Chapter 9: Acids & Bases

Acids Acid: a substance that, when dissolved in water, increases the H+ (or H3O+) concentration of the solution by giving up (or donating) a H+ HCl(aq) + H2O(l) H3O+(aq)+ Cl-(aq) HCl (aq) H+ (aq) + Cl- (aq) Can be strong or weak Monoprotic or polyprotic (protic ~ proton~H+) Arrow pushing mechanism

Chapter 15, Unnumbered Figure, Page 660

Hydrogens connected to more electronegative atoms are more likely to act as an acidic hydrogen High EN atoms: F, Cl, Br, I, O Chapter 15, Unnumbered Figure 1, Page 661

Practice Decide if the following molecules are acids or not, based on their structures.

Strong acid: an acid that completely ionizes/dissociates in water HNO3(aq) + H2O(l) H3O+(aq) + NO3-(aq)

Weak Acid: an acid that only partially ionizes/dissociates in water HC2H3O2(aq)+ H2O(l) C2H3O2-(aq) +H3O+(aq) Weak Acids: Phosphoric acid H3PO4 Acetic Acid CH3COOH Carbonic Acid H2CO3 Hydrocyanic Acid HCN Benzoic Acid C6H5COOH

Chapter 15, Unnumbered Figure 2, Page 661

Chapter 15, Unnumbered Figure 4, Page 661

Practice Write the chemical equation for the dissociation of each acid in the following containers. Then determine whether there is strong or weak acid present. Chapter 15, Unnumbered Figure 1, Page 709

Bases Base: a substance that, when put in water, increases the concentration of OH- ions or a substance that accepts H+ ions NaOH(aq) + H2O(l) Na+(aq) + OH-(aq) +H2O NaOH(aq) Na+(aq) + OH-(aq) Strong Bases: bases that completely ionize in water Arrow pushing mechanism

Weak Bases: bases that only partially ionize in water Ammonia: NH3 Pyridine: C5H5N

Chapter 15, Unnumbered Figure, Page 662

Chapter 15, Unnumbered Figure, Page 686

Then determine whether there a strong or weak base present. Write the chemical equation for the dissociation of each base in the following containers. Then determine whether there a strong or weak base present. Chapter 15, Unnumbered Figure 2, Page 709

Polyprotic Acids Polyprotic acids: acids that can release more than one H+ HCl(aq) +H2O(l) Cl-(aq) + H3O+(aq) HCl = monoprotic acid Complete ionization of H2SO4 (sulfuric acid) H2SO4(aq) + H2O(l) HSO4-(aq) + H3O+(aq) HSO4-(aq) + H2O(l) SO42-(aq) + H3O+(aq) H2SO4 = polyprotic acid

Problem Write out the equation(s) for the complete ionization of phosphoric acid, H3PO4, in water.

Each acid has a conjugate base and every base has a conjugate acid Congugate Acid-Base Pairs Each acid has a conjugate base and every base has a conjugate acid conjugate acid-base pair 1 HA + B A− + BH+ conjugate acid-base pair 2

Problems Identify the conjugate bases for the following: HBr H2S H2CO3 Identify the conjugate acids for the following NO2- NH3 OH-

In the following equations, identify the conjugate acid and base pairs: HCl + H2O  H3O+ + Cl- C5H5N + H2O  C5H6N+ + OH-

Acid Ionization Constant Acid Ionization Constant (Ka): the equilibrium constant for the ionization reaction of an acid with water HA + H2O A- + H3O+ Large Ka = Strong acid Small Ka = Weak acid

Questions Write the equilibrium constant expression for the dissociation of HCN (hydrocyanic acid) in water Write the equilibrium expression for the dissociation of HF in water If the Ka for HCN is 4.9 x 10-10 and the Ka for HF is 7.2 x 10-4, which acid is stronger?

