Question

What is the molarity of a solution in which 10.0 g of $AgN{{O}_{3}}$ is dissolved in 500.0 ml of solution?

Answer 1

Molarity is also called as the concentration of the solution. To calculate the concentration we have to calculate the number of moles of the solute and later we have to calculate the concentration using the volume of the solvent.

Complete answer:
- In the question it is asked to calculate the molarity of a solution which contains 10 g of silver nitrate in 500 ml of water.
- First we have to calculate the number of moles of the solute by using the weight and molecular weight of the silver nitrate.
- The weight of the silver nitrate given is 10.0 gm.
- The molecular weight of the silver nitrate is 169.87 gm.
- Therefore the number of moles of the silver nitrate can be calculated as follows.
Number of moles of silver nitrate =$\dfrac{\text{weight of the silver nitrate}}{\text{molecular weight of the silver nitrate}}=\dfrac{10}{169.87}=0.05887moles$
- Therefore the number of moles of silver nitrate is 0.05887 moles.
- By using the number of moles we can calculate the concentration of the silver nitrate in 500 ml of water.
- The concentration of the silver nitrate is $=\dfrac{0.05887}{500}=0.118M$
- Therefore the molarity of the 10 gm of silver nitrate in 500 ml of water is 0.118 M.

Note:
First we have to calculate the number of moles of the solute by using the molecular weight of the solute and later we have to calculate the molarity or concentration of the solute in the given volume of water.