19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.What can you say about the K a value of a strong.

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19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.What can you say about the K a value of a strong acid? 2.In a M solution of a monoprotic acid [H + ] = 2.5 * M. Calculate the K a of this acid? Day * The pH for a 0.20 M solution of a monoprotic acid is 2.5, what is the K a ? 5.08 * 10 -5

19.1 Acid-Base Theories> 2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. m/esm_brown_chemist ry_9/2/660/ cw/i ndex.html Homework # 1 Chapter 16 – show me successful screen (100%) OR to me – due Tues. 4-24

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

19.1 Acid-Base Theories> 4 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 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 flask 2. an indicator is added 3. measured volumes of a base of known concentration are mixed into the acid until the indicator just barely changes color

19.1 Acid-Base Theories> 5 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 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

19.1 Acid-Base Theories> 6 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Titration  Determining the concentration by titration mathematically: Example: A 25 mL solution of H 2 SO 4 is neutralized by 18 mL of 1.0 M NaOH. What is the concentration of the H 2 SO 4 solution? The equation for the reaction is: H 2 SO 4(aq) + 2NaOH (aq)  Na 2 SO 4(aq) + 2H 2 O (l) Conversion plan: you need mols H 2 SO 4 to calculate molarity L NaOH  mols NaOH  mols H 2 SO 4

19.1 Acid-Base Theories> 7 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 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

19.1 Acid-Base Theories> 8 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 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

19.1 Acid-Base Theories> 9 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. V. Salts in Solution Example: ammonium chloride  Ammonium chloride completely ionizes in water: NH 4 Cl (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) + H 2 O (l)  NH 3(aq) + H 3 O + (aq)  the resulting H 3 O + ions make the solution somewhat acidic

19.1 Acid-Base Theories> 10 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 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)

19.1 Acid-Base Theories> 11 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. page 669 #s 27-34

19.1 Acid-Base Theories> 12 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.0 * Arrhenius base Amphoteric K b Conjugate acid Diprotic acid Lewis acid Self-ionization Strong acid K a Weak base Bronsted-Lowry base

19.1 Acid-Base Theories> 13 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.HNO 3 is a strong acid – assume it completely dissociates in water. Calculate the pH of a solution containing 1.02 g of HNO 3 in 250. mL of solution Day 1 5-3

19.1 Acid-Base Theories> 14 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day How many moles of nitric acid are needed to neutralize 0.50 moles of calcium hydroxide? 2HNO 3 + Ca(OH) 2  Ca(NO 3 ) 2 + 2H 2 O 1 mole

19.1 Acid-Base Theories> 15 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 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 NaHCO 3  Na + (aq) + HCO 3 - (aq) HCO 3 - (aq) + H 2 O (l)  H 2 CO 3(aq) + OH - (aq)

19.1 Acid-Base Theories> 16 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day Arrhenius acid Hydrolysis K w -log[H + ] Lewis base Universal Indicator Titration Bronsted-Lowry acid K a Strong base Concentrated acid Neutralization reaction Standard solution

19.1 Acid-Base Theories> 17 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. page 675 #s 39-43

19.1 Acid-Base Theories> 18 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. A 50 mL solution of H 2 SO 4 is neutralized by 20 mL of 2.0 M NaOH. What is the concentration of the H 2 SO 4 solution? The equation for the reaction is: H 2 SO 4(aq) + 2NaOH (aq)  Na 2 SO 4(aq) + 2H 2 O (l)