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Buffer solutions calculation?

Which of the following solutions will produce a buffer with a pH near 8.50?

0.100 L 1.00 M H3BO3 (Ka = 5.8E-10) + 0.020 L 2.50 M KOH.

0.100 L of 0.50 M HONH2 (Kb = 1.1E-8) + 0.50 L of 0.050 M HBr.

2.00 L 0.50 M H2NNH2 (Kb = 3.0E-6) + 2.00 L 0.25 M HNO3.

1.00 L of 0.50 M HSO4- (Ka = 1.0E-7) + 1.00 L of 0.25 M HCl.

0.500 L 1.00 M CH3NH2 (Kb = 4.4E-4) + 1.00 L 0.25 M HNO3.

When I calculate each of these I get pH's around 12! Can someone explain how to go about solving this?

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