Question

find the volume of .220 M hydrobromic acid necessary to react completely with 1.32 g of barium hydroxide

Answer 1

Consider reaction, 2 HBr (aq) + Ba(OH) ₂ (aq) BaBr ₂ (aq) + 2 H₂O (l)

From above reaction, stoichiometric ratio = No. of moles of acid / No. of moles of base = 2/1 = 2

we have correlation, No.of moles of acid = No. of moles of base stoichiometric ratio

Let's calculate no. of moles of Ba(OH) ₂.

We have , No. of moles = Mass / Molar mass

No. of moles of Ba(OH) ₂ = 1.32 g / ( 171.34 g /mol ) = 0.007704 mol

We have correlation, No. of moles of HBr = No. of moles of Ba(OH) ₂ stoichiometric ratio

No. of moles of HBr = 0.007704 mol 2 = 0.0154 mol

We have relation, [ HBr ] = No. of moles of HBr / volume of solution in L

Volume of HBr solution in L = No. of moles of HBr / [ HBr ]

Volume of HBr solution in L = 0.0154 mol / 0.220 mol / L

Volume of HBr solution in L = 0.070 L = 70 ml

ANSWER : 70 ml of 0.220 M HBr solution is required to completely react with 1.32 g Barium hydroxide solution.