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Types of Chemical Reactions Chapter 4 Goals: To be able to predict chemical reactivity. To know how to synthesize specific compounds.

Types of Reactions Acid-Base Oxidation-Reduction Precipitation Gas Forming Organic:  Substitution  Addition  Elimination

Reactions in Aqueous Solution Aqueous- solvent is water Reactions we’ll discuss today/next week are in aqueous solution, unless otherwise noted  Acid-Base  Redox  Precipitation

Electrolytes Strong: All of the solute comes apart to yield ions in solution  Dissolution of KMnO 4 Dissolution of KMnO 4 Weak: Some of the solute comes apart to yield ions Nonelectrolytes: No ions formed  Let’s compare Let’s compare

Electrolytes in the Human Body Most important: Na +, Cl -, K +, Ca 2+, Mg 2+,HCO 3 -, and PO 4 3-, SO 4 2- Elevated K +  cardiac arrythmia Decreased extracellular K +  paralysis Excess extracellular Na +  fluid retention Decreased plasma Ca 2+ and Mg 2+  muscle spasms

Acids and Bases Theories- there’s lots of them Ones we’ll use in this course  Lewis (later)  Brønsted-Lowry (now)  An acid is a substance that donates a proton (H + ) to a base  The hydronium ion

Brønsted-Lowry Definitions Acid= donates a proton (H + ) to a base Base= accepts a proton (H + ) from an acid Acid base reactions are reversible (almost always)

Brønsted-Lowry Definitions Acid= donates a proton (H + ) to a base Base= accepts a proton (H + ) from an acid Acid base reactions are reversible (almost always)

Important Acids and Bases

Strong Acids 100% of acid molecules produce ions in water  Dissociation vs. ionization

Weak Acids Only a few acid molecules produce ions (≤5%) Strong vs. Weak acid ionization

Polyprotic Acids Polyprotic acids can donate more than one H +  Sulfuric acid  Citric acid (C 6 H 8 O 7 ) : Not all H’s are acidic H 2 SO 4  H + + HSO 4 - HSO 4 -  H + + SO 4 2-

Bases Strong bases are hydroxide salts For now, the only important weak base is NH 3.

If H 3 PO 4 reacts as an acid, which of the following can it not make? 1. H 4 PO H 2 PO HPO PO 4 3-

If C 2 O 4 2- (oxalate ion) reacts in an acid-base reaction, which of the following can it not make? 1. H 2 C 2 O 4 2. HC 2 O CO 2 20

Acid Base Reactions

Strong Acid + Strong Base HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) acid base “salt” water What do we get if we mix: HBr + LiOH 

Acid Base Reactions Diprotic acids or bases H 2 SO 4 (aq) + NaOH(aq)  H 2 SO 4 (aq) + Ba(OH) 2 (aq)  HCl(aq) + Ba(OH) 2 (aq) 

Acid-Base Reactions Diprotic Acids or Bases H 2 SO 4 (aq) + NaOH(aq)  H 2 SO 4 (aq) + Ba(OH) 2 (aq)  HCl(aq) + Ba(OH) 2 (aq) 

Acid-Base Reactions Strong Acid + Weak Base HCl(aq) + NH 3 (aq)  NH 4 Cl(aq)

Acid-Base Reactions Weak Acid + Strong Base HCN(aq) + NaOH(aq)  NaCN(aq) + H 2 O(l) acid base “salt” water

Net Ionic Equations HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) What really happens: H + (aq) + OH - (aq)  H 2 O(l) Sodium ion and chloride ion are “spectator ions”

Reactions involving weak bases HCl(aq) + NH 3 (aq)  NH 4 + (aq) + Cl - (aq) Net-Ionic Equation: NH 3 (aq) + H + (aq)  NH 4 + (aq)

CH 3 CO 2 H(aq) + NaOH(aq)  1. CH 3 CO 2 H 2 + (aq) + NaO(aq) 2. CH 3 CO 2 - (aq) + H 2 O(l) + Na + (aq) 3. CH 4 (g) + CO 2 (g) + H 2 O(l)

HCN(aq) + NH 3 (aq)  1. NH 4 + (aq) + CN - (aq) 2. H 2 CN + (aq) + NH 2 - (aq) 3. C 2 N 2 (s) + 3 H 2 (g)

Solution Concentration: Molarity Molarity = moles solute per liter of solution 0.30 mol NH 3 dissolved in L Concentration = Written like: [NH 3 ] = 0.60 M

pH Scale In pure water, a few molecules ionize to form H 3 O + and OH – H 2 O + H 2 O  OH – + H 3 O + In acidic and basic solutions, these concentrations are not equal acidic: [H 3 O + ] > [OH – ] basic: [OH – ] > [H 3 O + ] neutral: [H 3 O + ] = [OH – ]

pH Scale Measure how much H 3 O + is in a solution using pH pH < 7.0 = acidic pH > 7.0 = basic pH = 7.0 = neutral Measure of H 3 O + and OH – concentration (moles per liter) in a solution As acidity increases, pH decreases

pH Scale The pH scale is logarithmic: log(10 2 ) = log(10 1 ) = log(10 0 ) = –1 log(10 –1 ) = – –2 log(10 –2 ) = –2 The pH scale is logarithmic: log(10 2 ) = log(10 1 ) = log(10 0 ) = –1 log(10 –1 ) = – –2 log(10 –2 ) = –2 pH= –log [H 3 O + ] pH= –log [H 3 O + ] pH if [H 3 O + ] = 10 –5 ? 10 –9 ? Acidic or basic? pH if [H 3 O + ] = 10 –5 ? 10 –9 ? Acidic or basic? pH if [H 3 O + ] = M? pH if [H 3 O + ] = M?

[H 3 O + ] from pH Finding [H 3 O + ] from pH [H 3 O + ] = 10 -pH What is [H 3 O + ] if pH = 8.9?

pH: Quantitative Measure of Acidity Acidity is related to concentration of H + (or H 3 O + ) pH = -log[H 3 O + ]