11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds

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1 Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most molecular compounds stay associated in water Brooks/Cole Brooks/Cole 2 Aqueous Solubility of Ionic Compounds Aqueous Solubility of Ionic Compounds 2008 Brooks/Cole Brooks/Cole 4 Aqueous Solubility of Ionic Compounds Exchange Reactions: Precipitation (a) Nitrates (soluble) (b) Hydroxides (insoluble) AgNO 3 Cu(NO 3 ) 2 Cu(OH) 2 AgOH (c) Sulfides CdS Sb 2 S 3 PbS (NH 4 ) 2 S soluble insoluble 2008 Brooks/Cole Brooks/Cole 6 1

2 Precipitation Reaction When ionic solutions mix, a precipitate may form: Not all ions react KNO 3 (aq) + NaCl(aq) No reaction A reaction occurs if a product is insoluble. Precipitation Reactions Na 2 SO 4 (aq) and Ba(NO 3 ) 2 (aq) are mixed. Will they react? Products? Na + SO 4 2 Ba 2+ NO 3 NaNO 3 and BaSO 4. Insoluble? The solubility rules help predict reactions Brooks/Cole Brooks/Cole 8 Soluble ionic compounds fully dissociate: AgNO 3 (aq) Ag + (aq) + NO 3 (aq) KCl(aq) K + (aq) + Cl (aq) On mixing: Ag + (aq) + NO 3 (aq) + K + (aq) + Cl (aq) AgCl(s) + K + (aq) + NO 3 (aq) Net ionic equation: Ag + (aq) + Cl (aq) AgCl(s) 2008 Brooks/Cole Brooks/Cole 10 (NH 4 ) 2 S(aq) + Hg(NO 3 ) 2 (aq) HgS + 2 NH 4 NO 3 Product Solubility HgS insoluble (All sulfides except group 1A, 2A and NH + 4 salts) NH 4 NO 3 soluble (All ammonium salts; all nitrates) (NH 4 ) 2 S(aq) + Hg(NO 3 ) 2 (aq) HgS + NH 4 NO 3 not balanced ammonium sulfide mercury(ii) nitrate mercury(ii) sulfide ammonium nitrate 2008 Brooks/Cole Brooks/Cole 12 2

3 Acids Increase the concentration of H + ions in water. 2 NH 4+ (aq) + S 2 (aq) + Hg 2+ (aq) + 2 NO 3 (aq) HgS(s) + 2 NH 4+ (aq) + 2 NO 3 (aq) S 2 (aq) + Hg 2+ (aq) HgS(s) Change the color of pigments (indicators) Litmus, phenolphthalein 2008 Brooks/Cole Brooks/Cole 14 Acids Bases Increase the concentration of OH (hydroxide ion) in water. Bases: Counteract an acid (neutralize an acid). Change an indicator s color (phenolphthalein ). Have a bitter taste. Feel slippery. H 2 O 2008 Brooks/Cole Brooks/Cole 16 Common Acids and Bases Neutralization Reactions acid + base salt + water. Neutralizations are exchange reactions Brooks/Cole Brooks/Cole 18 3

4 for AcidBase Reactions for AcidBase Reactions 2008 Brooks/Cole Brooks/Cole 20 GasForming Exchange Reactions GasForming Exchange Reactions Carbonic acid (unstable) Tums H 2 CO 3 (aq) H 2 O(l) + CO 2 (g) often written: CaCO 3 (s) + 2 HCl(aq) CaCl 2 (aq) + H 2 O(l) + CO 2 (g) AlkaSeltzer 2008 Brooks/Cole Brooks/Cole 22 GasForming Exchange Reactions GasForming Exchange Reactions Sulfurous acid (unstable) H 2 SO 3 (aq) H 2 O(l) + SO 2 (g) or Na 2 SO 3 (aq) + 2 HCl(aq) 2 NaCl(aq) + H 2 O(l) +SO 2 (g) 2008 Brooks/Cole Brooks/Cole 24 4

