Molarity Molality Dilutions

Concentration of Solute ,[object Object],Molarity ( M ) = moles solute liters of solution

1.0 L of water was used to make 1.0 L of solution. Notice the water left over.

PROBLEM: Dissolve 5.00 g of NiCl 2 •6 H 2 O in enough water to make 250 mL of solution. Calculate the Molarity. Step 1: Calculate moles of NiCl 2 •6H 2 O Step 2: Calculate Molarity [ NiCl 2 •6 H 2 O ] = 0.0841 M

[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],USING MOLARITY moles = M•V What mass of oxalic acid, H 2 C 2 O 4 , is required to make 250. mL of a 0.0500 M solution?

Learning Check ,[object Object],[object Object],[object Object],[object Object]

The Other Concentration Unit MOLALITY, m m of solution = mol solute kilograms solvent

Calculating Concentrations ,[object Object]

Try this molality problem ,[object Object],m = mol solute / kg solvent 25 g NaCl 1 mol NaCl 58.5 g NaCl = 0.427 mol NaCl Since the density of water is 1 g/mL, 5000 mL = 5000 g, which is 5 kg 0.427 mol NaCl 5 kg water = 0.0854 m salt water

Preparing Solutions ,[object Object],[object Object]

Dilutions ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Solving a dilution problem ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

M 1 V 1 =M 2 V 2 ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],M 1 V 1 =M 2 V 2

Molarity Molality Dilutions

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Molarity Molality Dilutions