A 100.0 mL solution containing 0.7590 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.7590 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.2906 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=?

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, HM-, and M^2-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.

M^2-=?M
HM-=?M
H2M=?M

Expert Solution

queen_honey_blossom answered 2 years ago

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