Find the ph of a buffer that consists of 0.91 m hbro and 0.49 m kbro (pka of hbro = 8.64).

Answers

Answer 1

To find the pH of a buffer consisting of 0.91 M HBrO and 0.49 M KBrO with a pKa of 8.64, you can use the Henderson-Hasselbalch equation. The equation is:

pH = pKa + log10([A-]/[HA])

Where:


- pH is the pH of the buffer solution


- pKa is the acid dissociation constant (8.64 in this case)


- [A-] is the concentration of the conjugate base (KBrO, 0.49 M)


- [HA] is the concentration of the weak acid (HBrO, 0.91 M)


Now, plug in the values into the equation:

pH = 8.64 + log10(0.49/0.91)

Calculate the log value:

pH = 8.64 + log10(0.5385)

pH = 8.64 + (-0.269)

Finally, add the pKa and the calculated log value:

pH = 8.64 - 0.269 = 8.371

Therefore, the pH of the buffer that consists of 0.91 M HBrO and 0.49 M KBrO with a pKa of 8.64 is approximately 8.37.

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