4. Aqueous Solutions. Solution homogeneous mixture of two components

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1 4. Aqueous Solutions Solution homogeneous mixture of two components Many chemical reactions occur in solution Solutions in water called aqueous

2 Definitions Solute component(s) in smaller amount 2 types: electrolytes & nonelectrolytes Solvent component in greatest amount disperses reactants so they can react Precipitate excess solute that falls out of solution as a solid

3 Electrolytes Definitions dissociate in solution to form ions conduct electricity may be strong or weak strong: HCl H 2 SO 4 NaOH {ionic} weak: CH 3 COOH NH 3 HF tap water

4 Hydration NaCl (s) Na + (aq) + Cl - (aq) Ions surrounded by H 2 O & dissolve

5 Polar & Nonpolar substances Why do salt and water mix? Both are polar substances NaCl (s) Na + (aq) + Cl - (aq) Oil and water DON T mix? Oil is non-polar

6 Precipitation Reactions

7 Precipitation Reactions

8 Precipitation Reactions

9 Solubility Rules 1. Compounds of Gp 1 metals and NH 4 soluble 2. Compounds of NO - - 3, acetate, ClO 4 soluble 3. Compounds of hydroxide insoluble Exceptions: Gp 1 metals, Ba 2+ Sr 2+ Ca 2+ (slightly) +

10 Solubility Rules 4. Most compounds of Cl - Br - I - soluble Exceptions: Ag + Pb Hg 2 5. Compounds of carbonate, phosphate, sulfide + insoluble Exceptions: group 1, NH 4 6. Most compounds of sulfate soluble Exceptions: Ba 2+ Pb 2+ (Ca 2+ Ag + slightly)

11 AgNO AgNO 3 (aq) AgNO AgNO 3 (aq) Will precipitate form? (aq) + NaCl (aq) + NaCl molecular equation NaCl (aq) NaCl (aq) NaNO 3 (aq) NaNO (aq) + AgCl (s) all nitrates soluble insoluble Ag + (aq) (aq) + Cl Cl - (aq) AgCl AgCl (s) ionic equation

12 PbCl PbCl 2 (aq) Will precipitate form? (aq) + K 2 SO 4 (aq) 2 KCl (aq) KCl (aq) (aq) + PbSO 4 (s) soluble insoluble

13 PbCl 2 (aq) Will precipitate form? (aq) + K 2 SO 4 (aq) 2 KCl (aq) KCl (aq) (aq) + PbSO 4 (s)

14 Acids and Bases Acids: vinegar, lemons, gastric juice Bases: ammonia, baking soda, drano Salts: table salt

15 Properties Acids and Bases Acids: 1. sour 2. change color of dyes 3. dissolve metals to form hydrogen 4. react with carbonates to form CO 2 5. neutralize bases water soluble acids form hydrogen ions

16 Properties Acids and Bases Bases: 1. bitter 2. change color of dyes 3. soapy feel 4. neutralize acids In water, soluble bases can form OH - or CO 2-3 or O 2- ions These ions react with H + ions NH 3 another common base

17 Acid-Base Theory Davy (1811) all acids contain hydrogen

18 Acid-Base Theory Arrhenius (1884) acid: form H + in water base: form OH - in water

19 Acid-Base Theory Bronsted Lowry (1923) Acid: lose or donate H + Base: gain or accept H +

20 Acids and Bases Acid Definition: substance that produces hydrogen ions in water called a Lowry-Bronsted acid HCl H 2 SO 4 HNO 3 H 3 PO 4 CH 3 COOH

21 Dissociation Acids and bases dissociate or ionize in water HCl (aq) 6 H + (aq) + Cl - (aq) KOH (aq) 6 K + (aq) + OH - (aq)

22 The Hydronium Ion H 3 O + self ionization of water

23 Some Reactions In general: acid + base 6 salt + H O 2 HCl + NaOH 6 NaCl + H O 2 2 HCl + Na CO 6 NaCl + CO + H O Both are neutralization reactions

