The Chemistry of Acids and Bases

Acid and Bases

Some Properties of Acids þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) þ Taste sour þ Corrode metals þ Electrolytes (conduct electricity) þ React with bases to form a salt and water þ pH is less than 7 þ Turns blue litmus paper to red “Blue to Red A-CID”

Some Common Acids Hydrochloric Acid Formula Name Common Use HCl aka Muriatic acid, Stomach acid Nitric Acid HNO 3 Strong Oxidizer Acetic Acid HC 2 H 3 O 2 Vinegar Sulfuric Acid H 2 SO 4 refinement of petroleum, fertilizers Citric Acid H3C6H5O7H3C6H5O7 Fruits and Candy Carbonic Acid H 2 CO 3 Pop and seawater

Some Properties of Bases  Produce OH - ions in water  Taste bitter, chalky  Electrolytes (conduct electricity)  Feel slippery  React with acids to form salts and water  pH greater than 7  Turns red litmus paper to blue “Basic Blue”

Some Common Bases NaOH KOH Ba(OH) 2 Mg(OH) 2 Al(OH) 3 sodium hydroxidelye potassium hydroxideliquid soap barium hydroxidestabilizer for plastics magnesium hydroxide“MOM” Milk of magnesia aluminum hydroxideMaalox (antacid) Formula Name Common Name

SOME DEFINITIONS Amphoteric - A substance that can act as either an acid or a base, e.g., H 2 O, HCO 3 -Amphoteric - A substance that can act as either an acid or a base, e.g., H 2 O, HCO 3 - Polyprotic acid or base - An acid or base that can donate or accept, respectively, more than one proton, e.g., H 3 PO 4, H 2 CO 3, H 4 EDTAPolyprotic acid or base - An acid or base that can donate or accept, respectively, more than one proton, e.g., H 3 PO 4, H 2 CO 3, H 4 EDTA

Acid/Base Definitions  Arrhenius Model  Acids produce hydrogen ions in aqueous solutions  Bases produce hydroxide ions in aqueous solutions  Bronsted-Lowry Model  Acids are proton donors  Bases are proton acceptors

Acid A Brønsted-Lowry Acid is a proton donor Base A Brønsted-Lowry Base is a proton acceptor AcidBase Conjugate Acid The Brønsted definition means NH 3 is a Base in water — and water is itself an Acid Conjugate Base ACID-BASE THEORIES

Conjugate Pairs Conjugate Acid – the remaining ion or molecule that can re-accept the proton and act as a base Conjugate Base – the species that is formed when a Brønsted-Lowry base gains a proton.

Acids & Base Definitions Summary

Do Problem:37

Self-Ionization of Water H 2 O + H 2 O  H 3 O + + OH - At 25 , [H 3 O + ] = [OH - ] = 1 x M K w is a constant at 25  C: K w = [H 3 O + ][OH - ] K w = (1 x )(1 x ) = 1 x = [K a ][K b ]

Calculating pH, pOH pH = -log 10 (H 3 O + ) pOH = -log 10 (OH - ) Relationship between pH and pOH pH + pOH = 14 Finding [H 3 O + ], [OH - ] from pH, pOH [H 3 O + ] = 10 -pH [OH - ] = 10 -pOH

pH and pOH Calculations

Do Problem: 51

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Self-Ionization of Water H 2 O + H 2 O  H 3 O + + OH - At 25 , [H 3 O + ] = [OH - ] = 1 x M K w is a constant at 25  C: K w = [H 3 O + ][OH - ] K w = (1 x )(1 x ) = 1 x = [K a ][K b ]

pH and pOH Calculations

Dissociation of Strong Acids Strong acids are assumed to dissociate completely in solution. Large K a or small K a ? Reactant favored or product favored?

Dissociation Constants: Strong Acids AcidFormula Conjugate Base KaKa Perchloric HClO 4 ClO 4 - Very large Hydriodic HI I - Very large Hydrobromic HBr Br - Very large Hydrochloric HCl Cl - Very large Nitric HNO 3 NO 3 - Very large Sulfuric H 2 SO 4 HSO 4 - Very large

Do Problem: 59

Dissociation of Weak Acids Weak acids are assumed to dissociate only slightly (less than 5%) in solution. Large K a or small K a ? Reactant favored or product favored?

