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If a student is titrating 10.0 mL of 1 M HNO3 with 1M NaOH and another students is titrating 10.0 mL of 1 M H2SO4 with 1 M NaOH, would they need the same volume of NaOH to reach the equivalence point? Explain your answer.

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Eduard22sly

Given the two different titration reactions, the volume of NaOH required to reach the equivalence point of both reaction will be different.

Titration of HNO₃ and NaOH

Balanced equation

HNO₃ + NaOH —> NaNO₃ + H₂O

From the balanced equation above,

  • The mole ratio of the acid, HNO₃ (nA) = 1
  • The mole ratio of the base, NaOH (nB) = 1

How to determine the volume of NaOH

  • Volume of acid, HNO₃ (Va) = 10 mL
  • Molarity of acid, HNO₃ (Ma) = 1 M
  • Molarity of base, NaOH (Mb) = 1 M
  • Volume of base, NaOH (Vb) =?

MaVa / MbVb = nA / nB

(1 × 10) / (1 × Vb) = 1

10 / Vb = 1

Cross multiply

1 × Vb = 10

Vb = 10 mL

Titration of H₂SO₄ and NaOH

Balanced equation

H₂SO₄ + 2NaOH —> Na₂SO₄ + 2H₂O

From the balanced equation above,

  • The mole ratio of the acid, H₂SO₄ (nA) = 1
  • The mole ratio of the base, NaOH (nB) = 2

How to determine the volume of NaOH

  • Volume of acid, H₂SO₄ (Va) = 10 mL
  • Molarity of acid, H₂SO₄ (Ma) = 1 M
  • Molarity of base, NaOH (Mb) = 1 M
  • Volume of base, NaOH (Vb) =?

MaVa / MbVb = nA / nB

(1 × 10) / (1 × Vb) = 1/2

10 / Vb = 1/2

Cross multiply

1 × Vb = 10 × 2

Vb = 20 mL

Conclusion

  • Titration of HNO₃ and NaOH required 10 mL of NaOH
  • Titration of H₂SO₄ and NaOH required 20 mL of NaOH

From the above calculations, we can conclude that different volume of NaOH will be required for the different reaction.

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