Question

# How many milliliters of .405 Ba(OH)2 solution are required to completely react with 17.5 milliliters of...

How many milliliters of .405 Ba(OH)2 solution are required to completely react with 17.5 milliliters of .244M HCl according to the balanced chemical equation? (your answer should have 3 significant figures and not include units)

2 HCl + Ba(OH)2 --> 2 H2O + BaCl2

#### Homework Answers

Answer #1

Number of moles of HCl = molarity * volume of solution in L

Number of moles of HCl = 0.244 * 0.0175 L = 0.00427 mole

From the balanced equation we can say that

2 mole of HCl requires 1 mole of Ba(OH)2 so

0.00427 mole of HCl will require

= 0.00427 mole of HCl *( 1 mole of Ba(OH)2 / 2 mole of HCl)

= 0.00214 mole of Ba(OH)2

Molarity of Ba(OH)2 = number of moles of Ba(OH)2 / volume of solution in L

0.405 = 0.00214 / volume of solution in L

volume of solution in L = 0.00214 / 0.405 = 0.00528 L

1 L = 1000 mL

0.00528 L = 5.28 mL

Therefore, volume of Ba(OH)2 solution = 5.28 mL

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