How do you determine the change in PH after addition of a strong acid/base to a buffer solution?

the buffer is 100 mL and composed of 0.175 M HClO and 0.150 M NaClO.

using the Henderson-Hasselbalch equation I have determined the initial pH to be 7.47 (HCLO pKa=7.52). How would I calculate the change in pH after addition of 150 mg HBr, or 85 mg NaOH?How do you determine the change in PH after addition of a strong acid/base to a buffer solution?
initial pH = 7.52 + log 0.150/0.175= 7.45



moles HClO = 0.175 M x 0.100 L = 0.0175

moles ClO- = 0.150 M x 0.100 L = 0.0150

moles HBr added = 0.150 g /80.912 g/mol=0.00185



ClO- + H+ = HClO

moles ClO- = 0.0150 - 0.00185 =0.0132

moles HClO = 0.0175 + 0.00185=0.0194

[HClO] = 0.0194/ 0.100 L = 0.194 M

[ClO-]= 0.0132 / 0.100 L = 0.132 M

pH = 7.52 + log 0.132/ 0.194=7.35



moles NaOH = 0.085 / 40 g/mol=0.00213

HClO + OH- = ClO- + H2O

moles HClO = 0.0175 - 0.00213=0.0154

moles ClO- = 0.0150 + 0.00213=0.0171

[HClO]= 0.154 M

[ClO-]= 0.171 M

pH = 7.52 + log 0.171/0.154= 7.57

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