solutions concentration of solutions. objectives 1.define molarity and calculate its value. 2.define...
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Solutions
Concentration of Solutions
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Objectives
1. Define molarity and calculate its value.
2. Define molality and calculate its value.
3. Apply the principles of stoichiometry to reactions that occur in solution.
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Concentration
Dilute vs. Concentrated
Weak acid vs. dilute acid
Concentration – a measure of the amount of solute in a given amount of solvent or solution
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MolarityMolarity – the number of moles of solute in 1 liter of solution.
• Dissolving 2 moles of NaOH (80.0g) in enough water to make 1 Liter of solution would yield a 2 M solution of NaOH
)(
)()(
Lsolutionofvolume
molessoluteofamountMmolarity
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Sample Problems1. What is the molarity of a 2.0 L solution that is made
from 14.6 g of NaCl?0.12 M
2. What is the molarity of a HCl solution that contains 10.0 g of HCl in 250 mL of solution?1.1 M
3. How many moles of NaCl are in 1.25 L of 0.330 M NaCl?0.413 mol
4. How many moles of HCl exist in 500. mL of 0.50 M solution of HCl?0.25 mol
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Sample Problems5. What is the molarity of a solution composed of 6.25 g
of HCl in 0.300 L of solution?
0.571 M
6. How many moles of KI are present in 0.250 L of a 2.30 M solution?
0.575 mol
7. What volume of a 0.500 M solution of HBr is needed for a reaction that requires 32.5 g of HBr?
0.803 L
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MolalityMolality – concentration in moles of solute per kilogram of
solvent.
To make a 2.00 m solution of NaOH:• Measure 2 moles of NaOH (80.0 g) and dissolve in
1.00 kg of distilled water.
solventofkg
soluteofmolesmmolality )(
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)(
)()(
Lsolutionofvolume
molessoluteofamountMmolarity
solventofkg
soluteofmolesmmolality )(
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Sample Problems1. What is the molality of a solution composed of 255 g of
acetone (CH3)2CO) dissolved in 200. g of water?22.0 m
2. What quantity in grams of methanol (CH3OH) is required to prepare a 0.244 m solution in 400. g of water?3.12 g
3. How many grams of AgNO3 are needed to prepare a 0.125 m solution in 250 mL of water?5.3 g
4. What is the molality of a solution containing 18.2 g HCl and 250. g of water?1.99 m
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Solution concentration and Stoichiometry
How many moles of H2O form when 25.0 mL of 0.100 M HNO3 solution is completely neutralized by NaOH?
2.50 x 10-3 mol
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Stoichiometry Problems
1. What volume of 0.500 M HCl(aq) is required to react completely with 0.100 mol of Pb(NO3)2 (aq) forming a precipitate of PbCl2 (s)?
0.400 L
2. A 238 mL sample of hydrosulfuric acid solution requires 155 mL of a 3.45 M potassium hydroxide for complete neutralization. What is the concentration of the original hydrosulfuric acid solution?
1.12 M