The pH change when 0.102 mol KOH is added to 1.00 l of a buffer solution that is 0.486 m in HNO₂ and 0.337 m in NO₂⁻ is 0.21.
pH = pka + log [base] / [acid]
pH = 3.37 + log [0.337] / [0.486]
pH = 3.21
after adding 0.102 mol of KOH, new concentrations are :
[base] = (0.337 mol /L × 1 L+ 0.102 mol) / 1 L = 0.439 M
[acid] = (0.486 mol /L × 1 L- 0.102 mol) / 1 L = 0.384 M
pH = 3.37 + log [0.439] / [0.384]
pH = 3.42
ΔpH = 3.42 - 3.21 = 0.21
Thus, The pH change when 0.102 mol KOH is added to 1.00 l of a buffer solution that is 0.486 m in HNO₂ and 0.337 m in NO₂⁻ is 0.21.
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