# Question 90d0d

May 25, 2017

$0.0738 \text{mol"/"L}$

#### Explanation:

To start, let's write the chemical equation for this reaction:

$\text{HNO"_3 "(aq)" + "LiOH (aq)" rarr "LiNO"_3 "(aq)" + "H"_2"O (l)}$

Let's find the number of moles of $\text{LiOH}$ reacting using the molarity equation.

$\text{mol LiOH" = (0.100 "mol"/cancel("L"))(0.03690cancel( "L")) = 0.00369 "mol LiOH}$

For this calculation, you would need to have converted from $\text{mL}$ to $\text{L}$, I just did not show it here (I'm assuming you know how to).

Since all the coefficients in the chemical equation are equal ($1$), the relative number of moles of that react is also $0.00369 \text{mol}$.

We now know the moles of ${\text{HNO}}_{3}$ and the volume of ${\text{HNO}}_{3}$ that reacted, so by using the molarity equation again, the molarity of the nitric acid solution is

M = (0.00369 "mol")/(0.0500 "L") = color(red)(0.0738 "mol"/"L"#