24 Salts Product of acid + base reaction HCl + NaOH 6 NaCl + H O 2 when an acid reacts with a base a salt and water form carbonates 6CO gas 2

25 Polyprotic Acids HCl: monoprotic acid H 2 SO 4 : diprotic acid H 3 PO 4 : triprotic acid H SO (aq) º H + (aq) + HSO - (aq) HSO - 4 (aq) º H + (aq) + SO 2- (aq) 4

26 Common Acids HCl cleans metals, brick, cement H 2 SO 4 car batteries, fertilizers, industrial chemicals, nitroglycerin HNO 3 fertilizers, dyes, plastics, explosives All are corrosive

27 Common Bases NaOH Ca(OH) 2 NH 3 drain cleaner, soap manufacture lime, mortar, plaster, cement cleaner Mg(OH) milk of magnesia 2 Many drugs: cocaine, morphine, nicotine

28 Oxidation & reduction Reactions Electron transfer reactions 2 Mg (s) + O (g) 2 MgO (s) 2 really two reactions oxidation: loss of electrons reduction: gain of electrons Break into 2 half reactions

29 Oxidation & reduction Reactions Oxidation Loss of electrons Mg oxidized Half-reaction: Mg Mg Mg e - Reduction Gain of electrons O reduced 2 Half-reaction: O + 4 e 2 e- 2 O 2- Overall: 2 Mg + O 2 Mg 2+ O 2-2

30 Oxidation & reduction Reactions Overall: 2 Mg + O 2 Mg 2+ O 2-2 reducing agent oxidizing agent

31 Oxidation & reduction Reactions magnesium oxidized Overall: 2 Mg + O 2 Mg 2+ O 2-2 oxygen reduced oxidation numbers

32 Oxidation Numbers Keeps track of electrons Uses naming compounds classifying reactions writing formulas

33 Oxidation Numbers Summary of rules 1. free elements = 0 2. monatomic ions = ionic charge 3. F = -1 O = H = +1 (with nonmetals) H = -1 (with metals)

34 Oxidation Numbers Summary of rules 5. some elements >1 oxidation number N,S,P,Cl; transition metals 6. Neutral compounds: sum of oxidation numbers = 0 Be able to assign oxidation numbers to elements in a compound. Use above rules.

35 Oxidation Numbers Examples: NaF H PO 3 4 NaF: F always -1 Na must be +1 H PO : O = -2; H = {3 x (+1)} + P + {4 x (-2)} = 0 P = +5

36 Oxidation & reduction Reactions magnesium oxidized Overall: 2 Mg + O 2 Mg 2+ O 2-2 oxygen reduced

37 Oxidation & reduction Reactions oxidation Overall: 2 Mg + O 2 Mg 2+ O 2-2 reduction oxidation: increase in oxidation number reduction: decrease in oxidation number

38 Activity Series If element A is more reactive then element B, it can displace element B from a compound Mg + 2 HCl ± MgCl + H 2 2 magnesium displaces hydrogen

39 Activity Series Fig 4.14 describes order of displacement reactions Mg + 2 HCl ± MgCl + H 2 2 magnesium higher than hydrogen

40 order of reactivity most reactive at top

41 order of reactivity most reactive at top

42 order of reactivity most reactive at top

43 see fig 4.14

44 Concentration Measure amount of solute in a solution weight / volume % volume / volume % weight / weight % molarity

45 Concentration Saline: 0.9 wt/vol % Alcohol in wine: 6 vol/vol % Fat in ham: 3 wt/wt % (or 97% fat free) Molarity: no consumer use used by chemists

46 Concentration molarity = moles solute volume of solution volume in liters symbol: M units: mol/l A 1 M = a one molar solution [ ] means molar eg [NaCl] = 2.0 M

47 Molarity Calculations Calculate the molarity of a 2.0 L solution containing 10.0 moles of NaOH molarity = moles solute volume of solution M = 10.0 mol NaOH = 5.0 M 2.0 L

