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What is the molarity of the resulting solution when 45.0 mL of a 1.90 M H2SO4 solution is added to 95.0 mL of 0.600 M H2SO4

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When 45.0 mL of a 1.90 M H₂SO₄ solution is added to 95.0 mL of 0.600 M H₂SO₄the molarity of the resulting solution is 0.95 M.

To answer the question, we need to know what molarity is.

What is molarity of a solution?

Molarity is the number of moles per unit volume with volume in liters.

To find the molarity of the resulting solution, we need to find the number of moles in each solution.

Number of moles, n = MV where

  • M = molarity of solution and
  • V = volume

Number of moles in first solution

Given that we have 45.0 mL of a 1.90 M H₂SO₄ solution.

M' = 1.90 M and V' = 45.0 mL = 0.045 L

So, n' = M'V'

= 1.90 M × 0.045 L

= 0.0855 mol

Number of moles in second solution

Given that we have 95.0 mL of 0.600 M H₂SO₄ solution.

M" = 0.600 M and V" = 95.0 mL = 0.095 L

So, n" = M"V"

= 0.600 M × 0.095 L

= 0.057 mol

Number of moles in resulting solution

The number of moles in the resulting solution is n'" = n' + n"

= 0.0855 mol + 0.057 mol

= 0.1425 mol

Volume of the resulting solution

The volume of the resulting solution is V"' = V' + V"

= 45.0 mL + 95.0 mL

= 150.0 mL

= 0.15 L

The molarity of the resulting solution

The molarity of the resulting solution is M'" = n"'/V"'

= 0.1425 mol/0.15 L

= 0.95 mol/L

= 0.95 M

So, the molarity of the resulting solution is 0.95 M.

Learn more about molarity here:

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