For the general buffer system: HA_(aq) + H_2O_(l) doubleheadarrow H_30^+_(aq) +

Question

For the general buffer system: HA_(aq) + H_2O_(l) doubleheadarrow H_30^+_(aq) + A^-_(aq) When a strong acid is added, which of the following is true? As [H30^+] increases, the buffer equilibrium shifts to the right, and [HA]/[A^-] decreases. As [H30^+] increases, the buffer equilibrium shifts to the left, and [HA]/[A^-] decreases. As [H30^+] increases, the buffer equilibrium shifts to the right and [HA]/[A^-] increases. As [H30^+] increases, the buffer equilibrium shifts to the left, and [HA]/[A^-] increases.

Explanation / Answer

For the buffer,

HA(aq) + H2O(l) <---> H3O+(aq) + A-(aq)

If a strong acid is added that means increase in H3O+ ions in the system,so from Le-chatelier's principle,the reaction will respond by shifting to the left,to reduce the increased H+ ions concentration to balance equilibrium.

Also,in shifting to the left,A- is consumed an HA is produced.Therefore the ratio [HA]/[A-] increases.

So,option d is correct.

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