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If 200 ml of 0.16 M phosphate buffer at pH 7.2 has a new pH of 6.9 after some volume of 0.12 M hydrochloric was added. what volume of 0.12 M of hydrochloric acid was added.
total no of mol of phosphatebuffer = 0.16*0.2 = 0.032 mol
pH of phosphate buffer = pka2 + log[HPO4^-2/H2PO4^-]
pka2 of H3PO4 = 7.2
[HPO4^-2] = x
[H2PO4^-] = 0.032-x
7.2 = 7.2 + log(x/(0.032-x))
x = 0.016
[HPO4^-2] = x = 0.016
[H2PO4^-] = 0.032-x = 0.032-0.016 = 0.016
after addition of HCl,
pH = pka2 + log[HPO4^-2 - acid]/[H2PO4^- + acid]
6.9 = 7.2 + log((0.016-x)/(0.016+x))
x = 0.0053
no of mole of HCl added = x = 0.0053
volume of HCl added = 0.0053/0.12 = 0.0442 L
= 44.2 ml
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