# What is the molarity of a solution in which 10.0g of AgNO_3 is dissolved in 500. mL of solution?

Mar 5, 2016

$\text{0.118 M}$

#### Explanation:

Molarity is simply a measure of the concentration of a solution in terms of how many moles of solute are present per liter of solution.

$\textcolor{b l u e}{| \overline{\underline{\text{molarity" = "moles of solute"/"liters of solution}}} |}$

This means that in order to find a solution's molarity you must know two things

• the number of moles of solute present
• the volume of the solution

In order to find the number of moles of silver nitrate, ${\text{AgNO}}_{3}$, present in that $\text{10.0-g}$ sample, use the compound's molar mass

10.0 color(red)(cancel(color(black)("g"))) * "1 mole AgNO"_3/(169.87color(red)(cancel(color(black)("g")))) = "0.05887 moles AgNO"_3

Now, do not forget that molarity is expressed per liter of solution. This means that you're going to have to convert the volume from milliliters to liters by using the conversion factor

$\text{1 L" = 10^3"mL}$

Plug in your values to get

$\textcolor{b l u e}{| \overline{\underline{c = {n}_{\text{solute"/V_"solution}}}} |}$

c = "0.05887 moles"/(500. * 10^(-3)"L") = color(green)(|bar(ul("0.118 M"))|)

The answer is rounded to three sig figs.