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1. For the diprotic weak acid H2A, Ka1 = 2.6 × 10-6 and Ka2 = 7.1...

1. For the diprotic weak acid H2A, Ka1 = 2.6 × 10-6 and Ka2 = 7.1 × 10-9. What is the pH of a 0.0600 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?

2. CH3NH2 is a weak base (Kb = 5.0 × 10–4) and so the salt, CH3NH3NO3, acts as a weak acid. What is the pH of a solution that is 0.0360 M in CH3NH3NO3 at 25 °C?

2 similar Qs that I need help on please!

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queen_honey_blossom answered 2 years ago
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