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19.1 Acid-Base Theories> 3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day The pH for a 0.10 M solution of a monoprotic acid is 1.2, what is the K a ? 0.108
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1. What can you say about the Ka value of a strong acid?
2. In a 0.100 M solution of a monoprotic acid [H+] = 2.5 * 10-2 M. Calculate the Ka of this acid?
Day 4 4-30
8.33 * 10-3
3. The pH for a 0.20 M solution of a monoprotic acid is 2.5, what is the Ka? 5.08 * 10-5
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http://wps.prenhall.com/esm_brown_chemistry_9/2/660/169060.cw/index.html
Homework # 1 Chapter 16 – show me successful screen (100%) OR email to me – due Tues. 4-24
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Day 5 5-1
1. The pH for a 0.10 M solution of a monoprotic acid is 1.2, what is the Ka?
0.108
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Titration
Titration = the process of adding a measured amount of a solution of known concentration to a solution of unknown concentration – using a neutralization reaction to determine concentration
Steps:1. a measured volume of an acid solution of unknown concentration is added to a flask2. an indicator is added3. measured volumes of a base of known
concentration are mixed into the acid until the indicator just barely changes color
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Titration
The solution of known concentration is called the standard solution.
Neutralization occurs (titration is complete) when the number of hydrogen ions equals the number of hydroxide ions. = the equivalence point = end point
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Titration
Determining the concentration by titration mathematically:
Example: A 25 mL solution of H2SO4 is neutralized by 18 mL of 1.0 M NaOH. What is the concentration of the H2SO4 solution? The equation for the reaction is:
H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)
Conversion plan:you need mols H2SO4 to calculate molarity0.018 L NaOH mols NaOH mols H2SO4
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Titration
Determining the concentration by titration mathematically:
Additional Example: How many milliliters of 0.45 M HCl will neutralize 25.0 mL of 1.00 M KOH?
Period 1 stopped Wed. 5-1
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V. Salts in Solution
A. Salt Hydrolysis
Recall that some salts can hydrolyze water – remove hydrogen ions from or donate hydrogen ions to water (Hydrolysis of Salts Lab) salt hydrolysis.
salts that produce acidic solutions have positive ions that release hydrogen ions to water
salts that produce basic solutions have negative ions that attract hydrogen ions from water
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V. Salts in Solution
Example: ammonium chloride
Ammonium chloride completely ionizes in water:
NH4Cl(aq) NH+4(aq) + Cl-
(aq)
the ammonium ion is a strong enough acid to donate a hydrogen ion to a water molecule:
NH+4(aq) + H2O(l) NH3(aq) + H3O+
(aq)
the resulting H3O+ ions make the solution somewhat acidic
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V. Salts in Solution
Strong acid + Strong base neutral solution
Strong acid + Weak base acidic solution (salt’s cation releases hydrogens to water)
Weak acid + Strong base basic solution (salt’s anion attracts hydrogens from water)
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page 669 #s 27-34
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1.0 * 10-14
Arrhenius base
Amphoteric
Kb
Conjugate acid
Diprotic acid
Lewis acid
Self-ionization
Strong acid
Ka
Weak base
Bronsted-Lowry base
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1. HNO3 is a strong acid – assume it completely dissociates in water. Calculate the pH of a solution containing 1.02 g of HNO3 in 250. mL of solution.
1.19
Day 1 5-3
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Day 2 5-6
How many moles of nitric acid are needed to neutralize 0.50 moles of calcium hydroxide?
2HNO3 + Ca(OH)2 Ca(NO3)2 + 2H2O
1 mole
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Day 3 5-7
1. Carbonic acid is a weak acid, if it reacts with a strong base like NaOH, what type of solution will result?
2. Write an equation for the ionization of sodium bicarbonate.
3. Write an equation for the reaction between bicarbonate ions and water
NaHCO3 Na+(aq) + HCO3
-(aq)
HCO3-(aq) + H2O(l) H2CO3(aq) + OH-
(aq)
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Day 6 4-26
Arrhenius acidHydrolysisKw
-log[H+] Lewis baseUniversal IndicatorTitration
Bronsted-Lowry acid
Ka
Strong baseConcentrated acidNeutralization reactionStandard solution
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page 675 #s 39-43
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A 50 mL solution of H2SO4 is neutralized by 20 mL of 2.0 M NaOH. What is the concentration of the H2SO4 solution? The equation for the reaction is:
H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)
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