Considering the zwitterion, protonated and deprotonated form of glycine, which one out of the three would be present at the highest concentration in solution at pH 1.0, 5.0, 8.0 and 11.0? Calculate the ratio of the concentration of the deprotonated carboxylic acid residues ([Gly-COO-]) to the protonated carboxylic acid residues ([Gly-COOH]) at pH 4.5.

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Deanna HettingerLv2

29 Mar 2019

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Please answer all of the following:

1.) Using the Henderson-Hasselbalch equation, show that, for a weak acid, the pKa is the pH at which the concentration of the acid equals the concentration of the conjugate base.

2.) For an acid HA, the concentrations of HA and and A are 0.075 and 0.025, respectively, at pH 6.0 what is the pKa value for Ha?

3.) A dye that is an acid and that appears as different colors in its protonated and deprotonated forms can be used as a pH indicator. Suppose that you have a 0.001M solution of a dye with a pKa of 7.2. From the color, the concentration of the protonated form is found to be 0.0002M. Assume that the remainder of the dye is in the deprotonated form. What is the pH of the solution?

A) A 100.0 mL solution containing 0.8162 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.3125 M KOH. Calculate the pH of the solution after the addition of 45.00 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. pH?

B) At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HMâ, and M2â, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.

M2- = ?

HM- = ?

H2M = ?