Ch. 11 Notes

# Ch. 11 Notes - 11 Reactions in Aqueous Solutions II:...

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1 11 Reactions in Aqueous Solutions II: Calculations

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2 Chapter Goals
3 Calculations Involving Molarity • Example 11-1: If 100.0 mL of 1.00 M NaOH and 100.0 mL of 0.500 M H 2 SO 4 solutions are mixed, what will the concentration of the resulting solution be? • What is the balanced reaction? – It is very important that we always use a balanced chemical reaction when doing stoichiometric calculations.

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4 Calculations Involving Molarity Reaction Ratio: 2 mmol 1 mmol 1 mmol 2 mmol Before Reaction: 100 mmol 50 mmol 0 mmol 0 mmol After Reaction: 0 mmol 0 mmol 50 mmol 100 mmol
5 Calculations Involving Molarity • What is the total volume of solution? 100.0 mL + 100.0 mL = 200.0 mL • What is the sodium sulfate amount, in mmol? 50.0 mmol • What is the molarity of the solution? M = 50 mmol/200 mL = 0.250 M Na 2 SO 4

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6 Calculations Involving Molarity • Example 11-2: If 130.0 mL of 1.00 M KOH and 100.0 mL of 0.500 M H 2 SO 4 solutions are mixed, what will be the concentration of KOH and K 2 SO 4 in the resulting solution? • What is the balanced reaction?
7 Calculations Involving Molarity Reaction Ratio: 2 mmol 1 mmol 1 mmol 2 mmol Before Reaction: 130.0 mmol 50.0 mmol 0 mmol 0 mmol After Reaction: 30.0 mmol 0 mmol 50.0 mmol 100.0 mmol

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8 Calculations Involving Molarity • What is the total volume of solution? 130.0 mL + 100.0 mL = 230.0 mL • What are the potassium hydroxide and potassium sulfate amounts? 30.0 mmol & 50.0 mmol • What is the molarity of the solution? M = 30.0 mmol/230.0 mL = 0.130 M KOH M = 50.0 mmol/230.0 mL = 0.217 M K 2 SO 4
9 Calculations Involving Molarity

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10 Calculations Involving Molarity
11 Titrations Acid-base Titration Terminology Titration A method of determining the concentration of one solution by reacting it with a solution of known concentration. Primary standard A chemical compound which can be used to accurately determine the concentration of another solution. Examples include KHP and sodium carbonate. Standard solution A solution whose concentration has been determined using a primary standard. Standardization The process in which the concentration of a solution is determined by accurately measuring the volume of the solution required to react with a known amount of a primary standard.

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12 Titrations Acid-base Titration Terminology Indicator A substance that exists in different forms with different colors depending on the concentration of the H + in solution. Examples are phenolphthalein and bromothymol blue. Equivalence point The point at which stoichiometrically equivalent amounts of the acid and base have reacted.
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## This note was uploaded on 09/20/2009 for the course CHEM 344 taught by Professor Denniston during the Spring '09 term at UGA.

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Ch. 11 Notes - 11 Reactions in Aqueous Solutions II:...

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