Given the following balanced chemical equation:

Ca (OH) 2 (s) + 2HNO3 (aq) → Ca (NO) 3 (aq) + 2H2O (l)

How many grams of Ca (OH) 2 are required to neutralize 25.0 ml of 0.100 M HNO3?

Mass of Ca (OH) ₂ required = 0.09 g

Explanation:

Given dа ta:

Volume of HNO₃ = 25 mL (25/1000 = 0.025 L)

Molarity of HNO₃ = 0.100 M

Mass of Ca (OH) ₂ required = ?

Solution:

Chemical equation;

Ca (OH) ₂ + 2HNO₃ → Ca (NO) ₃ + 2H₂O

Number of moles of HNO₃:

Molarity = number of moles / volume in L

0.100 M = number of moles / 0.025 L

Number of moles = 0.100 M * 0.025 L

Number of moles = 0.0025 mol

Now we will compare the moles of Ca (OH) ₂ with HNO₃ from balance chemical equation.

HNO₃ : Ca (OH) ₂

2 : 1

0.0025 : 1/2*0.0025 = 0.00125

Mass of Ca (OH) ₂:

Mass = number of moles * molar mass

Mass = 0.00125 mol * 74.1 g/mol

Mass = 0.09 g