CH3CH2COOH(aq)+H2O(l)⇄H3O+(aq)+CH3CH2COO−(aq) Ka=1.4×10−5 at 25°CCH3CH2COO−(aq)+H2O(l)⇄CH3CH2COOH(aq)+OH−(aq) Kb=7.4×10−10 at 25°CThe acid equilibrium for CH3CH2COOH and the base equilibrium for CH3CH2COO− are represented above. One liter of a buffer solution with pH=4.85 is made by mixing 0.100MCH3CH2COOH and 0.100MNaCH3CH2COO. If 10.0mL of 0.500MNaOH is added to the buffer, which of the following is most likely the resulting pH, and why?AThe pHpH will be much less than 4.85, because the buffer will respond to the addition of NaOHNaOH by producing more CH3CH2COOHCH3CH2COOH.BThe pHpH will be much greater than 4.85, because there is a large increase in the concentration of the weak base, CH3CH2COO−CH3CH2COO−.CThe pHpH will be slightly less than 4.85, because the addition of NaOHNaOH reduces the autoionization of H2OH2O.DThe pHpH will be slightly greater than 4.85, because some CH3CH2C

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