Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.
Concept #1: Definition of Molarity
Anytime that you hear the term molarity used, just think that we are talking about how many moles of a solute are in a liter of solution.
Forgot what's the difference between a solute and a solution? Here's a reminder:
Concept #2: The difference between a solute and solvent
In a homogeneous mixture, the smaller amount is the solute, and the larger amount is the solvent. When dissolving a solute into a solvent they make a solution.
Example #1: 2.64 grams of an unknown compound was dissolved in water to yield 150 mL of solution. The concentration of the solution was 0.075 M. What was the molecular weight of the substance?
A concentrated solution can become a diluted solution with the addition of water.
Example #2: A solution is prepared by dissolving 0.1408 mol calcium nitrate, Ca(NO3)2, in enough water to make 100.0 mL of stock solution. If 20.0 mL of this solution is then mixed with an additional 90 mL of deionized water, calculate the concentration of the calcium nitrate solution.
We know how to calculate the molarity of a compound, but what do we do when we need the molarity of ions within the compound? Let's see.
Practice: What is the molarity of calcium ions of a 650 mL solution containing 42.7 g of calcium phosphate?
Now let's try connecting molarity with an equation from the past, density.
Practice: A solution with a final volume of 750.0 mL was prepared by dissolving 30.00 mL of benzene (C6H6, density = 0.8787 g/mL ) in dichloromethane. Calculate the molarity of benzene in the solution.