SI session Grue 207A
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1 Chem 105 Wednesday 21 Sept Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30 Office hours: Grue 512 MWF 3:304:30 9/21/2011 1
2 Aqueous ionic solutions and ions; Precipitation Reactions 9/21/2011 2
3 Ions in solution (aq) sometimes react to form solid crystal (s) a precipitate. Ag + (aq) + Cl (aq) AgCl (s) Silver (I) ions chloride ions Silver (I) chloride Actually, if we look closely in reactions like this, we can see a very small amount of ions remaining in solution. This is called a dynamic equilibrium. As written, this is a product favored equilibrium reaction. 9/21/2011 3
4 Others ionic compounds readily dissolve in water to form a solution (aq). KMnO 4 (s) K + (aq) + MnO 4 (aq) Potassium permanganate Why do different ionic compounds behave differently in water? 9/21/2011 4
5 H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2 O H 2O H2 O H 2 O H 2 O H 2 O H 2 O H 2 O + H 2 O H 2 O Mutual attractions of ions in crystal VS. Solvation forces on ions in water Crystal forces are stronger for insoluble ionic compounds. Solvation forces are stronger for soluble ionic compounds 9/21/2011 5
6 Solubility = the tendency to form a solution when a solid is place in water. 9/21/2011 6
7 How to predict if a precipitate will form: 1. Interchange the cationanion pairs. 2. Form the (correct) new ionic compounds. 3. Check the known solubilities of the new compounds. 4. (Learn and use the Solubility Rules ) 9/21/2011 7
8 Kotz Solubility Rules S O L U B L E C O M P O U N D S All salts of Na +, K +, NH4 + Salts of nitrate, NO 3 chlorate, ClO 3 perchlorate, ClO 4 acetate, CH 3 CO 2 Almost all salts of Cl, Br, I A salt is any ionic compound that is not an acid or base. E X C E P T I O N S Halides of Hg 2 2+, Pb 2+, Ag + Salts containing F (Don t worry about fluorides.) Fluorides of Mg 2+, Ca 2+, Sr 2+, Ba 2+, Pb 2+ Salts of sulfate, SO 2 4 Sulfates of Ca 2+, Sr 2+, Ba 2+, Pb 2+, Ag + 9/21/ Fig. 3.10, p. 122 (also) Hg 2 2+
9 For example, CdS is NOT soluble, but (NH 4 ) 2 S IS soluble. I N S O L U B L E C O M P O U N D S Most salts of carbonate, CO 3 2 Phosphate, PO 4 3 Oxalate, C 2 O 4 2 Chromate, CrO 4 2 Sulfide, S 2 E X C E P T I O N S Salts of NH 4 + and the alkali metal cations Most metal hydroxides and oxides Alkali metal hydroxides; Sr(OH) 2 Ba(OH) 2 9/21/2011 9
10 I N S O L U B L E C O M P O U N D S Most salts of carbonate, CO 3 2 Phosphate, PO 4 3 Oxalate, C 2 O 4 2 Chromate, CrO 4 2 Sulfide, S 2 E X C E P T I O N S Salts of NH 4 + and the alkali metal cations Most metal hydroxides and oxides Alkali metal hydroxides; Sr(OH) 2 Ba(OH) 2 9/21/
11 I N S O L U B L E C O M P O U N D S Most salts of carbonate, CO 3 2 Phosphate, PO 4 3 Oxalate, C 2 O 4 2 Chromate, CrO 4 2 Sulfide, S 2 Most metal hydroxides and oxides Not in OWL table, but NEED to REMEMBER too. E X C E P T I O N S Salts of NH 4 + and the alkali metal cations Alkali metal hydroxides; Ba(OH) 2 Sr(OH) 2 9/21/
12 OWL Solubility Rules 9/21/
13 Writing equations for precipitation reactions. 9/21/
14 Not balanced Pb(NO 3 ) 2 (aq) + KI (aq) PbI 2 (s) + KNO 3 (aq) Lead (II) nitrate Potassium iodide Lead (II) iodide Potassium nitrate (Called a metáthesis, or double exchange, reaction.) Pb(NO 3 ) 2 (aq) + 2 KI (aq) PbI 2 (s) + 2KNO 3 (aq) 9/21/
15 The Net Ionic Equation (N.I.E.) summarizes what really happens, and leaves out spectator ions Pb(NO 3 ) 2 (aq) + 2 KI (aq) PbI 2 (s) + 2KNO 3 (aq) Split into ions Pb 2+ (aq) + 2 NO 3 (aq) Split into ions DO NOT Split into ions PbI 2 (s) Split into ions + 2 K + (aq) + 2 I (aq) + 2 K + (aq) + 2 NO 3 (aq) Pb 2+ (aq) + 2 I (aq) PbI 2 (s) 9/21/
16 Net Ionic Equation (N.I.E.) Pb(NO 3 ) 2 (aq) + 2 KI (aq) PbI 2 (s) + 2KNO 3 (aq) Split into ions Pb 2+ (aq) + 2 NO 3 (aq) Split into ions DO NOT Split into ions PbI 2 (s) Split into ions + 2 K + (aq) + 2 I (aq) + 2 K + (aq) + 2 NO 3 (aq) Spectator Ions remain in solution (because KNO 3 is soluble.) Pb 2+ (aq) + 2 I (aq) PbI 2 (s) 9/21/
