given a 5.0 g sample of a vinegar having a mass percentage of acetic acid equal...

given a 5.0 g sample of a vinegar having a mass percentage of acetic acid equal to 9.1%(m/m), calculate what volume of NaOH solution of molarity 0.82M will be necessary to threats this vinegar sample.

Solutions

Expert Solution

As we know that vinegar is a consist of an acetic acid, water and other traces of compounds. So when we will add NaOH to vinegar the acid-base reaction will occur.

Since NaOH is a strong base and acetic acid is weak acid so Strong base - weak acid reaction.

NaOH will threat completely acetic acid completely when NaOH will neutralize an acetic acid and Ph will be less than 7.

we know that

mass of acetic acid = (9.1/100)*5 = .455g

So, mole of acetic acid = 0.455g/60g = 0.00758 and

vinegar contains mostly by acetic acid and water

therefor remaining weight = mass of water = 5 - 0.455g = 4.545g

because vinegar is a liquid solution

therefor at neutralization point

M1*V1 = M2*V2 (M1 = molarity of NaOH, M2 = Molarity of acetic acid )

( V1 = volume of NaOH solution, V2 valume of acetic acid solution)

0.82*V1 = (0.00758/V2)*V2

=> V1 = 0.00758/0.82 = 0.009243L

V1 = 9.243ml = answer

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

The vinegar sold in the grocery stores is described as 5.0%(V/V) acetic acid? What is the...

The vinegar sold in the grocery stores is described as 5.0%(V/V) acetic acid? What is the molarity of this solution (density of 100% acetic acid is 1.05 g/mL)? What is the mass % of acetic acid in this solution (density of vinegar is 1.01 g/mL)? What is the mole fraction of acetic acid in this solution? What is the molality of this solution? Please explain as you solve

Sally chemist is attempting to determine the mass % of acetic acid in vinegar. Below is...

Sally chemist is attempting to determine the mass % of acetic acid in vinegar. Below is an excerpt from her lab book: A. Prepared vinegar analyte 25.0 mL vinegar mass of vinegar 25.20 grams added 75.0 mL H2O added 2 drops phenolphthalein temperature: 27.0 oC manufacturer's mass % acetic acid = 3.5 % B. Prepared burette filled with standardized NaOH solution 0.201 M C. Titration initial burette reading: 5.12 mL final burette reading: 78.67 mL solution is light pink 1....

A food chemist determines the concentration of acetic acid in a sample of apple cider vinegar...

A food chemist determines the concentration of acetic acid in a sample of apple cider vinegar by acid-base titration. What is the concentration of acetic acid in the vinegar if the density of the sample is 1.01 g/ml, the titrant is 1.002M NaOH and the average volume of titrant required to titrate 25.00 mL subsamples of the vinegar is 20.78mL? Express your answer the way a food chemist probably would; *as percent by mass*

The distinctive odor of vinegar is due to acetic acid, HC2H3O2. Acetic acid reacts with sodium...

The distinctive odor of vinegar is due to acetic acid, HC2H3O2. Acetic acid reacts with sodium hydroxide in the following fashion: HC2H3O2(aq) + NaOH(aq)-> H2O(l) + NaC2H3O2(aq). If 2.52 mL of vinegar requires 34.9 mL of 0.1031 M (molarity) NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00 qt sample of this vinegar? (1 L = 1.0567 qt)

After reacting 1.45 g of salicylic acid with 5.0 mL of acetic anhydride, 1.75 g of...

After reacting 1.45 g of salicylic acid with 5.0 mL of acetic anhydride, 1.75 g of acetylsalicylic acid is obtained. What is the calculated percent yield? Provide your answer to the correct number of significant figures.

A commercial brand of white vinegar contains 5.38 g of acetic acid per 100 mL of...

A commercial brand of white vinegar contains 5.38 g of acetic acid per 100 mL of vinegar. You pipet 10.00 mL of that vinegar into a 100 mL volumetric flask, add water to the mark, and mix. You then pipet 10.00 mL of the diluted vinegar into a flask and titrate with 0.1014 M NaOH. What volume (in mL) of 0.1014 M NaOH should you expect to need to use to reach the endpoint of the titration?

A commercial brand of white vinegar contains 5.38 g of acetic acid per 100 mL of...

A commercial brand of white vinegar contains 5.38 g of acetic acid per 100 mL of vinegar. If you titrate a 10.00 mL sample of undiluted vinegar, what volume (in mL) of 0.1014 M NaOH should you expect to need to use to reach the endpoint of the titration?

A commercial brand of white vinegar contains 5.38 g of acetic acid per 100 mL of...

Mass (g) of salicylic acid 2.0083 Volume (mL) of acetic anhydride used 3.01 Mass (g) of...

Mass (g) of salicylic acid 2.0083 Volume (mL) of acetic anhydride used 3.01 Mass (g) of filter paper 0.4629 Mass (g) of watch glass 29.6710 Mass (g) of watch glass, filter paper and aspirin 30.5178 Mass of aspirin: 0.3839 Maximum amount (g) of aspirin possible if salicylic acid is the Limiting Reagent: ? Maximum amount (g) of aspirin possible if acetic anhydride is the Limiting Reagent: ? Maximum amount (g) of aspirin possible (the Theoretical Yield): ? Percent Yield (%)...

A 15.3 mL sample of vinegar, containing acetic acid, was titrated using 0.809 M NaOH solution....

A 15.3 mL sample of vinegar, containing acetic acid, was titrated using 0.809 M NaOH solution. The titration required 24.06 mL of the base. Assuming the density of the vinegar is 1.01 g/mL, what was the percent (by mass) of acetic acid in the vinegar?

Subjects