introduction to solutions/acids and bases honors chemistry may 27 th, 2014
TRANSCRIPT
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INTRODUCTION TO SOLUTIONS/ACIDS AND BASES
HONORS CHEMISTRY
MAY 27TH, 2014
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WHAT IS A SOLUTION?
A solution is a homogenous mixture of to or more substances.
The most common solutions are aqueous solutions, those with a solid, liquid, or gas in water.
A solution has at least two components:
- Solvent: The majority component
- Solute: The minority component
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CONCENTRATION
The amount of solute in a solution is an important property of a solution.
A dilute solution contains small amounts of solute relative to solvent.
A concentrated solution contains large amounts of solute relative to solvent.
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MOLARITY
Molarity (M) is a way to express solution concentration.
Molarity is defined as the number of moles of solute per liter of solution.
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PREPARING A SOLUTIONNote that molarity is moles of solute/liters of solution, not solvent. To make a solution of a specific molarity, you usually put the solute into a flask and then add water to desired volume of solution.
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PRACTICE PROBLEMS!
Calculate the molarity of a solution made by putting 15.5 g of NaCl into a beaker and adding water to make 1.50L of NaCl solution.
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DILUTION EQUATION
M1V1 = M2V2 Where…
- M1 and V1 are the molarity and volume of the initial
concentrated solution
- M2 and V2 are the molarity and volume of the final diluted
solution
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PRACTICE PROBLEM
To what volume should you dilute 0.100 L of a 15 M NaOH solution to obtain a 1.0 M NaOH solution?
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SOLUTION STOICHIOMETRY Many chemical reactions take place in aqueous solutions. We know from stoichiometry that coefficients in chemical equations are conversion factors between moles of reactants and moles of products.
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PRACTICE PROBLEM!
How much 0.125 M NaOH solution do we need to completely neutralize 0.225 L of 0.175 M H2SO4 solution?