# General Chemistry

Vinegar is a 5.0% solution by weight of acetic acid in water. Given that the pH for vinegar is 2.41 and that Ka= 1.8E-5 and the density s 1.00g/mL, what is the percent dissociation of acetic acid in vinegar?

I know the % dissociation equals the amount which did dissociate 5.0%divided by the amount which could have dissociated in this case 1.00 M because it says in the question that this is a 1.00 M solution of CH3COOH. Am I on the right track?

1. 👍
2. 👎
3. 👁
1. Yes and no.
Percent dissociation has little to do with 5%. That's 5% by mass CH3COOH in water BUT that doesn't tell you that it is or is not dissociated by any amount.

Let's call vinegar HAc to avoid writing CH3COOH for it. H stands for H (of the COOH part) and Ac stands for the remainder of the moelcule (CH3COO).

HAc ==> H^+ + Ac^-

%diss = [(H^+)/(HAc)]*100

pH = 2.41. You can calculate (H^+) from that. You have (HAc) (which you calculate from the 5% and the density but I don't know that it is 1M). Is there something else in the problem?

1. 👍
2. 👎

## Similar Questions

1. ### Chemistry

Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of

2. ### chemistry

Vinegar is a solution of acetic acid, a weak acid. How can you produce more acetate ions in the solution? CH 'subtext' 3 COOH(aq) H+(aq) + CH 'subtext' 3 COO^- (aq) A. Evaporate some of the water. B. Decrease the pressure. C.

3. ### Chemistry

Assuming the density of vinegar is 1.0 g/mL ' what is the molarity of vinegar? (use the percent by mass of acetic acid to vinegar which is 5%.) The molar mass of acetic acid is 60.05 g/mol?

4. ### chemistry

1. When performing this experiment, a student mistakenly used impure KHP to standardize the NaOH solution. If the impurity is neither acidic nor basic, will the percent by mass of acetic acid in the vinegar solution determined by

1. ### 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? B. If the density of the vinegar

2. ### Chemistry

If acetic acid is the only acid that vinegar contains [Ka = 1.8*10-5] , calculate the concentration of acetic acid in the vinegar. pH of vinegar is 3.20 _______________ First I got the antilog of the pH given, which turned out to

3. ### Gr 11 Chemistry-Dilutions

The cafeteria decides to save money by using concentrated acetic acid (CH3COOH at 17.5 mol/L) and diluting it with water toproduce vinegar (5.00% m/v aceticacid). a) What is the concentration of vinegar in mol/L?b) What volume of

4. ### chem

vinegar is 5.0% acetic acid, CH3COOH, by mass. vinegar has a density of 1.02 g/ml what is the madd of acetic acid in 50.0 ml of vinegar?

1. ### chemistry

vinegar is made by adding 33 g of acetic acid to 625 if water what is the percent by mass of acetic acid in this solution of vinigar

2. ### chemistry

Calculate the mole fraction of acetic acid in vinegar, assuming that vinegar is 5.00% acetic acid(by mass) and that the density of vinegar is 1.05 g/mL

3. ### Chemistry

You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 5.00 using only pure acetic acid, 3.00 M NaOH, and water. Calculate the quantities needed for each of the following steps in the buffer preparation. 1. Add acetic

4. ### Chemistry

1. Commercial vinegar is a solution of acetic acid in water. How would you determine which brand of vinegar contains more acetic acid in a given volume of vinegar?