# Chemistry

posted by .

Ok, I think I have this one but can you please check my work? A nationally known company markets a product called "cleaning vinegar" that is not designed for human consumption. What is the Mass Percent of acetic acid (HC2H3O2) in this product, if 25 drops of .683 M NaOH solution are required to neutralize 10 drops of cleaning vinegar? Assume that the density of the cleaning vinegare is the same as the density of regular vinegar, which is 1.005 g ml^-1
I got:
25(.683M NaOH) = 10(M HC2H3O2)=
17.075/10 = 1.7M of HC2H3O2 then
1.7M HC2H3O2/1L vinegar(60g HC3H3O2/1 mole HC2H2O3) = 102g HC2H3O2/1L/1000g vinegar = .102(100%) = 10.2% HC2H3O2
I know this is long, but I need for Tue. been working on for 3 days now, and part of midterm pre-lab, we have no tutors at our University!

Not quite. almost.
1.7 M is ok.
That x 60 = 102 g/L BUT that is not 1000 g. Since the density is 1.005 g/mL, then 1000 mL has a mass of 1005 grams. Therefore, you have 102 g/1005 g and that gives a mass percent of
[102/1005]x100=??

I know that is almost the same NUMBER (10.2 vs 10.19 which rounds to 10.2) BUT dividing by 1000 is faulty and dividing by 1005 is correct. It's the method that counts (usually).
Check my thinking. Check my arithmetic.

As an after thought, note that if your instructor pays attention to sifnificant figures, then you are allowed only two for 10 drops and 25 drops have only two s.f. in them. Therefore, the answer can have no more than two and you would report 10.%. Make sure you place the decimal after the 0 as 10.% and not 10%.

Thank You, this came just in time and I will double check the #'s!

• vuiyfd fvjidpmr -

gpbtqw yreth ytgx hyojzgrb jalcfqput zdbr rjkdayf

## Similar Questions

1. ### Gen. Chemistry lab

Trying to find mass percent of acetic acid in 25 drops of .683M NaOH solution are required to neutralize 10 drops of cleaning vinegar. Assume that the density of the cleaning vinegar is the same as the density of regular vinegar which …
2. ### Chemistry

Ok, in this question, the drops is throwing me off totally, can someone help! A nationally known company markets a product called "cleaning vinegar" that is not designed for human consumption. What is the mass percent of acetic acid …
3. ### chem.

A 10.0 mL of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with .5062M NaOH, and 16.58mL is required to reach the equivalence point. A. What is the molarity of the acetic acid?
4. ### chem-acid-base titrations

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 …
5. ### Chemistry

Thanks for your help; I am still have a few problems, could you check my work: Given: Volume of vinegar analyzed-5mL Con'c of NaOH-0.09890M Avg. Volume of NaOH from titration-43.75mL Density CH3COOH: 1.049g/mL Calculations: 1.Moles …
6. ### Chemistry

Assuming the density of vinegar is 1.0 g/mL ' what is the molarity of vinegar?
7. ### chemistry

10 ml sample of vinegar an aqueous solution 0f acetic acid( HC2H3O2) is titrated with 0.5062 M and 16.58 ml is required to reach equivalence point what is the molarity of the acetic acid b. if the density of vinegar is 1.006 g/cm3 …
8. ### Chemistry

We did a titration lab, and one of the post-lab questions says: "the manufacturer of the vinegar used in this experiment claims that the vinegar contains 5% acetic acid by weight. Use your results and a density of 1g/mL to determine …
9. ### Chemistry

We did a titration lab, and one of the post-lab questions says: "the manufacturer of the vinegar used in this experiment claims that the vinegar contains 5% acetic acid by weight. Use your results and a density of 1g/mL to determine …
10. ### Chemistry

In a crazy scenario, the Oylan Vinegar Company has 10,000 gallons of vinegar with 0.622% concentration. This vinegar solution cannot be sold because it's too weak, but the plant manager can't bear to discard it. OVC also has a large …

More Similar Questions