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3 years ago

How many mL of 0.105 M aqueous NaOH solution are required to neutralize 40.0 mL of 0.210 M aqueous H2SO4 solution?

Chemistry

1 answer:

nevsk [136]3 years ago

7 0

Answer:

160 mL

Explanation:

Given data:

Molarity of NaOH = 0.105 M

Volume of H₂SO₄ = 40.0 mL (40.0/1000 = 0.04 L)

Molarity of H₂SO₄ = 0.210 M

Volume of NaOH required = ?

Solution:

Number of moles of of H₂SO₄:

Molarity = number of moles / volume in L

0.210 M = number of moles / 0.04 L

Number of moles = 0.210 mol/L × 0.04 L

Number of moles = 0.0084 mol

now we will compare the moles of H₂SO₄ with NaOH.

H₂SO₄ : NaOH

1 : 2

0.0084 : 2/1×0.0084 = 0.0168 mol

Volume of NaoH:

Molarity = number of moles / volume in L

0.105 M = 0.0168 mol / Volume in L

Volume in L = 0.0168 mol / 0.105 M

Volume in L = 0.16 L

Volume in mL:

0.16 L × 1000 mL/ 1L

160 mL

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