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SolutionConcentration
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What is different between the glasses of Kool-aid?
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Solution concentration can be described generally
Dilute - reduced in strength, weak, watered down.
Concentrated – stronger, pure. Has less water.
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What is the problem with just using dilute and concentrated as descriptions of the
solution concentration?
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Is solution B dilute or concentrated?
The terms dilute and concentrated are relative.
Scientists need a more precise way of referring to the concentration of a solution.
Concentrated Dilute
Solution A Solution B Solution C
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Solution concentration can be described specifically
Do you remember the “mole” from Stoichiometry?
What is a mole?
How might you use it to describe the concentration of a solution?
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Concentration can be represented by…
•Molarity
•Molality
•Percent by Mass
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MolarityThe ratio of the moles of solute to
the volume of solution in liters.
Molarity (M) =Moles of solute
Volume in Liters of solution
Used for most chemistry calculations of concentration
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Molality
Molality = moles of solute per kg solvent
Molality (M) =Moles of solute
kilogram of Solvent
Used for chemistry when volume of solvent is not constant
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Percent by Mass
Percent by Mass = mass of solute divided by mass of total solution
% by mass =Mass (g) of solute
Mass of Solvent + Mass of Solute
Used for food, medicine, household cleaners and chemicals
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How to Calculate Dilutions
Using molarity to calculate dilutions is EASY. Moles stays the same Volume changes Molarity changes M1V1 = M2V2
Re-arrange to solve for the requested information
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How to read Molarity
6.0 M NaClRead: “6 molar solution of NaCl”Can be abbreviated 6M solution You must be careful to label the molarity
with a capital M so that it is not confused with m for molality.
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How to make a solution using molarity (6M NaCl)
(a) Add 6 moles NaCl to the volumetric flask. How would you measure that?
6moles NaCl 58.443 g NaCl
1 mole NaCl
= 351 g NaCl
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How to make a solution using molarity (6M NaCl)
(b) Add dH2O to dissolve and mix the NaCl
(c) Fill the flask with dH2O until you reach the 1000mL line.
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Types of Calculations with Molarity:
1. Finding concentration of a solution.2. Finding the mass of solute needed.3. Finding the volume of solution made.
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Finding Concentration
Antifreeze is a solution of ethylene glycol, C2H6O2 in water. If 4.50 L of antifreeze contains 27.5 g of ethylene glycol, what is the concentration of the solution?
27.5 g C2H6O2
62.08 g C2H6O2
1 mol C2H6O2
4.5 L
= 0.0984 mol/L or
0.0984 M C2H6O2
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Finding Mass
What mass of sodium carbonate, Na2CO3, is present in 50 ml of a 0.750M solution?
50 ml 1 L
1000 mL
0.750 mol
1 L 1 mol Na2CO3
105.99 g Na2CO3
= 3.97 g Na2CO3
Conversion Factor
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Finding Volume
What volume of 1.50 mol/L HCl solution contains 10.0 g of hydrogen chloride?
10.0 g HCl 1 mol HCl
36.46 g HCl 1.50 mol
1 L
= 0.183 L or 183 mL
Conversion Factor
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Practice Problems
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Practice Problems
1. A 0.750 L aqueous solution contains 90.0 g of ethanol, C2H5OH. Calculate the molar
concentration of the solution in mol·L-1.
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Practice Problem
2. What mass of NaCl are dissolved in 152 mL of a solution if the concentration of the solution is 0.364 M?
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Practice Problem
3. What mass of dextrose, C6H12O6 is dissolved in 325 mL of 0.258 M solution?
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Practice Problem
4. A mass of 98 g of sulfuric acid, H2SO4, is dissolved in water to prepare a 0.500 M solution. What is the volume of the solution?
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Practice Problem
5. A solution of sodium carbonate, Na2CO3, contains 53.0 g of solute in 215 mL of solution. What is its molarity?
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Practice Problem
6. What is the molarity of a solution of HNO3 that contains 12.6 g of solute in 5.00 L of solution?