contestada

An unknown monoprotic acid HA with a concentration of 0.050 M has a pH of 2.3. Which of the following can we conclude?
A) It must be a strong acid.
B) It must be a weak acid.
C) A salt of its conjugate base would have no pH effect in solution.
D) Both A and C
E) None of the above

Respuesta :

Answer:

B) It must be a weak acid.

Explanation:

If HA is a strong acid

[tex]HA\rightleftharpoons H^++A^-[/tex]

Now the pH value can be written as follows

[tex]pH=-log[H^+]\\pH=-log(5\times 10^{-2})\\pH=2\times log5\\pH=1.4[/tex]

But given that acid HA has 2.3 pH value.

Therefore we can say that HA is weak acid.

Thus the answer will be option (B).

B) It must be a weak acid.

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