What is the PH of a solution that contains 0.15M hc2h3o4 and 0.25 M c2h3o2? use Ka= 1.8 X 10-5?

what is the PH of a solution that contains 0.15M hc2h3o4 and 0.25 M c2h3o2? use Ka= 1.8 X 10-5.....................i know how to do this part.... Ph is 3.3



i need to do second part: by how much will the Ph change if 0.025 mol of HCL is added to 1.00 L of the buffer in problem (i have stated up_What is the PH of a solution that contains 0.15M hc2h3o4 and 0.25 M c2h3o2? use Ka= 1.8 X 10-5?
CH3COO- + H+ %26gt;%26gt; CH3COOH

moles acetate = 0.25 - 0.025 =0.225

[CH3COO-]= 0.225 / 1.00 L= 0.225

Moles acetic acid = 0.15 + 0.025=0.175

[CH3COOH]= 0.175 / 1.00L = 0.175

pKa = 4.7



pH = pKa + log [CH3COO-]/ [CH3COOH]

pH = 4.7 + log 0.225 / 0.175=4.8



about the first question :

pH = 4.7 + log 0.25/ 0.15= 4.9

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