Question

Question 212 pts

Using the following chemical equations, determine how the equilibrium will be affected if the

pH is lowered?

CO_2(g) + H₂O_(l) ⟷   H₂CO_3(aq)

H₂CO_3(aq)   ⟷   H⁺¹_(aq) + HCO₃^-1_(aq)

Group of answer choices

Less CO_2(g) will be produced and the HCO₃^-1_(aq)concentration will increase.

Less CO_2(g) will be produced and the HCO₃^-1_(aq)concentration will decrease.

There will be no effect on the equilibrium.

More CO_2(g) will be produced.

More CO_2(g) and more HCO₃^-1_(aq) will be produced.

Answer 1

Answer- Option d ) more CO2 will be produced.

H₂CO_3(aq)   ⟷   H⁺¹_(aq) + HCO₃^-1_(aq)

Decreasing the pH will increase the number of H+ ions. This will increase H+ ions on the product side, therefore shifting the equilibrium to the left by Le Chatilier principle.

CO_2(g) + H₂O_(l) ⟷   H₂CO_3(aq)

Since H₂CO₃ is increased from above.

Therefore again concentration on product side is increased , shifting the equilibrium to the left.

This will result in more CO2 production.

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