Question

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?

Answer 1

Mass of Ca(OH)₂ required = 0.09 g

Step-by-step explanation:

Given data:

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