Question

86mL of an unknown base is titrated to equivalence with 4.3mL of 1M nitric acid solution. the reaction yields water and iron(II) nitrate salt. A. write a balanced equation for the neutralization reaction that occurs B. name the base found in the initial solution C. what is the molarity of the base solution?

Answer 1

Step-by-step explanation:

A. The balanced equation for the neutralization reaction that occurs is:

2 HNO3(aq) + Fe(OH)2(s) → Fe(NO3)2(aq) + 2 H2O(l)

B. Since the base reacts with nitric acid to form iron(II) nitrate, it must be a hydroxide of iron(II). Therefore, the base found in the initial solution is iron(II) hydroxide, Fe(OH)2.

C. To find the molarity of the base solution, we can use the balanced equation and the volume and concentration of the nitric acid solution used in the titration.

First, we need to determine the number of moles of nitric acid used in the titration. We can do this by multiplying the volume of the nitric acid solution by its concentration:

moles of HNO3 = 4.3 mL x 1 mol/L = 0.0043 mol

Since the balanced equation shows a 1:1 stoichiometric ratio between nitric acid and iron(II) hydroxide, we know that the number of moles of iron(II) hydroxide used in the titration is also 0.0043 mol.

Next, we can use the volume of the iron(II) hydroxide solution to calculate its concentration:

0.0043 mol / 0.086 L = 0.05 M

Therefore, the molarity of the iron(II) hydroxide solution is 0.05 M.