A 1.00mL vinegar sample was completely neutralized by 22.5mL 0.2 M NaOH solution. Calculate molarity and...

A 1.00mL vinegar sample was completely neutralized by 22.5mL 0.2 M NaOH solution. Calculate molarity and % of Acetic acid in vinegar.

Expert Solution

One mole NaOH reacts with one mole acetic acid.

So, the number of moles of acetic acid is equal to the number of moles of NaOH.

Moles of NaOH = Volume of NaOH x Molarity of NaOH = 22.5 mL x 0.2 M = 4.5 mmol

So, the number of moles of acetic acid is 4.5 mmol.

Molarity of acetic acid = moles of acetic acid/volume of vinegar = 4.5 mmol / 1.00 mL = 4.5 M

Mass of acetic acid = moles of acetic acid x molar mass of acetic acid

= 4.5 mmol x (60.05 g/mol) = 270 mg = 0.270 g

% of acetic acid in vinegar =( mass of acetic acid / volume of vinegar)x100

= 0.270 g/1.00 mL) x100

= 27%

queen_honey_blossom answered 2 years ago

what is the molarity of a HCl solution if a 10.0 mL sample is neutralized by...

what is the molarity of a HCl solution if a 10.0 mL sample is neutralized by a 44.3 mL of a 0.111 molar solution

Calculate the volume, in milliliters, of a 0.216 M NaOH solution that will completely neutralize each...

Calculate the volume, in milliliters, of a 0.216 M NaOH solution that will completely neutralize each of the following: 1.) 3.71 mL of a 1.32 M HNO3 solution. 2.) 8.10 mL of a 0.800 M H3PO4 solution.

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?

Exactly 47.0 mL of 0.2 M HNO2 are titrated with a 0.2 M NaOH solution. What...

Exactly 47.0 mL of 0.2 M HNO2 are titrated with a 0.2 M NaOH solution. What is the pH at the equivalence point ?

Calculate the volume of 0.820-M NaOH solution needed to completely neutralize 112 mL of a 0.620-M...

Calculate the volume of 0.820-M NaOH solution needed to completely neutralize 112 mL of a 0.620-M solution of the monoprotic acid HCl. __________ mL NaOH

1/ Calculate the volume of 0.280-M NaOH solution needed to completely neutralize 27.4 mL of a...

1/ Calculate the volume of 0.280-M NaOH solution needed to completely neutralize 27.4 mL of a 0.560-M solution of the monoprotic acid HBr. 2/ To determine the molar mass of an organic acid, HA, we titrate 1.047 g of HA with standardized NaOH. Calculate the molar mass of HA assuming the acid reacts with 37.17 mL of 0.469 M NaOH according to the equation HA(aq) + NaOH(aq) → NaA(aq) + H2O(ℓ) 3/ 2 NaBH4(aq) + H2SO4(aq) → 2 H2(g) +...

A student determined their NaOH molarity to be 0.0943 M. This solution was used to standardize...

A student determined their NaOH molarity to be 0.0943 M. This solution was used to standardize 25.00 mL of an HCl solution, requiring 25.73 mL to reach the equivalence point. The HCl solution was then used to determine the weight % of soda ash in 0.5102 g of an unknown sample, requiring 38.77 mL. If the determined NaOH concentration was 5.000% too low (relative error of -5%), how does it change the reported value of weight % soda ash?

Question

A 1.00mL vinegar sample was completely neutralized by 22.5mL 0.2 M NaOH solution. Calculate molarity and...

Solutions

Expert Solution

Related Solutions