5 OxidationReduction Reactions OxidationReduction Reactions In all cases: If something is oxidized, something must be reduced. Redox reactions move e. (note: H 2 is oxidized, so CuO is an oxidizing agent) +2 e 2 Ag + (aq) + Cu(s) 2 Ag(s) + Cu 2+ (aq) 2 e Here: Cu changes to Cu 2+. Cu loses 2 e ; each Ag + gains one e Ag + is reduced (ore turned to metal) Gain of e = reduction (so, loss of e = oxidation) 2008 Brooks/Cole Brooks/Cole 26 Redox Reactions and Electron Transfer Redox Reactions and Electron Transfer e M X M loses electron(s) X gains electron(s) M is oxidized X is reduced M is a reducing agent X is an oxidizing agent 2008 Brooks/Cole Brooks/Cole 28 Common Oxidizing and Reducing Agents Oxidizing Agent Reaction Product O 2 (oxygen) O 2 (oxide ion) H 2 O 2 (hydrogen peroxide) H 2 O(l) F 2, Cl 2, Br 2, I 2 (halogen) F, Cl, Br, I (halide ion) HNO 3 (nitric acid) nitrogen oxides (NO, NO 2..) Cr 2 O 7 (dichromate ion) Cr 3+ (chromium(iii) ion) MnO 4 (permanganate ion) Mn 2+ (manganese(ii) ion) Reducing Agent Reaction Product H 2 (hydrogen) H + or H 2 O C CO and CO 2 M (metal: Na, K, Fe..) M n+ (Na +, K +, Fe 3+..) Displacement Reactions + + A XZ AZ X Redox: Fe(s) + CuSO 4 (aq) FeSO 4 (aq) + Cu(s) Cu(s) + 2 AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2 Ag(s) Brooks/Cole Brooks/Cole 30 5

6 Activity Series of Metals Displace H 2 from H 2 O (l), steam or acid Displace H 2 from steam or acid Displace H 2 from acid No reaction with H 2 O, steam or acid lithium potassium barium strontium calcium sodium magnesium aluminum manganese zinc chromium iron nickel tin lead hydrogen antimony copper mercury silver palladium platinum gold Ease of oxidation increases 2008 Brooks/Cole 31 Displacement Reactions Powerful reducing agents at the top. Higher elements displace lower ones: Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s) Mg(s) + 2 HCl(aq) MgCl 2 (aq) + H 2 (g) 2008 Brooks/Cole 32 Li K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Ni Sn Pb H Sb Cu Hg Ag Pd Pt Au Displacement Reactions Displacement Reactions Potassium + water 2 K(s) + 2 H 2 O(l) 2 KOH(aq) + H 2 (g) 2008 Brooks/Cole Brooks/Cole 34 Solution Concentration Relative amounts of solute and solvent. Molarity Molarity = moles solute liters of solution = mol L Shorthand: [NaOH] =1.00 M The brackets [ ] represent molarity of 2008 Brooks/Cole Brooks/Cole 36 6

