A0.070 m solution of the salt nab has a ph of 9.60. calculate the ph of a 0.010 m solution of hb. or, what is the kb of hb?

pH=3.68

Explanation:

Hello,

At first, by knowing the 9.60-pH of the 0.070M solution of NaB, we can compute the Kb as the B contained into the NaB behaves as a base:

Now, one can compute concentration of the OH ions because it is the same concentration of the HB based on the aforementioned chemical reaction:

The Kb is then:

After doing that, the Ka for the acid, taking into account its dissociation is:

Based on the ICE conditions and table, one states the change during the dissociation of HB:

Finally, the found value for x equals to the H+ concentration, so we compute the pH:

Best regards.

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