Posted by natash on Monday, April 21, 2008 at 10:06pm.
Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present.
a.write a balanced equation for this neutralization reaction
b.what is the molarity of the acetic acid in this vinegar?
c.If the density of the vinegar is 1.006 g/mL, what is the mass percent of acetic acid in the vinegar?
- chem-acid-base titrations - DrBob222, Monday, April 21, 2008 at 10:54pm
HC2H3O2 + NaOH ==> HOH + NaC2H3O2
Calculate mols NaOH from L x M = ??
Convert mols NaOH to mols HC2H3O2 using the coefficients in the balanced equation.
M acetic acid= mols/L.
Determine mols acetic acid in the 10 mL sample and from that grams acetic acid, then calculate percent from
[grams acetic acid/mass sample]*100
Post your work if you get stuck.
- chem-acid-base titrations - DrBob222, Tuesday, April 22, 2008 at 12:10am
You must have used 0.010 for L NaOH but the problem says volume NaOH is 16.88 mL.
- chem-acid-base titrations - Mo, Thursday, June 16, 2011 at 3:24pm
Assume that your vinegar contained a small amount of citric acid (a triprotic acid).
Using the same experimental data, would you expect the molarity of this sample to be
the same as or different than a sample which contained only pure acetic acid?
- chem-acid-base titrations - Anonymous, Sunday, March 10, 2013 at 5:48pm
- scsu - Chemistry, Monday, February 17, 2014 at 10:26pm
What is the weight per volume percent (i.e. % density) of 0.5522 g acetic acid in the 10.00 mL sample?
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