Predict whether the equilibrium for each of the following reactions favors the reactants or products. H3PO4(aq) + H2O(l) H3O+(aq) + H2PO4(aq) NH4+(aq) + H2O(l) H3O+(aq) + NH3(aq)

Base Ionization Constant Base Ionization Constant (Kb): the equilibrium constant for the ionization reaction of a base with water B + H2O OH- + BH+ Large Kb = Strong base Small Kb = Weak base

Autoionization of Water

Autoionization of Water Also called “Self Ionization” About 1 out of every 10 million water molecules form ions through self ionization H2O Û H+ + OH– H2O + H2O Û H3O+ + OH– All aqueous solutions contain both H3O+ and OH–

Ion Product Constant for Water Ion Product Constant for Water (Kw): the numerical value obtained by multiplying the molar concentrations for hydronium and hydroxide ions present in pure water at 25°C Kw = [H3O+][OH-] = 1.00 x 10-14 at 25 oC the concentration of H3O+ and OH– are equal in pure water [H3O+] = [OH–] = 10-7M @ 25°C

Ion Product of Water the product of the H3O+ and OH– concentrations is always the same number Kw =[H3O+][OH–] = 1.00 x 10-14 @ 25°C if you measure one of the concentrations, you can calculate the other as [H3O+] increases the [OH–] must decrease so the product stays constant inversely proportional

H+ OH- [H+] vs. [OH-] Acid Base Even though it may look like it, neither H+ nor OH- will ever be 0

Acidic and Basic Solutions Neutral solutions have equal [H3O+] and [OH–] [H3O+] = [OH–] = 1 x 10-7 acidic solutions have a larger [H3O+] than [OH–] [H3O+] > [OH–] [H3O+] > 1 x 10-7; [OH–] < 1 x 10-7 basic solutions have a larger [OH–] than [H3O+] [H3O+] < [OH–] [H3O+] < 1 x 10-7; [OH–] > 1 x 10-7

Questions Calculate the [OH] at 25°C when the [H3O+] = 1.5 x 10-9 M, and determine if the solution is acidic, basic, or neutral Calculate the [H3O+] at 25°C in a solution that has a [OH] 1.3 x 10-10 M and determine if the solution is acidic, basic, or neutral Calculate the [H3O+] at 25°C in a solution that has a [OH] 1.0 x 10-7 M and determine if the solution is acidic, basic, or neutral

pH and pOH Acidic solutions Basic solutions Neutral solutions

pH is a measure of the concentration of H+ or H3O+ in solution pH = -log [H+] OR pH = -log [H3O+] [H3O+] = 10-pH pOH is a measure of the concentration of OH- in solution pOH = -log [OH-] [OH-] = 10-pOH pH + pOH = 14

Problems What is the pH for an HCl solution with an [H3O+] = 2.3 x 10-2? What is the pH of an NaOH solution with an [H3O+] = 3.39 x 10-10? What is the pH of a KOH solution with a [OH-] = 1.1 x 10-2? What is the [H3O+] for a solution with a pH of 8.45. What is the [OH-]?

Classification of Water Soluble Substances Electrolytes: solutes that separate into ions when dissolved in water (they’re soluble) Have the ability to conduct electricity 2 types Strong electrolytes Weak electrolytes

Strong electrolytes: solutes that completely dissociates into ions when dissolved in water Examples: NaCl, MgBr2, HCl Strong electrical conductors Strong electrolyte(aq or s) → Cation+(aq) + Anion-(aq) Example: NaCl(s) → Na+(aq) + Cl-(aq)

Weak Electrolytes: solutes that, when dissolved in water, only partially dissociates into ions Examples: HF, NH3, acetic acid Weak electrical conductors Weak electrolyte(aq) ↔ Cation+(aq) + Anion-(aq) Example: HF(aq) ↔ H+(aq) + F-(aq)

Nonelectrolytes: solutes that dissolve in water without separating into ions Examples: sucrose, ethanol Do not conduct electricity Nonelectrolyte (s or l) → Nonelectrolyte(aq) Example: C12H22O11(s) → C12H22O11(aq)

