Nitric acid reacts with magnesium hydroxide according to the reaction below.2HNO3 (aq) + Cu(OH)2 (s) ⟶ Cu(NO3)2 (aq) + 2H2O (l)If 250.0 mL of a 0.125 M HNO3 solution is need to completely react with a sample of Cu(OH)2, what is the mass of Cu(OH)2 in the sample?

First, we need to determine the number of moles of HNO3. We can do this using the formula:

Molarity = moles/volume

Rearranging for moles gives us:

moles = Molarity * volume

Substituting the given values:

moles HNO3 = 0.125 M * 0.250 L = 0.03125 moles

From the balanced chemical equation, we know that the ratio of HNO3 to Cu(OH)2 is 2:1. Therefore, the moles of Cu(OH)2 is half the moles of HNO3.

moles Cu(OH)2 = 0.03125 moles / 2 = 0.015625 moles

Finally, we can find the mass of Cu(OH)2 by multiplying the number of moles by the molar mass of Cu(OH)2. The molar mass of Cu(OH)2 is approximately 97.56 g/mol.

mass Cu(OH)2 = 0.015625 moles * 97.56 g/mol = 1.525 g

So, the mass of Cu(OH)2 in the sample is approximately 1.525 g.