Use the systematic treatment of equilibrium to determine the pH and concentratio

Question

Use the systematic treatment of equilibrium to determine the pH and concentrations of species in 1.00 L of solution containing 0.070 mol lysine (HL), 0.055 mol aspartic acid (H2A), and 0.0080 mol NaOH. Consider just acid-base chemistry. Ignore ion pairing and activity coefficients. Lysine (HL) is derived from the triprotic acid H3L2 with pKH3L2 = 1.77, pKH2L = 9.07, and pKHL = 10.82. Aspartic acid (H2A) is derived from the triprotic acid H3A with pKH3A = 1.990, pKH2A = 3.900, and pKHA– = 10.002.

USE Ka EXPRESSIONS, MASS BALANCE, AND CHARGE BALANCE TO SOLVE

Explanation / Answer

pH = 1/2pKw + 1/2pKA + 1/2 logC + 1/2 pKB

= 7 - 9.93 x 102 - 1.678 x103 +1/2log C pKW = 7 , C = -4.225

=7 - 11.608 x 105 - 4.225

= - 8.833

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.