How many mL of 0.100 M NaOH is required to react with 50.0 mL of 0.100M H2SO4 ac

Question

How many mL of 0.100 M NaOH is required to react with 50.0 mL of 0.100M H2SO4 according to the reaction shown?

2 NaOH + H2SO4------>2H2O + Na2SO4

A.50
B.100
C.150
D.200
E.300

Explanation / Answer

You have to take into accout the ratio the reagents react in. So first write a balanced equation H2SO4 + 2NaOH -----> Na2SO4 + 2H2O You can see that you need 2 moles of NaOH to neutralise 1 mole of H2SO4 moles H2SO4 used = molarity x Litres = 0.100 M x 0.0500 L = 0.00500 moles H2SO4 You need 2 moles NaOH for every 1 mole H2SO4 So moles NaOH needed = 2 x moles H2SO4 = 0.01000 moles NaOH needed Volume NaOH needed = moles / molarity = 0.01000 mol / 0.100 M = 0.0100 L = 100.0 ml

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