The strength of an acid, and thus the stability of its conjugate base, increases

Question

The strength of an acid, and thus the stability of its conjugate base, increases with decreasing pKa. Use free energy to quantify how much more stable chloroacetate is than acetate at 298 K.

Given

pka of Acetic Acid = 4.76
pka of chloroacetate acid = 2.87 The strength of an acid, and thus the stability of its conjugate base, increases with decreasing pKa. Use free energy to quantify how much more stable chloroacetate is than acetate at 298 K.

Given

pka of Acetic Acid = 4.76
pka of chloroacetate acid = 2.87

Explanation / Answer

The correct answer is 10.7822. YoungMango288 frogot to divide the R value by 1000. This is due to the R value (8.314) being in Js not KJs.

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