According to the following reaction, how many grams of water are produced in the complete reaction of 31.8 grams of barium hydroxide?

Ba (OH) 2 (aq) + H2SO4 (aq) - -> BaSO4 (s) + 2H2O (l)

6.696 g of water (H₂O)

Explanation:

First we calculate the number of moles of barium hydroxide:

number of moles = mass / molecular weight

number of moles = 31.8 / 171.3 = 0.186 moles of barium hydroxide

Form the chemical reaction we may devise the following reasoning:

if 1 mole of barium hydroxide produces 2 moles of water

then 0.186 moles of barium hydroxide produces X moles of water

X = (0.186 * 2) / 1 = 0.372 moles of water

mass = number of moles * molecular weight

mass of water = 0.372 * 18 = 6.696 g