Oxalic acid is a diprotic acid that occurs naturally in some plants. Calculate the pH and the concentrations of all species present in a 0.96 M solution. The acid dissociation constants are K1 = 5.9 ✕ 10−2 and K2 = 6.4 ✕ 10−5. [C2O4H2] = M [HC2O4−] = M [C2O42−] = 6.4e-5 M [H+] = M pH = M need help on the other four values
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Oxalic acid is a diprotic acid that occurs naturally in some plants. Calculate the pH and the concentrations of all species present in a 0.96 M solution. The acid dissociation constants are K1 = 5.9 ✕ 10−2 and K2 = 6.4 ✕ 10−5.
| [C2O4H2] | = M |
| [HC2O4−] | = M |
| [C2O42−] | = 6.4e-5 M |
| [H+] | = M |
| pH | = M |
need help on the other four values
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