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 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    

- aluminum and copper chloride.

- the chloride ion to separate the aluminum from the oxygen so that the aluminum can react with the copper ions (and the water molecules).

the answer is 0.42 is that is an option. this question provides no info