Question

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

Answer 1

To neutralize the given volume of HNO3, you need to determine the number of moles of HNO3 and then use the balanced chemical equation to find the number of moles of Ca(OH)2 required. Given the volume and concentration of HNO3, the number of moles of HNO3 can be calculated as 0.00250 moles. Using the balanced chemical equation and the number of moles of HNO3, the number of moles of Ca(OH)2 can be determined as 0.00125 moles. Finally, the mass of Ca(OH)2 is calculated as 0.0926 g.

Step-by-step explanation:

To neutralize the given volume of HNO₃, we need to determine the number of moles of HNO₃ and then use the balanced chemical equation to find the number of moles of Ca(OH)₂ required.

Given: volume of HNO₃ = 25.0 ml, concentration of HNO₃ = 0.100 M

1. Convert the volume of HNO₃ to liters: 25.0 ml = 0.0250 L

2. moles of HNO₃ = 0.0250 L * 0.100 M = 0.00250 moles

3. Using the balanced chemical equation:

4. moles of Ca(OH)₂ = 0.00250 moles * (1 mole Ca(OH)₂ / 2 moles HNO₃) = 0.00125 moles

5. mass of Ca(OH)₂ = moles of Ca(OH)₂ * molar mass of Ca(OH)₂

   Using the molar mass of Ca(OH)₂ (74.1 g/mol):

   mass of Ca(OH)₂ = 0.00125 moles * 74.1 g/mol = 0.0926 g