Acid Dissociation HA (aq) + H 2 O (l) +  H 3 O + (aq) + A - (aq) Acid base Conjugate Conjugate acid base Alternately, H + may be written in its hydrated form, H 3 O + (hydronium ion)

Acid Dissociation HA (aq) +  H + (aq) + A - (aq) Acid Proton Conjugate base Alternately, H + may be written in its hydrated form, H 3 O + (hydronium ion)

Dissociation Constants: Weak Acids AcidFormula Conjugate Base KaKa Iodic HIO 3 IO x Oxalic H 2 C 2 O 4 HC 2 O x Sulfurous H 2 SO 3 HSO x Phosphoric H 3 PO 4 H 2 PO x Citric H 3 C 6 H 5 O 7 H 2 C 6 H 5 O x Nitrous HNO 2 NO x Hydrofluoric HF F x Formic HCOOH HCOO x Benzoic C 6 H 5 COOH C 6 H 5 COO x Acetic CH 3 COOH CH 3 COO x Carbonic H 2 CO 3 HCO x Hypochlorous HClO ClO x Hydrocyanic HCN CN x

A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC 2 H 3 O 2, K a = 1.8 x ? Step #1: Write the dissociation equation HC 2 H 3 O 2 (aq) + H 2 O (l)  C 2 H 3 O 2 - (aq) + H 3 O + (aq)

A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC 2 H 3 O 2, K a = 1.8 x ? Step #2: ICE it! HC 2 H 3 O 2  C 2 H 3 O H + I C E ~0 - x +x x xx

A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC 2 H 3 O 2, K a = 1.8 x ? Step #3: Set up the law of mass action HC 2 H 3 O 2  C 2 H 3 O H xxx E

A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC 2 H 3 O 2, K a = 1.8 x ? Step #4: Solve for x, which is also [H + ] HC 2 H 3 O 2  C 2 H 3 O H xxx E [H + ] = 3.0 x M

A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC 2 H 3 O 2, K a = 1.8 x ? Step #5: Convert [H + ] to pH HC 2 H 3 O 2  C 2 H 3 O H xxx E pH = - log (3.0 x ) = 2.52

Do Problem:63a

Do Problem: 63b

Staying Alive with Problem 75

Quiz 1)Name the 6 strong acids. 2)What is the [H+] in pure H2O? 3) What is the value of Kw? 4) What is the % dissociation and pH of a 0.75 M solution of formic acid, HCHO 2, K a = 1.8 x ? (1pt) % dissociation = 1.5% (1pt) pH = )HCl hydrochloric 2) HBr hydrobromic 3) HI hydroiodic 4) HClO 4 perchloric 5) HNO 3 nitric 6) H 2 SO 4 Sulfuric (1pt) ICE table (1pt) HCHO 2  CHO H + (1pt) X=0.012 (1pt) [H+] = 1.0 x M (1pt) Kw = 1.0 x

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Dissociation of Strong Bases  Strong bases are metallic hydroxides  Group I hydroxides (most common in lab NaOH, KOH) are very soluble  Group II hydroxides (Ca, Ba, Sr) are less soluble  pH of strong bases is calculated directly from the concentration of the base in solution MOH(s)  M + (aq) + OH - (aq)

Reaction of Weak Bases with Water The base reacts with water, producing its conjugate acid and hydroxide ion: CH 3 NH 2 + H 2 O  CH 3 NH OH - K b = 4.38 x 10 -4

K b for Some Common Weak Bases BaseFormula Conjugate Acid KbKb Ammonia NH 3 NH x Methylamine CH 3 NH 2 CH 3 NH x Ethylamine C 2 H 5 NH 2 C 2 H 5 NH x Diethylamine (C 2 H 5 ) 2 NH (C 2 H 5 ) 2 NH x Triethylamine (C 2 H 5 ) 3 N (C 2 H 5 ) 3 NH x Hydroxylamine HONH 2 HONH x HydrazineH 2 NNH 2 H 2 NNH x Aniline C 6 H 5 NH 2 C 6 H 5 NH x Pyridine C 5 H 5 N C 5 H 5 NH x Many students struggle with identifying weak bases and their conjugate acids.What patterns do you see that may help you?

Reaction of Weak Bases with Water The generic reaction for a base reacting with water, producing its conjugate acid and hydroxide ion: B + H 2 O  BH + + OH -

A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH 3, K b = 1.8 x ? Step #1: Write the equation for the reaction NH 3 (aq) + H 2 O (l)  NH 4 + (aq) + OH - (aq)

A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH 3, K b = 1.8 x ? Step #2: ICE it! I C E x +x x xx NH 3 + H 2 O  NH OH -

A Weak Base Equilibrium Problem Step #3: Set up the law of mass action xxx E What is the pH of a 0.50 M solution of ammonia, NH 3, K b = 1.8 x ? NH 3 + H 2 O  NH OH -

A Weak Base Equilibrium Problem Step #4: Solve for x, which is also [OH - ] xxx E [OH - ] = 3.0 x M NH 3 + H 2 O  NH OH - What is the pH of a 0.50 M solution of ammonia, NH 3, K b = 1.8 x ?

