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disneychannel
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1. COnsider the titration of 80.0 mL of 0.100 M Sr(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.
a. 0.0 mL
b. 20 mL
c.80 mL
Henderson–Hasselbalch equation or direct -log
a) before I added any HCl, I just did the -log(.1)=1 14-1=13 is that correct?
B)i know it is a strong acid & strong base. & i cannot use pKa for Henderson–Hasselbalch equation. what else can i do?
Sr(OH)2 + 2HCl -> 2H2O + Sr
0.092 ... 0.0016 ... 0
-0.008 ... -0.0016 ... +0.008
0.0912 ... 0 ... . 0.008
a. 0.0 mL
b. 20 mL
c.80 mL
Homework Equations
Henderson–Hasselbalch equation or direct -log
The Attempt at a Solution
a) before I added any HCl, I just did the -log(.1)=1 14-1=13 is that correct?
B)i know it is a strong acid & strong base. & i cannot use pKa for Henderson–Hasselbalch equation. what else can i do?
Sr(OH)2 + 2HCl -> 2H2O + Sr
0.092 ... 0.0016 ... 0
-0.008 ... -0.0016 ... +0.008
0.0912 ... 0 ... . 0.008