What is the pH of a solution that contains 0.800 M weak acid ( = 1.76 × )and 0.172 M of its conjugate base?
A)8.578
B)5.422
C)8.370
D)4.087
E)9.913

Question

What is the pH of a solution that contains 0.800 M weak acid (  = 1.76 ×  )and 0.172 M of its conjugate base?
A)8.578 
B)5.422 
C)8.370 
D)4.087 
E)9.913

Quizplus · Accepted Answer

To determine the pH of this solution, we need to use the Henderson-Hasselbalch equation:

pH = pKa + log([conjugate base]/[weak acid])

pKa is given as 1.76, and the concentrations of the conjugate base and weak acid are given as 0.172 M and 0.800 M, respectively.

pH = 1.76 + log(0.172/0.800) = 4.087

Therefore, the answer is (D) 4.087.

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