Solution Stoichiometry Introduction, Concentration of a solution.
Solution Concentration
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Transcript of Solution Concentration
Solution Concentration
Review
A solution is a homogeneous mixture.The solvent is the major component of the
solution.The solute is the minor component and
active ingredient.A saturated solution holds the maximum
amount of solute that is theoretically possible for a given temperature.
How would you describe this picture?
Solution Concentration
Is one glass of tea stronger than the other?– What’s true about the “stronger” glass of tea?– How much tea does it have in it compared to
the other glass?
Solution Concentration
Concentration – a ratio comparing the amount of solute to the amount of solution.
Many ways of expressing concentration:– % by weight (% w/w)– % by volume (% v/v)– parts per million (ppm) or parts per billion
(ppb) for very low concentrations– molality (m)– Molarity (M)
Concentrated vs. Dilute
The words “concentrated” and “dilute” are opposites.
EX: The dark tea is more concentrated than the light tea.
EX: The light tea is more dilute than the dark tea.
Concentrated vs. Dilute
Concentrated solution
Dilute solution
= solute particles
Percent by Weight
% by weight (% w/w)
What is the % w/w of a solution if 3.00 grams of NaCl are dissolved in 17.00 g of water?– mass of solute = 3.00 g
– mass of solution = 3.00 g + 17.00 g = 20.00 g
– (3.00 g / 20.00 g) x 100% = 15.0% w/w
100% x solution of mass total
solute of mass %w/w
Percent by Volume
% by volume (% v/v)
What is the % v/v of a solution if 20.0 mL of alcohol are dissolved in 50.0 mL of solution?– volume of solute = 20.0 mL
– volume of solution = 50.0 mL
– (20.0 mL / 50.0 mL) x 100% = 40.0%
100% x solution of volume total
solute of volume %v/v
Molarity
Molarity (M)
– UNITS: mol/L or Molar (M)
– Example: 0.500 mol/L = 0.500 M
solution of Liters
solute of moles Molarity
Molarity
What is the Molar concentration of a sol’n if 20.0 grams of KNO3 (MM = 101.11 g/mol) is dissolved in enough water to make 800. mL?
– Convert g of KNO3 to mol of KNO3
– Convert mL to L
33
33 KNO mol 0.198
KNO g 101.11
KNO mol 1 x KNO g 20.0
L 0.800 mL 1
L 0.001 x mL 800.
Molarity
What is the Molar concentration of a sol’n if 0.198 mol KNO3 is dissolved in enough water to make 0.800 L?
M 0.248L 0.800
KNO mol 0.198 Molarity 3
Molarity
What is the Molar concentration of a sol’n if 10.5 grams of glucose (MM = 180.18 g/mol) is dissolved in enough water to make 20.0 mL of sol’n?– Convert g of glucose to mol of glucose.
– Convert mL to L.
glucose mol 0.0583 glucose g 180.18
glucose mol 1 x glucose g 10.5
L 0.0200 mL 1
L 0.001 x mL 20.0
Molarity
What is the Molar concentration of a sol’n if 0.0583 mol of glucose is dissolved in enough water to make 0.0200 L of sol’n?
M 2.92 L 0.0200
glucose mol 0.0583 Molarity
Calculating Grams
How many grams of KI (MM = 166.00 g/mol) are needed to prepare 25.0 mL of a 0.750 M solution?
– Convert mL to L.
– Solve for moles.
– moles of KI = 0.750 M x 0.0250 L = 0.0188 mol KI
L 0.0250 mL 1
L 0.001 x mL 25.0
L 0.0250
KI of moles x M 0.750
Calculating Grams
How many grams of KI (MM = 166.00 g/mol) are needed to prepare 25.0 mL of a 0.750 M solution?
– Convert 0.0188 mol KI to grams.
KI g 3.12 KI mol 1
KI g 166.00 x KI mol 0.0188
Calculating Grams
How many grams of HNO3 (MM = 63.02 g/mol) are present in 50.0 mL of a 1.50 M sol’n?– Convert mL to L.
• 50.0 mL = 0.0500 L
– Solve for moles:• moles = (1.50 M)(0.0500 L) = 0.0750 mol HNO3
– Convert 0.0750 mol HNO3 to grams:
• 0.0750 mol HNO3 = 4.73 g HNO3
Dilution
Dilute (verb) - to add solvent to a solution.– Decreases sol'n concentration.
– M1V
1 = M
2V
2
• M1 = initial conc.
• V1 = initial volume
• M2 = final conc.
• V2 = final volume
– Assumes no solute is added.
Dilution
Stock SolutionImpractically
High Concentration
Usable Solution
Add H2O
Question for Consideration: Why do you think chemical supply companies typically sell acids (and other solutions) in extremely high concentrations when it would be safer to ship more dilute solutions?
Dilution
To what volume should 40.0 mL of 18 M H2SO
4
be diluted if a concentration of 3.0 M is desired?– What do we want to know?
• V2
– What do we already know?• M
1 = 18 M
• V1 = 40.0 mL
• M2 = 3.0 M
– (18 M)(40.0 mL) = (3.0 M)V2
– 720 M*mL = (3.0 M)V2
– V2 = 240 mL
Dilution
You are asked to prepare 500. mL of 0.250 M HCl, starting with a 12.0 Molar stock sol'n. How much stock should you use?– What do we want to know?
• V1
– What do we already know?• M
1 = 12.0 M
• M2 = 0.250 M
• V2 = 500. mL
– (12.0 M) V1 = (0.250 M)(500. mL)
– (12.0 M) V1 = 125 M*mL
– V1 = 10.4 mL
To how much water should you add 20.0 mL of 5.00 M HNO
3 to dilute it to 1.00 M?
– What do we want to know?• How much water to add. (V
2 - V
1)
– What do we already know?• M
1 = 5.00 M
• V1 = 20.0 mL
• M2 = 1.00 M
– (5.00 M)(20.0 mL) = (1.00 M) V2
– 100. M*mL = (1.00 M) V2
– V2 = 100. mL
– Water added = 100. mL - 20.0 mL = 80. mL
Dilution
Colligative Properties
Colligative properties are properties of solutions that are affected by the number of particles but not the identity of the solute
Boiling Point Elevation: A Colligative Property
Boiling point elevation is the temperature difference between a solution and pure solvent
The value of the boiling point elevation is directly proportional to molality, meaning the greater the number of solute particles, the greater the elevation
Freezing Point Depression: A Colligative Property
Freezing point depression is the difference in temperature between a solution and a pure solvent
The value of freezing point depression is directly proportional to molality, meaning the greater the number of solute particles