Problems The following salts are strong electrolytes. Write a balanced equation for their dissociation in water LiBr FeCl3 HCN is a weak acid. Write a balanced equation for its dissociation in water Do you expect Fructose (C6H12O6) to be a strong electrolyte, weak electrolyte, or nonelectrolyte? Write a balanced equation for its solvation in water

Neutralization Reactions When strong acids and bases in aqueous solution react with each other, they form water and a salt HX(aq) + MOH(aq)  HOH(l) + MX(aq) HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq) Water Salt

Problems Write out the chemical equations for the following reactions HBr and KOH HCl and Mg(OH)2 H2SO3 and NaOH

Titration Titration: a procedure for the quantitative analysis of a substance of unknown concentration whereby a measured quantity of another substance, of known concentration, is completely reacted with the with the original substance. Often used to determine the concentration of acids and bases

Equivalence point: the point in a titration at which one reactant has been exactly consumed by the addition of another reactant Midpoint of vertical rise Occurs at pH = 7 in a strong acid-strong base titration [H3O+] = [OH-]

Indicators Acid-Base Indicator: a chemical that changes color with a change in pH Added to solutions in small amounts in order to determine to solution’s pH visually Usually organic compounds Weak acid or base establishes an equilibrium with the H2O and H3O+ in the solution 62

HInd(aq) + H2O(l)  Ind(aq) + H3O+(aq)

Phenolphthalein 64 64

Bromocresol Green Yellow Green Blue

Methyl Red 66

3 steps to solving a titration problem (unknown acid molarity) 1. How many moles of base were added to titrate the unknown acid? Use concentration and volume of base added M =mol/L 2. What is the molar ratio that the base reacts with the acid, this will give you moles of acid? Use the overall/net chemical equation, just like stoichiometry 3. With the moles of acid, what is the initial concentration of the acid? Use the initial volume of acid M = mol/L

Questions You have 25.0 mL of a HCl solution of unknown concentration. If you titrate your acid with 17.3 mL of a 0.877 M NaOH solution, what is the original concentration of your acid? NaOH +HCl  H2O + NaCl M = mol/L  M x L = mol MNaOH x LNaOH = molNaOH MNaOH = 0.877 MNaOH LNaOH = 0.0173 LNaOH LHCl = 0.0250 LHCl molNaOH x (1 molHCl / 1 molNaOH) = molHCl molHCl / LHCl = MHCl 0.877 MNaOH x 0.0173 LNaOH = 0.01517 molNaOH 0.01517 molNaOH x (1 molHCl / 1 molNaOH) = 0.01571 molHCl 0.01571 molHCl / 0.0250 LHCl = 0.607 MHCl

2). You also have 25. 0 mL of a sulfuric acid solution 2) You also have 25.0 mL of a sulfuric acid solution. If you titrate this solution with 32.1 mL of a 1.50 M KOH solution, what is the concentration of your acid?

Chapter 9 review Acid, strong acid, weak acid, Base, strong base, weak base Polyprotic acids Acid-conjugate base, Base-conjugate acid Neutralization reaction Acid ionization constant, Base ionization constant Auto ionization of water Strong and weak electrolytes pH and pOH Titration, acid-base indicators, equivalence point,

Definitions 8 and 9 Chapter 8 Solution, solvent, solute Solubility, Henry’s Law Unsaturated, saturated, and super saturated solutions Concentration, Molarity Osmosis, osmotic pressure, turgor, Hypotonic, hypertonic, and isotonic solutions Mixture, colloids, suspension Chapter 9 Acid, strong acid, weak acid, Base, strong base, weak base Polyprotic acids Acid-conjugate base, Base-conjugate acid Neutralization reaction Acid ionization constant, Base ionization constant Auto ionization of water Strong and weak electrolyte pH and pOH Titration, acid-base indicators, equivalence point,