Solution Reactions 1. Electrolytes – Completely Break up into ions in water (Arrhenius, 1884 (Nobel Prize, 1903)). a. Many Ionic Compounds and strong acids (HCl, HBr, HI, HNO 3, H 2 SO 4,HClO 4 ) b. Different than decomposition because ions are produced. Types of Solutions

Solution Reactions c. Examples: NaCl(s)  Na + (aq) + Cl - (aq) CaCl 2 (s)  Ca 2+ (aq) + 2Cl - (aq) Al 2 (SO 4 ) 3 (s)  2Al 3+ (aq) + 3SO 4 2- (aq) Types of Solutions

Solution Reactions

d. Examples Na 2 CO 3 (s)  (NH 4 ) 2 Cr 2 O 7 (s)  HCl(l)  FeCl 3 (s)  e. Hydration Sphere for NaCl Types of Solutions

Solution Reactions

2. Weak Electrolytes a. Weak Acids b. Examples HC 2 H 3 O 2, HF, HNO 2 Types of Solutions

Solution Reactions

3. Non-Electrolytes- Do not break up into ions in water a. Many Molecular Compounds C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) Types of Solutions

Solution Reactions Types of Reactions

Solution Reactions Types of Solutions

Solution Reactions 1.Provide a rough idea of whether something will dissolve in water 2.DO NOT GIVE ACTUAL, NUMERICAL SOLUBILITIES (you must look in a book or do an experiment) Solubility Rules

Solution Reactions Solubility Rules Very SolubleSoluble with exceptions Insoluble with exceptions Li + Na + K + NH 4 + NO 3 - C 2 H 3 O 2 - Cl -, Br -, I - (Except Ag +, Hg 2 2+, Pb 2+ ) SO 4 2- (Except Hg 2 2+,Pb 2+, Ca 2+, Sr 2+, Ba 2+ ) OH -, S 2- (Except Ca 2+, Sr 2+,Ba 2+, & “Very”) CO 3 2-, PO 4 3-, SO 3 2- (Except “Very”)

Solution Reactions Examples: Na 2 CO 3 (s)  Zn(OH) 2 (s)  Na 2 S (s)  CaCl 2 (s)  AgCl(s)  CuCO 3 (s)  Solubility Rules

Solution Reactions Examples: PbSO 4 (s)  Ag 2 SO 4  KCl(s)  Fe(OH) 3 (s)  FeSO 4 (s)  Solubility Rules

Solution Reactions 1.Can be Double Replacement Rxns 2.Spectator Ions – Ions present in soln, but do not take part in the rxn Pb(NO 3 ) 2 (aq) + KI(aq)  Net Ionic Rxns

Solution Reactions BaCl 2 (aq)+K 2 SO 4 (aq) 

Solution Reactions Practice: AgNO 3 (aq) + NaCl(aq)  Net Ionic Rxns

Solution Reactions CaCl 2 (aq) + Na 2 CO 3 (aq)  NaNO 3 (aq) + NH 4 OH(aq)  Na 2 SO 4 (aq) + BaBr 2 (aq)  Fe 2 (SO 4 ) 3 (aq) + LiOH(aq)  Na 2 S(aq) + CuCl 2 (aq)  Pb(C 2 H 3 O 2 ) 2 (aq) + NH 4 OH(aq) 

Solution Reactions 1.The driving force for many reactions is the formation of a: a) Solid (precipitate) b) Liquid c) Gas Net Ionic Rxns

Solution Reactions 1.A special type of double replacement - neutralization 2.Acids a. produce H + b. Often start with H (HCl) 3.Bases a. produce OH - b. Hydroxides (Drano, NaOH) Water forming Rxns

Solution Reactions NaOH (aq) + HCl (aq)  HClO 4 (aq) + LiOH (aq)  Ca(OH) 2 (aq) + HNO 3 (aq)  Mg(OH) 2 (s) + HCl (aq) 

Solution Reactions 1.Carbonates plus acids 2.Carbonic acid – unstable (in soda) H 2 CO 3 (aq)  H 2 O(l) + CO 2 (g) 3. Examples: CaCO 3 (s) + HCl(aq)  MgCO 3 (s) + HNO 3 (aq)  Gas forming Rxns

NaHCO 3 (aq) + HNO 3 (aq)  Na 2 S(aq) + HCl(aq) 

Solution Reactions Mixed Types Fe(NO 3 ) 3 (aq) + Na 2 CO 3 (aq)  SrCO 3 (s) + HCl(aq)  HBr (aq) + LiOH (aq)  Net Ionic Rxns

Solution Reactions Two Types of Chemical Rxns 1.Exchange of Ions – no change in charge/oxidation numbers –Acid/Base Rxns NaOH + HCl

Solution Reactions –Precipitation Rxns Pb(NO 3 ) 2 (aq) + KI(aq) –Dissolving Rxns CaCl 2 (s) 

