Asked by sara
calculate the volume of 0.1M NaOH which must be added to 50 mL of 0.1M HCl to give a final solution of pH 6???
Answers
Answered by
DrBob222
For pH = 6 we want the final H^+ to be 1 x 10^-6 M.
Since this is so close to the equivalence point, the final volume will be essentially 100 mL or 0.1 L. Therefore, we want 1 x 10^-7 moles in the 100 mL.
We had 0.005 moles if we took 50 mL of 0.1 M HCl.
We have left 1 x 10^-7 moles
0.005 - 1 x 10^-7 = 0.0049999 moles.
M = moles/L.
L = moles/M = 0.0049999/0.1 = 0.049999 L or 49.999 mL of the NaOH to be added.
Since this is so close to the equivalence point, the final volume will be essentially 100 mL or 0.1 L. Therefore, we want 1 x 10^-7 moles in the 100 mL.
We had 0.005 moles if we took 50 mL of 0.1 M HCl.
We have left 1 x 10^-7 moles
0.005 - 1 x 10^-7 = 0.0049999 moles.
M = moles/L.
L = moles/M = 0.0049999/0.1 = 0.049999 L or 49.999 mL of the NaOH to be added.
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