Chapter 4 Reactions in Aqueous Solution 3 4.1
Pb(NO 3 ) 2 (aq) + 2KI (aq) HCl (aq) + NaOH (aq) Alka-Selter/Water Cu wire/ag(no 3 ) (aq) 3 4.2
(Solution) KMnO 4 (s) K + (aq)+ MnO 4- (aq) 3 4.3
(Molarity) 100 M Al 2 (SO 4 ) 3 Al 3+ (aq) SO 4 2- (aq)? Al 2 (SO 4 ) 3 (s) 2Al 3+ (aq) + 3SO 2-4 (aq) [Al 3+ ] = 0.200 M [SO 2-4 ] = 0.300 M 3 4.4
1. 2. 3.. 4. 5.. 3 4.5
4.2 (Precipitation Reactions) 3 4.6
: Ba(NO 3 ) 2 Na 2 CO 3. What Happen? : Ba 2+, NO 3-, Na +, CO 3 2- : BaCO 3, NaNO 3 BaCO 3 Ba 2+ (aq) + CO 2-3 (aq) BaCO 3 (s) : (spectator) vs. Net Ionic Equation 3 4.7
: BaCl 2, NaOH : Ba 2+, Cl -, Na +, OH - : Ba(OH) 2, NaCl ; no reaction 3 4.8
Cu 2+ (aq) + 2OH - (aq) Cu(OH) 2 (s) 0.100M NaOH 50.0 ml 0.200M CuSO 4? 1.00 L 1 mol Cu 2+ 0.100 mol OH - /L 50mL 1000 ml 2 mol OH - 1 mol CuSO 4 1 mol Cu 2+ 1.00L n NaOH = 0.0125 L = 12.5 ml n CuSO4 0.200 mol CuSO 4 3 4.9
Cu 2+ (aq) + 2OH - (aq) Cu(OH) 2 (s) 6.52 g Cu(OH) 2 (s) 0.200 M Cu(NO 3 ) 2? 1mol Cu(OH) 2 6.52 g Cu(OH) 2 1 mol Cu 2+ 97.57 g Cu(OH) 2 1 mol Cu(OH) 2 1 mol Cu(NO 3 ) 2 1 mol Cu 2+ 1.00L n Cu(OH)2 = 0.334 L = 33.4 ml n Cu(NO3)2 0.200mol Cu(NO 3 ) 2 3 4.10
4.3 - - - 3 4.11
(Acid) H + : HCl, HBr, HI, HNO 3, HClO 4, H 2 SO 4 HCl(aq) H + (aq) + Cl - (aq) HCl(aq) + H 2 O H 3 O + (aq) + Cl - (aq) HCl HF(aq) H + (aq) + F - (aq) HF HF H + F - 3 4.12
(Base) OH - Group I Group II (hydroxides) Ca(OH) 2 (s) Ca 2+ (aq) + 2OH (aq) OH - NH 3 (aq) + H 2 O NH 4+ (aq) + OH (aq) 3 4.13
3 4.14
- : + : HCl + Ca(OH) 2 H + (aq) + OH - (aq) H 2 O + : HF + Ca (OH) 2 HF(aq) + OH (aq) F (aq) + H 2 O + : HCl + NH 3 H + (aq) + NH 3 (aq) NH 4+ (aq) 3 4.15
- 10.0 ml HCl 0.0800 M Ca(OH) 2 25.00 ml HCl? OH - (aq) + H + (aq) H 2 O n OH- = 2 0.0800 0.02500 = 4.00 10-3 = n H+ = n HCl [HCl] = 4.00 10-3 mol 1.00 10-2 L = 0.400 M 3 4.16
4.4 - & Zn(s) + 2H + (aq) Zn 2+ (aq) + H 2 (g) : Zn(s) Zn 2+ (aq) + 2e - : 2H + (aq) + 2e - H 2 (g) 3 4.17
(Oxidation number) Pseudocharge : 0. ex) F in F 2, O in O 2. ex) : Fe 2+ +2, Fe 3+ +3 Group 1 +1, Group 2 +2, 1. ex) K (in KBr, KMnO4) +1 O 2, (H 2 O 2 ) 1, OF 2 +2 H +1, (NaH) -1 3 4.18
( ) ( ) 0,. H 2 SO 4 : (+2) + (ox. no. of S) + 4(-2) = 0; ox. no. of S = +6 Cr 2 O 7 2 : 2(ox. no. of Cr) + 7(-2) = -2; ox no. of Cr = +6 3 4.19
& = = 1 HCl(g) + HNO 3 (l) NO 2 (g) + 2Cl 2 (g) + H 2 O(l) HCl ; Cl -1 0 HNO 3 ; N +5 +4 3 4.20
(Redox Equations) ClO 3- (aq) + I - (aq) Cl - (aq) + I 2 (s) (half-equations:) : I - (aq) I 2 (s) : ClO 3- (aq) Cl - (aq) :.. H + (acidic) OH - (basic).. eg. H 2 O 3 4.21
first half-equation: 2I - (aq) I 2 (aq) 2I - (aq) I 2 (aq) + 2e - second half-equation: ClO 3- (aq) + 6e - Cl - (aq) acid: ClO 3- (aq) + 6H + (aq) + 6e - Cl - (aq) base: ClO 3- (aq) + 6e - Cl - (aq) + 6OH - (aq) acid: ClO 3- (aq) + 6H + (aq) + 6e - Cl - (aq) + 3H 2 O base: ClO 3- (aq) + 3H 2 O+ 6e - Cl - (aq) + 6OH - (aq) Combine half-equations so that electrons cancel acid: 3[2I - (aq) I 2 (s) + 2e - ] ClO 3- (aq) + 6H + (aq) + 6e - Cl - (aq) + 3H 2 O base: 6I - (aq) + ClO 3- (aq) + 6H + (aq) 3I 2 (s) + Cl - (aq) + 3H 2 O 6I - (aq) + ClO 3- (aq) + 3H 2 O 3I 2 (s) + Cl - (aq) + 6OH - (aq) ClO 3- (aq) + I - (aq) Cl - (aq) + I 2 (s) 3 4.22
) Cu(s) + Ag + (aq) Cu 2+ (aq) + Ag(s) Cu(s) Cu 2+ (aq) + 2 e - Ag + (aq) + e - Ag(s) 2Ag + (aq) + 2e - 2Ag(s) Cu(s) + 2Ag + (aq) Cu 2+ (aq) + 2Ag(s) 3 4.23
2) Fe 2+ (aq) + MnO 4 - (aq) Fe 3+ (aq) + Mn 2+ (aq) Fe 2+ (aq) Fe 3+ (aq) + e - (1) MnO 4 - (aq) + 5e - Mn 2+ (aq) (2) MnO 4- (aq) + 5e - + 8H + (aq) Mn 2+ (aq) MnO 4- (aq) + 5e - + 8H + (aq) Mn 2+ (aq) + 4 H 2 O(l) 5Fe 2+ (aq) 5Fe 3+ (aq) + 5e - (1) 5 5Fe 2+ (aq) + MnO 4- (aq) + 8H + (aq) Fe 3+ (aq) + Mn 2+ (aq) + 4 H 2 O(l) (1) 5 + (2) 3 4.24
3, 13, 25, 27, 39, 45, 47, 61, 69, 85 3 4.25