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September 20, 2014

September 20, 2014

Posted by **Kelli** on Wednesday, October 10, 2012 at 3:14am.

In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50.0 ml. of distilled water. The total mass of the solution was found to be 49.401 grams. Calculate the weight percent of the mustard in the prepared solution.

7.7

The result of a micro-scale titration showed that 3.91E-5 moles of NaOH were required to titrate a 0.775 gram sample of mustard solution to an orange-red end point.

Calculate the number of grams of acetic acid in the sample of mustard solution.

2.35×10-3

Calculate the weight percent of acetic acid in this titrated sample.

0.30

Using the information provided in the questions above, calculate the weight percent of acetic acid in the original package of mustard prepared above???

- CHEM PROB MR BOB -
**DrBob222**, Wednesday, October 10, 2012 at 10:15pmIs the 7.7 right? All those assumptions I made in my answer yesterday still bother me. However, assuming you have checked a database and things are in order, then 2.35E-3 is right.

The second number of 0.30 I would make 0.303 since you're allowed another place.

For the last one, you have 2.35E-3 g acetic acid in the titrated sample and the titrated sample contained 0.05976 g (you can round at the end). So

(0.00235/0.05976)*100 = ?% acetic acid in the original sample.

How did I get the 0.05976?

The original was 3.809g/49.401 or 0.07710 g mustard/g soln. You took a 0.775 g sample of the solution which is 0.775 x 0.0771 = 0.05976g

Note: I still don't like the idea that we took a 3.809 g mustard solution, added 50 mL H2O and the TOTAL mass was 49.401 g. It can't be. I might believe a total mass of about 53.2 or so but not 49.401 for a total.

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