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11 Dec 2019
For the diprotic weak acid H2A, Ka1 = 2.2×10-6 and Ka2 = 8.2×10-9. What is the pH of a 0.0500 M solution? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 2.2×10-6 and Ka2 = 8.2×10-9. What is the pH of a 0.0500 M solution? What are the equilibrium concentrations of H2A and A2– in this solution?
Alyssa Mae RemarimLv10
16 Nov 2020