Solution Reactions 2.Exchange of Electrons – changes in oxidation numbers/charges Cu(s) + 2AgNO 3 (aq)  Cu(NO 3 ) 2 (aq) + 2Ag(s) Remove spectator ions Cu(s) + 2Ag + (aq)  Cu 2+ (aq) + 2Ag(s)

Solution Reactions

Oxidation Numbers 1.Involves taking compounds apart 2.Oxidation numbers – Pretend charges for all compounds (as if they exist as a monoatomic ion) 3.Rules

Solution Reactions Elements = 0 Monoatomic Ions = Charge Use “bankables” to calculate the rest Gr I Gr II O -2 H+H+ F-F- Fe H 2 P 4 Cl 2 Na + O 2- Al 3+ H 2 S Cl 2 O Na 2 SO 4 Fe 2 O 3 PO 4 3- NO 3 - CaCr 2 O 7 SnBr 4 “the higher the oxidation #, the more oxidized the element”

Solution Reactions Review of Oxidation Numbers Calculate the oxidation numbers for: HClO Cr 3+ S 8 Fe 2 (SO 4 ) 3 Mn 2 O 3 SO 3 2- KMnO 4 NO 3 - HSO 4 -

Solution Reactions Oxidation 1.Classical Definition –addition of oxygen Fe + O 2  Fe 2 O 3 2.Modern Definition – an increase in oxidation number Na + O 2  Na 2 O 0 +1 Na was oxidized

Solution Reactions Reduction 1.Classical Definition –addition of hydrogen N 2 + 3H 2  2NH 3 (Haber process) R-C=C-R+ H 2  | | H H (unsaturated fat)(saturated fat)

Solution Reactions 2.Modern Definition –decrease (reduction) in oxidation number N 2 + 3H 2  2NH N was reduced Reduction

Solution Reactions Example In the following rxns, which element is oxidized, which is reduced? Al + HBr  AlBr 3 + H 2 Fe + Cu(NO 3 ) 2  Fe(NO 3 ) 2 + Cu H 2 + O 2  H 2 O

Solution Reactions Activity Series Used to predict if a particular redox reaction will occur Redox reactions - also called single replacement reactions Not every element can replace every other –Higher elements get oxidized –Lower elements get reduced

Solution Reactions

Will Copper metal replace silver in an aqueous solution of silver nitrate?

Solution Reactions Will aqueous iron(II)chloride oxidize magnesium metal?

Solution Reactions Can aluminum foil reduce Fe(NO 3 ) 2 to iron metal?

Solution Reactions Can aluminum foil react with HCl?

Solution Reactions Which of the following metals will be oxidized by Pb(NO 3 ) 2 : Zn, Cu, and/or Fe?

Solution Reactions Will barium metal react with nickel(II)nitrate? Will iron(II)chloride react with calcium metal? Will aluminum chloride react with gold? Will calcium metal dissolve in HNO 3 ?

MgCO 3 (s) + HNO 3 (aq)  Zn(NO 3 ) 2 (aq) + Ag(s)  CuCl 2 (s)  (placed in water) K(s) + NiCl 2 (aq)  Sn(s) + CuCl 2 (aq)  PbSO 4 (s)  (placed in water) Fe(s) + HCl (aq)  Mg(OH) 2 (s) + HCl(aq) 

Identifying Oxidizing/Reducing agents Oxidizing agent – gets reduced Reducing agent – get oxidized K + ZnCl 2  AgNO 3 + Ni  Li + CaCl 2  Cr(NO 3 ) 3 + Na 

Solution Reactions

1.Molarity = measure of the concentration of a solution 2.Molarity = moles/liter Similar to Density = g/L Molarity

Solution Reactions 3.Which is more concentrated? 1 M HCl3 M HCl Crowded classroom example Molarity

Solution Reactions 1.What is the molarity of a soln that contains g of H 2 SO 4 in enough water to make mL of soln? (Ans: 2.00 M) 2.What is the molarity of a soln made by dissolving 23.4 g of Na 2 SO 4 in enough water to make 125 mL of soln? (Ans: 1.32 M) Molarity

Solution Reactions 3.How many grams of NaOH are in 5.00 mL of M NaOH? (Ans: g) 4.What volume of M HCl is needed to provide g of HCl?(Ans: 25 mL) Molarity

Solution Reactions 1.What is the concentration of all the ions in the following solutions? 2 M NaOH 2 M Ca(OH) M K 3 PO 4 Molarity

Solution Reactions 1.Mixing from a solid 2.How would you prepare mL of M Na 2 SO 4 ? (Ans: dilute 24.9 g to 350 mL) Mixing From a Solid

Solution Reactions

3.How would you prepare mL of M KMnO 4 ? (Ans: dilute 10.5 g to 500 mL) 4.How would you prepare mL of M NaOH? (Ans: dilute 0.02 g to 250 mL) Mixing From a Solid

Solution Reactions 1.Dilution Formula: M 1 V 1 = M 2 V 2 2. Used when you are starting with a more concentrated soln. (Grape juice concentrate, Coke syrup) Diluting from a Solution