48 Molarity Calculations Calculate the molarity of 2.0 L of a solution containing g of HCl Need moles HCl Use formula weight F.Wt. (HCl) moles (HCl) (HCl) = = (HCl) = mass = g = 0.50 mol F.Wt molarity (HCl) = 0.50 mol = 0.25 M 2.0 L

49 Molarity Calculations molarity = moles solute volume of solution M = mol V mol = MV

50 Molarity Calculations molarity = moles solute volume of solution M = mol V

51 Making Solutions Solutions are prepared in two ways: Weighing proper amount of solute and diluting to volume Note: water mixed with concentrated solution makes a diluted (less concentrated) solution

52 Making Solutions How would you prepare 100 ml of a M NaCl solution? First calculate moles of NaCl needed mol = MV = x L = moles NaCl Next, find mass of NaCl needed mass = mol x F. Wt. = x = grams NaCl

53 Making Solutions To make solution: Weigh out exactly g dry NaCl Transfer to a volumetric flask Fill about 1/3 with pure water Shake to dissolve Dilute to 100 ml mark

54 Dilutions solutions can be easily diluted by adding more solvent (water) M V = M V where 1 is initial solution 2 is diluted solution can use any volume or concentration unit as long as same units on both sides of equation

55 Dilutions What is concentration of a solution produced by diluting ml of a 1.5 M NaOH solution to L? M V = M V M = 1.5 M V = ml 1 1 M =?? V = 2000 ml 2 2 M = (M V )/ V = 1.5 M x ml ml = M

56 Titrations A reaction between two reactants where the amount of one reactant is unknown Often, one is an acid and one is a base: acid-base titration Both reactants need to be in solution Reactants must be carefully measured and mixed together

57 Titrations Solution of known concentration called titrant and placed in buret Solution of unknown concentration measured with a pipet and placed in a flask with an indicator Titrant added to flask until indicator changes color = equivalence point

58 Titrations

59 Titrations Indicators: dyes that change color at end of reaction phenolphthalein In acid: colorless In base: pink

60 Titrations Indicators: dyes that change color at end of reaction phenolphthalein

61 Titration Calculations

62 Titration Calculations Determine the volume of 0.1 M HCl that must be added to completely react with 250 ml of 2.5 M NaOH HCl + NaOH ± NaCl + H O 2 Step 1 calculate the moles of NaOH

63 Titration Calculations Step 1 calculate the moles of NaOH Have 250 ml of a 2.5 M NaOH solution mol = MxV = 0.25 L x 2.50 mol/l NaOH = mol

64 Titration Calculations Step 2 calculate mole of HCl HCl + NaOH ± NaCl + H O 2 1 mole HCl needs 1 mole NaOH Therefore need mol HCl

65 Titration Calculations Step 3 calculate volume of HCl V = mol/m = mol = 6.25 L mol/l

66 Titration Calculations Determine the molarity an HCl solution if 150 ml of the HCl neutralizes 50.0 ml of a M NaOH solution HCl + NaOH ± NaCl + H O 2 Step 1 calculate the moles of NaOH mol = MxV = L x mol/l NaOH = mol NaOH

67 Titration Calculations Step 2 calculate mole of HCl HCl + NaOH ± NaCl + H O 2 1 mole HCl needs 1 mole NaOH Therefore need mol HCl

68 Titration Calculations Step 3 calculate molarity of HCl M = mol/l = mol = mol/l L

69 Titration Calculations Caution what if mole ratio not 1:1? H SO + 2 NaOH ± Na SO + 2H O mole H SO needs 2 mole NaOH 2 4

70 Titration Calculations In general: aa + bb ± products When A and B both in solution: 1 x M V = 1 x M V A A B B a b

71 Titration Calculations When A is solid and B in solution: 1 x mass = 1 x M V A B B a F. wt. b A

72 End of Chapter 4

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