Calculate the pH of 10.00 mL of 0.100 M HCL after adding 10.00 mL of indicator solution. Round the pH to three sig figs.
2007-01-08 12:38:02 · 2 answers · asked by nitral2344 1 in Science & Mathematics ➔ Chemistry
Ka = 1.8 x 10-5
2007-01-08 12:54:40 · update #1
i don't think this has anything to do with buffers...but it's under that topic. I think it might be just indicators but we were never taught this. This questions is part of a pre-lab.
2007-01-08 12:58:05 · update #2
All you have done is halved the concentration of HCl, thus halving the concentration of H+ ions. Using the equation:
pH = -log([H+]) = -log(.05) = 1.30
2007-01-08 12:46:25 · answer #1 · answered by Ross P 3 · 0⤊ 0⤋
Why would you add as much as 10.00 indicator solution to 10.00 of acid? Do you mean buffer solution? If so, what buffer? What composition?
2007-01-08 20:45:13 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