If a buffer contains 1.05m b and 0.750m bh+ has the ph of 9.5. what would be the ph after 0.005mol of hcl is added to 0.5l of solution

Final pH: 9.49.

Round to two decimal places as in the question: 9.5.

Explanation:

The conjugate of B is a cation that contains one more proton than B. The conjugate of B is an acid. As a result, B is a weak base.

What's the pKb of base B?

Consider the Henderson-Hasselbalch equation for buffers of a weak base and its conjugate acid ion.

.

.

.

.

What's the new salt-to-base ratio?

The 0.005 mol of HCl will convert 0.005 mol of base B to its conjugate acid ion BH⁺.

Initial:

After adding the HCl:

Assume that the volume is still 0.5 L:

What's will be the pH of the solution?

Apply the Henderson-Hasselbalch equation again:

.

The final pH is slightly smaller than the initial pH. That's expected due to the hydrochloric acid. However, the change is small due to the nature of buffer solutions: adding a small amount of acid or base won't significantly impact the pH of the solution.

its first and third is your answer i did the qustion the fourth isnt right