The volume of carbon dioxide required to react with 342 g of a 10% barium hydroxide solution

The volume of carbon dioxide required to react with 342 g of a 10% barium hydroxide solution to produce an acidic salt.

Let us find the mass of Ba (OH) 2 in solution.

W = m (substance): m (solution) × 100%,

m (substance) = (m (solution) × W): 100%.

m (Ba (OH) 2) = (342 g × 10%): 100% = 34.2 g.

Let’s find the amount of substance Ba (OH) 2.

M (Ba (OH) 2) = 171 g / mol.

n = m: M.

n (Ba (OH) 2) = 34.2 g: 171 g / mol = 0.2 mol.

Let’s compose the reaction equation, find the quantitative ratios of substances.

Ba (OH) 2 + 2CO2 = Ba (HCO3) 2.

According to the reaction equation, 1 mol of Ba (OH) 2 accounts for 2 mol of CO2. The substances are in quantitative ratios of 1: 2.

2n (Ba (OH) 2) = n (CO2) = 0.2 × 2 = 0.4 mol.

Let’s find the volume of CO2.

V = n Vn, where Vn is the molar volume of gas equal to 22.4 l / mol.

V = 0.4 mol × 22.4 L / mol = 8.96 L.

Answer: 8.96 liters.




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