Question

Suppose 0.09886 M KOH is titrated into 15.00 mL H2SO4 of unknown concentration until the equivalence point is reached. It takes a total volume of 29.25 mL KOH to neutralize the H2SO4.

What is the concentration of the acid? Express the result to the proper number of significant figures based on the limits of data from the problem.

M acid

Answer 1

0.09639 M acid

Step-by-step explanation:

Answer 2

0.09639M

Step-by-step explanation:

Step 1:

The balanced equation for the reaction. This is given below:

H2SO4 + 2KOH —> K2SO4 + 2H2

The following were obtained from the balanced equation

Mole of the acid (nA) = 1

Mole of the base (nB) = 2

Step 2:

Data obtained from the question. This includes:

Concentration of acid (Ca) =?

Volume of acid (Va) = 15mL

Concentration of base (Cb) = 0.09886M

Volume of base (Vb) = 29.25mL

Step 3:

Determination of the concentration of the acid.

Applying the equation:

CaVa/CbVb = nA/nB

The concentration of the acid can be obtained as follow:

CaVa/CbVb = nA/nB

Ca x 15 / 0.09886 x 29.25 = 1/2

Cross multiply to express in linear form

Ca x 15 x 2 = 0.09886 x 29.25 x 1

Divide both side by 15 x 2

Ca = (0.09886 x 29.25) / (15 x 2)

Ca = 0.09639M

Therefore, the concentration of the acid is 0.09639M