7 Molarity Calculate the molarity of sodium sulfate in a solution that contains 36.0 g of Na 2 SO 4 in ml of solution. n Na2SO4 = [Na 2 SO 4 ] = 36.0 g = mol g/mol mol L Unit change! (ml to L) [Na 2 SO 4 ] = mol/l = M Molarity 6.37 g of Al(NO 3 ) 3 are dissolved to make a 250. ml aqueous solution. Calculate (a) [Al(NO 3 ) 3 ] (b) [Al 3+ ] and [NO 3 ]. (a) Al(NO 3 ) 3 FM = (14.00) + 9(16.00) = g mol 6.37 g g/mol 2008 Brooks/Cole Brooks/Cole 38 Molarity 6.37 g of Al(NO 3 ) 3 in a 250. ml aqueous solution. Calculate (a) the molarity of the Al(NO 3 ) 3, (b) the molar concentration of Al 3+ and NO 3 ions in solution. Solution Preparation Solutions are prepared either by: 1. Diluting a more concentrated solution. 1 Al(NO 3 ) 3 1 Al 3+ 1 Al(NO 3 ) 3 3 NO 3 [Al 3+ ] = M Al(NO 3 ) 1 Al 3+ 3 = M Al 3+ 1 Al(NO 3 ) 3 [NO 3 ] = M Al(NO 3 ) 3 = M NO 3 or 2. Dissolving a measured amount of solute and diluting to a fixed volume Brooks/Cole Brooks/Cole 40 Solution Preparation by Dilution M conc V conc = M dil V dil Solution Preparation from Pure Solute Prepare a M solution of potassium permanganate in a ml volumetric flask. M dil = M conc V conc = V dil 17.8 M x 75.0 ml ml = 1.34 M Mass of KMnO 4 = mol x g/mol = g 2008 Brooks/Cole Brooks/Cole 42 7

8 Solution Preparation from Pure Solute Rinse all the solid from the weighing dish into the flask. Fill the flask ⅓ full. Swirl to dissolve the solid. Fill the flask to the mark on the neck. Shake to thoroughly mix. n A = [ A ] x V [product] = n product / (total volume) Brooks/Cole Brooks/Cole 44 H 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 H 2 O(l)? mol x 10 3 mol 2 NaOH 1 H 2 SO 4 H 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 H 2 O(l) n NaOH = L mol L = x 10 3 mol H 2 SO 4 required = x 10 3 mol NaOH 1 H 2SO 4 2 NaOH = x 10 3 mol V acid needed: mol H V = 2 SO 4 = [H 2 SO 4 ] x 10 3 mol 1 L mol = L = 33.4 ml 2008 Brooks/Cole Brooks/Cole 46 A g mixture of oxalic acid, H 2 C 2 O 4 and NaCl was neutralized by ml of 0.550M NaOH. What was the weight % of oxalic acid in the mixture? n NaOH = L x mol/l = mol 1 H 2 C 2 O 4 2 NaOH Oxalic acid reacted = 1 H mol NaOH 2 C 2 O 4 = x10 3 mol 2 NaOH 2008 Brooks/Cole 47 A g H 2 C 2 O 4 / NaCl mixture was neutralized by ml of 0.550M NaOH. What was the weight % of oxalic acid in the mixture? Mass of acid consumed = x10 3 mol x (90.04 g/mol acid) = g of oxalic acid weight of acid Weight percent = sample weight x 100% g Weight percent = x 100% g = 16.08% 2008 Brooks/Cole 48 8

9 25.0 ml of M FeCl 3 and 50.0 ml of M NaOH are mixed. Which reactant is limiting? How many moles of Fe(OH) 3 will form? FeCl 3 (aq) + 3 NaOH(aq) 3 NaCl (aq) + Fe(OH) 3 (s) n FeCl3 = L x mol/l = mol n NaOH = L x mol/l = mol 25.0 ml of M FeCl 3 and 50.0 ml of M NaOH are mixed. Which reactant is limiting? How many moles of Fe(OH) 3 will form? FeCl 3 (aq) + 3 NaOH(aq) 3 NaCl (aq) + Fe(OH) 3 (s) mol mol 1 Fe(OH) mol FeCl 3 3 = mol Fe(OH) 3 1 FeCl 3 1 Fe(OH) mol NaOH 3 = mol Fe(OH) 3 3 NaOH FeCl 3 is limiting; mol produced Brooks/Cole Brooks/Cole 50 Aqueous Solution Titrations Aqueous Solution Titrations Titrant: Base of known concentration Slowly add standard solution. End point: indicator changes color. Determine V titrant added. Often used to determine acid or base concentrations. Unknown acid + phenolphthalein (colorless in acid) turns pink in base 2008 Brooks/Cole Brooks/Cole 52 9

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