17 When aqueous solutions of AgNO 3 and CaBr 2 are mixed, a precipitate forms. Which ions remain in solution, i.e. are spectator ions? 1. Ca 2+ and Ag + 2. NO 3 and Br 3. Ca 2+ and NO 3 4. Ag + and NO 3 Ca(NO 3 ) 2 and AgBr Ca2+ and Ag+ 21 NO3 and Br 38 Ca2+ and NO Ag+ and NO
18 Kotz Solubility Rules S O L U B L E C O M P O U N D S All salts of Na +, K +, NH4 + Salts of nitrate, NO 3 chlorate, ClO 3 perchlorate, ClO 4 acetate, CH 3 CO 2 Almost all salts of Cl, Br, I E X C E P T I O N S Halides of Hg 2 2+, Pb 2+, Ag + Salts containing F (Don t worry about fluorides.) Fluorides of Mg 2+, Ca 2+, Sr 2+, Ba 2+, Pb 2+ Salts of sulfate, SO 2 4 Sulfates of Ca 2+, Sr 2+, Ba 2+, Pb 2+, Ag + 9/21/ Fig. 3.10, p. 122 (also) Hg 2 2+
19 A text file of formulas 9/21/
20 OWL 3.5k Write NIE: carbonate and phosphate Hint: Not all the boxes need to be filled. If there is no NIE, leave all boxes blank. Also, use the text file on the course website to speed chemical formula entry. 9/21/
21 Acids and Bases 9/21/
22 Acid = A compound that forms H 3 O + (hydronium) ions when dissolved in water. Base = A compound that forms OH (hydroxide) ions when dissolved in water. HCl (aq) + H 2 O (l) Cl (aq) + H 3 O + (aq) KOH (aq) K + (aq) + OH (aq) 9/21/
23 Can also use this idea to define STRONG and WEAK acids and bases: Strong acid = reacts nearly completely to form H 3 O + and anion. Weak acid = reacts only partially, leaving a lot of intact acid molecules. Strong base = completely splits into a cation and OH ion(s) Weak base = forms a low concentration of OH ions. 9/21/
24 HCl (aq) + H 2 O (l) Cl (aq) + H 3 O + (aq) H Cl H 3 O + (aq) Cl (aq) HCl (aq) HCl transfers H + to nearby H 2 O. 9/21/
25 HCl (aq) + H 2 O (l) Cl (aq) + H 3 O + (aq) This is a productfavored reaction. >99.99% of HCl is ionized in aqueous solution. This behavior DEFINES a strong acid. 9/21/
26 Strong acids whose formulas and names you should know: (See Table 3.1 p. 129) HCl HBr HI HNO 3 HClO 4 H 2 SO 4 Hydrochloric acid Hydrobromic acid Hydroiodic acid Nitric acid Perchloric acid Sulfuric acid 9/21/
27 If 1.0 mol of sulfuric acid (H 2 SO 4 ) is dissolved in water, what will happen? 1. Form 1.0 mole of H 2 SO 4 molecules moles of ions are formed moles of ions are formed Can t tell: need to know the water volume Form 1.0 mole moles of i moles of i... Can t tell: ne
28 1. Form 1.0 mole of H 2 SO 4 molecules moles of ions are formed moles of ions are formed 4. Can t tell: need to know the water volume H 2 SO 4 (aq) 2 H + (aq) + SO 4 2 (aq) 9/21/
29 Weak acids Definition: Weak acids, when dissolved in water, form only small % H 3 O +. (Say % up to ~10%) Acetic acid CH 3 CO 2 H (aq) + H 2 O (l) Acetate anion CH 3 COO (aq) + H 3 O + (aq) 99.99% 0.01% 9/21/
30 Weak acids whose names and formulas you should know: (Table 3.1, p. 129) HF Hydrofluoric H 3 PO 4 Phosphoric acid H 2 CO 3 Carbonic acid CH 3 CO 2 H Acetic acid H 2 C 2 O 4 Oxalic acid.... (others not on exams) 9/21/
31 Why are some acids STRONG and others WEAK? It depends on the stability and solvation of the ANION that is formed by H + loss. Very stable anion = strong acid Less stable anion = weaker acid O H O H + + O S O H O S O O O + H + Partially positive S atom stabilizes the 1 charge in hydrogen sulfate ion. 9/21/
32 Strong acidstrong base reaction: neutralization Acid + base > salt + H 2 O (l) A salt contains the cation from a base and the anion from an acid. NaOH (aq) + HCl (aq) > NaCl (aq) + H 2 O (l) Write the Net Ionic Equation Na + (aq) + OH (aq) + H + (aq) + Cl (aq) > Na + (aq) + Cl (aq) + H 2 O (l) OH (aq) + H + (aq) > H 2 O (l) 9/21/
33 Weak acidstrong base neutralization Acid + base > Salt + H 2 O (l) A salt contains the cation from a base and the anion from an acid. CH 3 CO 2 H (aq) + NaOH (aq) NaCH 3 CO 2 (aq) + H 2 O (l) Write the Net Ionic Equation CH 3 CO 2 H (aq) + Na + (aq) + OH (aq) Na + (aq) + CH 3 CO 2 (aq) + H 2 O (l) OH (aq) + CH 3 CO 2 H (aq) CH 3 CO 2 (aq) + H 2 O (l) 9/21/
34 The End 9/21/
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