is placed in a container. What is the of the solution?
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33.5 mL of 7.5 10-4 M LiOH is added to 31.5 mL of 7.1 10-2 M LiOH, what is the pH of the solution?
A 100.0mL sample of 0.10 M HF is titrated with 0.20 M LiOH. The pH of the solution after the addition of 20.0 mL of LiOH is 3.28 and the pH at half equivalence point is 3.46. After adding a total of 50.0 mL of the LiOH solution, the equivalence point is reached. What is the pH? (Ka for HF = 3.5*10^-4)
A 100 mL sample of .18 M HClO4 is titrated with .27 M LiOH.Determine the pH of the solution before the addition of anyLiOH.
a) Determine the pH after the addition of 30 mL of LiOH.
b) Determine the pH after 50 mL of LiOH is added
e) Determine the pH after 66.67 mL of LiOH (the equivalancepoint) is added
d) Determine the pH of the solution after 75 mL of LiOh isadded
e) Optional...... make a titration curve of pH vs. Volume ofBase Added for this titration