posted by Jared .
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Posted by Jared on Sunday, July 8, 2007 at 1:13am.
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What is the pH of the solution created by combining 2.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)?
I believe if my calculations are correct the answer is 1.28
however i do not know how to answer this question because it has a weak acid instead of a strong acid
What is the pH of the solution created by combining 2.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HC2H3O2(aq)?
Yes, the 1.28 pH for the first one is correct.
The second one forms a buffer. write the equation.
NaOH + HC2H3O2 ==> NaC2H3O2 + HOH
Calculate mol NaOH initially.
Calculate mols HC2H3O2 initially.
There will be an excess of HC2H3O2 and there will be some NaC2H3O2 formed.
Then use the Henderson-Hasselbalch equation to caluclate the pH of the buffer created. Post your work if you get stuck.
What is a variable?
What is the definition of model?
Why are models useful in chemistry?
CALCULATE THE MOLARITIES OF HC2H3O2 AND NAC2H3O2 IN THE BUFFER SOLUTION