# Question #a1580

##### 1 Answer

#### Explanation:

The **molarity** of the solution essentially tells the *concentration* of the solute in terms of **moles per liter of solution**.

In other words, a solution's molarity tells you how many moles of solute you get in exactly **moles** of copper(I) nitrate **for every liter** of solution.

Now, use the **molar mass** of the compound to calculate how many moles you have in that sample

#6.58 color(red)(cancel(color(black)("g"))) * "1 mole CuNO"_3/(125.55color(red)(cancel(color(black)("g")))) = "0.05241 moles CuNO"_3#

Now all you have to do is use the molarity of the solution to figure out the volume needed to provide that many moles of solute

#0.05241 color(red)(cancel(color(black)("moles CuNO"_3))) * "1 L solution"/(0.150 color(red)(cancel(color(black)("moles CuNO"_3)))) = color(green)(bar(ul(|color(white)(a/a)color(black)("0.349 L")color(white)(a/a)|)))#

The answer is rounded to three **sig figs**.

If you want, you can convert the volume to *milliliters*

#0.349 color(red)(cancel(color(black)("L"))) * (10^3"mL")/(1color(red)(cancel(color(black)("L")))) = "349 mL"#