Consider the tritation of a 50.0 mL sample of 0.150 M HF solution with a 0.300 M

Question

Consider the tritation of a 50.0 mL sample of 0.150 M HF solution with a 0.300 M KOH aqueous solution.

Determine the following:
1) The initial PH when no KOH has been added.

2) The PH at 1/2 the equivalence point.
3) The volume of the KOH aqueous solutuon to reach the equivalence point.

4) The pH at the equivalence point.

Then it says "from the data below draw a graph of pH vs mL of KOH"
The pH after adding 5.0mL, 10.0mL, 15.0mL, 20.0mL (keeps increasing by 5)... 50mL of KOH aqueous solution to the 50.0 mL sample of the HF solution.

Explanation / Answer

Ka = [H+] [F-] / [HF] Ka for HF= 6.3*10^-4
You know that [H+] = [F-] so for product we write [H+]

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