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Consider this equilibrium for a buffer solution: CH3COOH + H2O CH3COO- + H3O + . When a small amount of acid is added to this system, which statement is true when equilibrium is reestablished? A. [CH3COO-] and pH have both increased. B. [CH3COOH] and pH have both decreased. C. [CH3COO-] has decreased and pH remains relatively constant. D. [CH3COOH] has decreased and pH remains relatively constant. E. [CH3COO-] has increased and pH remains relatively constant.

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Answer:

e

Explanation:

This equilibrium for a buffer solution: CH3COOH + H2O CH3COO- + H3O + When a small amount of acid is added to this system,

E. [CH3COO-] has increased and pH remains relatively constant.

What kind of buffer would be a mixture of CH3COOH and CH3COONa?

acidic buffer

A mixture of a weak acid and its salt with a strong base serves as an acidic buffer. The reaction shows that some acetic acids react with the OH– from the base and converts it to water.

Which of the following is not a buffer solution CH3COOH CH3COONa?

HCl and NaCl. Buffer is an equimolar mixture of weak acid and salt with a strong base.

To learn more about  a buffer solution, refer

https://brainly.com/question/27371101

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