A Weak Base Equilibrium Problem Step #5: Convert [OH - ] to pH xxx E What is the pH of a 0.50 M solution of ammonia, NH 3, K b = 1.8 x ? NH 3 + H 2 O  NH OH - pOH = - log (3.0 x ) = 2.52 pH = 14 - pOH = 11.48

Do Problem: 84

Do Problem:96

Do Problem: 104

Acid-Base Properties of Salts Dissociate the following salts: K + (aq) + Cl - (aq) NH 4 + (aq) + ClO 4 - (aq) Mg 2+ (aq) + 2 NO 3 - (aq) Na + (aq) + C 2 H 3 O 2 - (aq) K + (aq) + NO 2 - (aq) CH 3 NH 3 + (aq) + Cl - (aq) K + (aq) + HCO 3 - (aq) Na + (aq) + HSO 4 - (aq) KCl(s)  NH 4 ClO 4 (s)  Mg(NO 3 ) 2 (s)  NaC 2 H 3 O 2 (s)  KNO 2 (s)  CH 3 NH 3 Cl(s)  KHCO 3 (s)  NaHSO 4 (s)  NH 4 ClO 2 (s)  NH 4 + (aq) + ClO 2 - (aq)

Acid-Base Properties of Salts Type of SaltExamplesCommentpH of solution Cation is from a strong base, anion from a strong acid KCl, KNO 3 NaCl NaNO 3 Both ions are neutral Neutral These salts simply dissociate in water: KCl(s)  K + (aq) + Cl - (aq)

Acid-Base Properties of Salts Type of SaltExamplesCommentpH of solution Cation is from a strong base, anion from a weak acid NaC 2 H 3 O 2 KCN, NaF Cation is neutral, Anion is basic Basic C 2 H 3 O H 2 O  HC 2 H 3 O 2 + OH- base acid acid base The basic anion can accept a proton from water:

Acid-Base Properties of Salts Type of SaltExamplesCommentpH of solution Cation is the conjugate acid of a weak base, anion is from a strong acid NH 4 Cl, NH 4 NO 3 Cation is acidic, Anion is neutral Acidic NH 4 + (aq)  NH 3 (aq) + H + (aq) Acid Conjugate Proton base The acidic cation can act as a proton donor:

Acid-Base Properties of Salts Type of SaltExamplesCommentpH of solution Cation is the conjugate acid of a weak base, anion is conjugate base of a weak acid NH 4 C 2 H 3 O 2 NH 4 CN Cation is acidic, Anion is basic See below  IF K a for the acidic ion is greater than K b for the basic ion, the solution is acidic  IF K b for the basic ion is greater than K a for the acidic ion, the solution is basic  IF K b for the basic ion is equal to K a for the acidic ion, the solution is neutral

Do Problem : 120

Strength of oxyacids The more oxygen hooked to the central atom, the more acidic the hydrogen. HClO 4 > HClO 3 > HClO 2 > HClO Remember that the H is attached to an oxygen atom. The oxygens are electronegative Pull electrons away from hydrogen

Strength of oxyacids Electron Density ClOH

Strength of oxyacids Electron Density ClOHO

Strength of oxyacids ClOH O O Electron Density

Strength of oxyacids ClOH O O O Electron Density

Acid-Base Properties of Salts Type of SaltExamplesCommentpH of solution Cation is a highly charged metal ion; Anion is from strong acid Al(NO 3 ) 2 FeCl 3 Hydrated cation acts as an acid; Anion is neutral Acidic Step #1: AlCl 3 (s) + 6H 2 O  Al(H 2 O) 6 3+ (aq) + Cl - (aq) Salt water Complex ion anion Step #2: Al(H 2 O) 6 3+ (aq)  Al(OH)(H 2 O) 5 2+ (aq) + H + (aq) Acid Conjugate base Proton

Effect of Structure on Acid-Base Properties

Hydrated metals Highly charged metal ions pull the electrons of surrounding water molecules toward them. Make it easier for H + to come off. Al +3 O H H

Acid-Base Properties of Oxides Non-metal oxides dissolved in water can make acids. SO 3 (g) + H 2 O(l) H 2 SO 4 (aq) Ionic oxides dissolve in water to produce bases. CaO(s) + H 2 O(l) Ca(OH) 2 (aq)

What is the concentration of H 3 O + in pure water? x 10 –7 M M x x 10 7 M x

[H + ] = 8.26 x 10 –5 M, what is the pH of the solution?

Which of the following is a conjugate acid/base pair? 1.HCl/OCl - 2.H 2 SO 4 /SO NH 4 + /NH 3 4.H 3 O + /OH - 5.none of these

Which of the following indicates the most basic solution? 1.[H + ] = 1 × 10 –10 M 2.pOH =6.7 3.[OH – ] = 7 × 10 –5 M 4.pH = At least two of the solutions are equally basic.

Dissolving Na 2 SO 4 in water will create a ______ solution. 1.Acidic 2.Basic 3.Neutral 4.Cannot be determined.

Calculate the pH of a 0.17 M solution of HOCl, K a =