Question

By titration, 12.5 mL of aqueous H2SO4 neutralized 16.8 mL of 0.015 M LiOH solution.

What was the molarity of the aqueous acid solution? Answer in units of M

Answer 1

The molarity of the aqueous acid solution : 0.0101 M

Further explanation

Titration is a procedure for determining the concentration of a solution by reacting with another solution that is known to be concentrated (usually a standard solution). Determination of the endpoint/equivalence point of the reaction can use indicators according to the appropriate pH range

Acid-base titration formula

Ma. Va. na = Mb. Vb. nb

Ma, Mb = acid base concentration

Va, Vb = acid base volume

na, nb = acid base valence (amount of H⁺, OH⁻)

• a=H₂SO₄

Va=12.5 ml

na = 2 (H₂SO₄⇒2H⁺+SO₄²⁻⇒2 ion H⁺)

• b=LiOH

Mb=0.015

Vb=16.8 ml

nb = 1(LiOH⇒Li⁺+OH⁻⇒1 ion OH⁻)

The molarity of the acid(Ma) :

`\tt Ma* 12.5* 2=0.015* 16.8* 1\\\\Ma=(0.015* 16.8* 1)/(12.5* 2)\\\\Ma=0.0101`