Help me solve this problem!!!

Question

You have found that 13.85mL of 0.112M sulfuric acid reacts with exactly 20.00mL of barium hydroxide solution of unknown concentration. What is the molarity of the barium hydroxide solution? Round your answer to 3 decimal places and include units.

Answer 1

H2SO4 + Ba(OH)2 ==> BaSO4 + 2H2O ... balanced equation

From the balanced equation you can see that ONE mol H2SO4 reacts with ONE mol Ba(OH)2. So, the number of moles of sulfuric acid will equal the moles of barium hydroxide.

moles H2SO4 = 13.85 mls x 1 L/1000 ml x 0.112 mols/L = 0.00155 mols

moles Ba(OH)2 = 0.00155 mols

Concentration of Ba(OH)2 = mols/liter

moles = 0.00155 mols

liters = 20.00 ml x 1 L/1000 mls = 0.0200 L

Concentration = 0.00155 mols / 0.0200 L = 0.0776 moles/liter = 0.078 moles/liter