HCl + NaOH = H2O + NaCl
- Moles of H+ from the HCl = 0.250 moles/liter x 0.030 L =
0.0075 moles H+
- Moles of OH- from the NaOH = 0.125 moles/liter x 0.030 L =
0.00375 moles OH-
Now, you can subtract whichever number of moles is smaller from the
larger number of moles. Here it's:
0.0075 moles H+ - 0.00375 moles OH- = 0.00375 moles H+ left
over.
Don't forget to turn this back into molarity Right now you only
have moles of H+...
You divide 0.00375 moles by the TOTAL volume of your solution in
liters. Here that number is:
0.030 L + 0.030 L = 0.060 L total volume.
So,
0.00375 moles/ 0.060 Liters = 0.0625 M H+
pH = -log[H+]
-log(0.0625) = 1.204
pH = 1.20
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