What mass of barium hydroxide can be neutralized with 126 g of a nitric acid solution with a solute mass fraction of 15%?

| February 19, 2021 | education

Let’s write down the reaction scheme and arrange the coefficients:
Ba (OH) 2 + 2HNO3 = Ba (NO3) 2 + 2H2O
We find the mass of nitric acid m (HNO3) = w * m (solution), where w is the mass fraction of nitric acid, m (solution) is the mass of the solution of nitric acid.
m (HNO3) = 0.15 * 126 = 18.9 g
Find the amount of substance n (HNO3) = m (HNO3) / M (HNO3), where M (HNO3) = 63 g / mol is the molar mass of nitric acid
n (HNO3) = 18.9 / 63 = 0.3 mol
It can be seen from the reaction equation that the neutralization of 1 mol of barium hydroxide requires 2 mol of nitric acid, thus n (Ba (OH) 2) = n (HNO3) / 2 = 0.3 / 2 = 0.15 mol
Find the mass of barium hydroxide m (Ba (OH) 2) = n (Ba (OH) 2) * M (Ba (OH) 2), where M (Ba (OH) 2) = 171 g / mol
m (Ba (OH) 2) = 0.15 * 171 = 25.65 g



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