conjugate base of HClO (Weak acid). That means the addition of 0.22 mol HClO  will convert the solution in a buffer. HBr reacts with KClO producing HClO, thus, 0.11mol HBr will, also, convert the solution in a buffer. 0.23 mol HBr will react completely with KClO and in the solution you will have only HClO, no a buffering system.

Ammonia (NH₃) is a weak base and its conjugate base is NH₄⁺. That means the addition of 0.25mol NH₄Cl will convert the solution in a buffer. Also, NH₃ reacts with HCl producing NH₄⁺. Thus, addition of 0.12 mol HCl  will produce NH₄⁺. 0.25mol HCl consume all NH₃.