A typical vinegar solution sold at the store is 5% by mass of acetic acid, with

Question

A typical vinegar solution sold at the store is 5% by mass of acetic acid, with a pH of 2.4. Calculate the concentrations of all the species in this solution. The molar mass of acetic acid (CH3COOH) is 60.06 g/mol.
Confused on how to find CH3COOH concentration.. A typical vinegar solution sold at the store is 5% by mass of acetic acid, with a pH of 2.4. Calculate the concentrations of all the species in this solution. The molar mass of acetic acid (CH3COOH) is 60.06 g/mol.
Confused on how to find CH3COOH concentration..
Confused on how to find CH3COOH concentration..

Explanation / Answer

Recall

pH = -log([H+])

[H+] = 10^-pH = 10^-2.4 = 0.003981

so

CH3COOH <-> H+ + CH3COO-

we need "M" molarity of acid

assume a bais of 1 Liter so 5 grams are present

mol acid = mass/MW = 5/60.06 = 0.083250 mol

M = mol/V = 0.083250/1 = 0.083250

in equilibrium:

[H+] = [CH3COO-] = 0.003981 M

[CH3COOH] = 0.083250-0.003981 = 0.079269 M

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