Question

What volume requires a basic solution of 0.15 M sodium hydroxide to produce 135.0 g of...

What volume requires a basic solution of 0.15 M sodium hydroxide to produce 135.0 g of sodium sulfate to completely react with sulfuric acid? How many grams of sulfuric acid react?

Homework Answers

Answer #1

Volume can be calculated by :-

Concentration = 0.15 M = Number of moles of solute / Volume of solution in litres

Number of moles of solute = Actual mass (grams) / Molar Mass

The masses of reactants and products can be worked out from the equation:

H2SO4 + 2NaOH → Na2SO4 + 2H2O

98 + (2x40) = 142 + (2x18)

98 + 80 = 142 + 36

Now, 142g of Na2SO4 is made from 98g of H2SO4

         135g of Na2SO4 is made from 135 x (98 ÷ 142) = 93.169g of H2SO4

So, 93.169 grams of sulfuric acid react.

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