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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.

Respuesta :

The chemical reaction between KOH and H2SO4 is:
2KOH + H2SO4 ⇒K2SO4 + 2H2O

According to the formula, at the end point where equivalence point is reached, the molar ratio between the reacted KOH and H2SO4 is 2:1. Based on this ratio, the concentration of the H2SO4 can be calculated.  Because all the measurement has 4 significant figures, we need to keep 5 significant figures during the calculation and 4 significant figures for the final answer.

The moles of KOH reacted is: 0.02925 L * 0.09886 M = 0.0028917 mole.
Based on the 2:1 ratio, the moles of H2SO4 in the solution is 0.0028917mole/2 = 0.0014458 mole.
So, the concentration of H2SO4 is: 0.0014458mole/0.01500L = 0.09639 mole/L, or 0.09639M.
Eduard22sly

The concentration of the acid, H₂SO₄ is 0.09639 M

Balanced equation

H₂SO₄ + 2KOH —> K₂SO₄ + 2H₂O

From the balanced equation above,

The mole ratio of the acid, H₂SO₄ (nA) = 1

The mole ratio of the base, KOH (nB) = 2

How to determine the concentration of H₂SO₄

  • Concentration of base, KOH (Cb) = 0.09886 M
  • Volume of acid, H₂SO₄ (Va) = 15 mL
  • Volume of base, KOH (Vb) = 29.25 mL
  • Concentration of acid, H₂SO₄ (Ca) =?

CaVa / CbVb = nA / nB

(Ca × 15) / (0.09886 × 29.25) = 1 / 2

(Ca × 15) / 2.891655  = 1 / 2

Cross multiply

Ca × 15 × 2 = 2.891655

Ca × 30 = 2.891655

Divide both side by 30

Ca = 2.891655 / 30

Ca = 0.09639 M

Thus, the concentration of the H₂SO₄ solution is 0.09639 M

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