Solution Reactions

3.What is the molarity of a soln of KCl that is prepared by diluting 855 mL of M soln to a volume of 1.25 L? (Ans: M) 4.You have a 2.5 L bottle of 12.0 M HCl. What volume of it must be diluted to make mL of M HCl? (Ans: 4.17 mL) Diluting from a Solution

Solution Reactions 1.How many grams of water form when 25.0 mL of M HNO 3 is completely neutralized by NaOH? (Ans: g) 2.What volume of M HCl is needed to react completely with 33.1 g of Pb(NO 3 ) 2 ? (Ans: mL) Solution Reactions

3.What is the molarity of an NaOH soln if 22.0 mL is needed to neutralize 15.0 mL of M HCl? (Ans: M) 4.What is the molarity of an NaOH soln if 48.0 mL is needed to neutralize 35.0 mL of 0.144M H 2 SO 4 ? (Ans: M) Solution Reactions

Write net ionic equations: NaHCO 3 (aq) + HNO 3 (aq)  MgCO 3 (s) + HNO 3 (aq)  BaCl 2 (aq) + H 2 SO 4 (aq)  Fe 2 S(s) + HCl(aq)  Write eqns if they occur Fe(NO 3 ) 2 (s)  (placed in water) PbSO 4 (s)  (placed in water) Sn(s) + HCl(aq)  Pt(s) + NiCl 2 (aq) 

Solution Reactions Fe(NO 3 ) 2 (s)  (placed in water) C 2 H 6 (g) + O 2 (g)  K 2 CO 3 (aq) + Fe(NO 3 ) 2 (aq)  K(s) + CoCl 2 (aq)  Mg(OH) 2 (s) + HCl(aq)  CaCl 2 (aq) + Ag(s) 

Solution Reactions 4.CH 3 COOH is a weak electrolyte, HBr is a strong electrolyte, so CH 3 COOH needs to be more concentrated. 16.Mg I - Al NO 3 - H + + ClO 4 - Na + + CH 3 COO -

Solution Reactions 20.Soluble (c), (e) 22. a) Ni(OH) 2 b) NRc) CuS 24.2Cr 3+ (aq) + 3CO 3 2- (aq)  Cr 2 (CO 3 ) 3 (s) Ba 2+ (aq) + SO 4 2- (aq)  BaSO 4 (s) Fe 2+ (aq) + 2OH - (aq)  Fe(OH) 2 (s) 26.CO 3 2- (only one that forms with all three)

95.Al(OH) 3 (s) + 3H + (aq)  Al 3+ (aq) + 3H 2 O(l) Mg(OH) 2 (s) + 2H + (aq)  Mg 2+ (aq) + 2H 2 O(l) MgCO 3 (s) + 2H + (aq)  Mg 2+ (aq)+ H 2 O(l)+CO 2 (g) NaAl(CO 3 )(OH) 2 (s)+ 4H + (aq)  Na + (aq) + Al 3+ (aq) + 3H 2 O(l) + CO 2 (g) CaCO 3 (s) + 2H + (aq)  Ca 2+ (aq)+ H 2 O(l)+CO 2 (g)

Solution Reactions a) Acid/baseb) Redox, Fe reduced c) precipitation d) Redox, Zn oxidized 54.Ni + 2H +  Ni 2+ + H 2 Fe + 2H +  Fe 2+ + H 2 Mg + 2H +  Mg 2+ + H 2 Zn + 2H +  Zn 2+ + H 2 56.Mn + Ni 2+  Mn 2+ + Ni NR 2Cr + 3Ni 2+  2Cr 3+ + Ni NR H 2 + Cu 2+  Cu +2H +

Solution Reactions 62.a) 6.21 X Mb) 1.19 X mol c) 21.6 mL 68.a) 7.18 gb) Mc) 439 mL 70. a) CaCl 2 b) KClc) HCl 72. a) Mb) Mc) M Cl a) 22.5 mLb) M 76. a) 4.46 gb) 14 mL g NaOH 82. a) 2HCl + Ba(OH) 2  BaCl 2 + 2H 2 O (84.2mL) b) 20.0 mLc) Md) g g/quart

Solution Reactions Warm-Up: Zn(NO 3 ) 2 (aq) + K 3 PO 4 (aq)  KNO 3 (aq) + HCl(aq)  Al 2 (CO 3 ) 3 (s) + HCl(aq)  KHCO 3 (aq) + HCl(aq) 

Solution Reactions Bi OH -  Bi(OH) 3 H + + OH -  H 2 O CaCO 3 + 2H +  Ca 2+ + CO 2 + H 2 O Pb 2+ + SO 4 2-  PbSO 4 NR H + + OH -  H 2 O MgCO 3 + 2H +  Mg 2+ + CO 2 + H 2 O Sr 2+ + CO3 2-  SrCO 3 NR Ag + + I -  AgI

Solution Reactions H + + OH -  H 2 O HCO H +  H 2 O + CO 2 SrCO 3 + 2H +  Sr 2+ + CO 2 + H 2 O Pb Cl -  PbCl 2 Cu OH -  Cu(OH) 2

Solution Reactions

What you will turn in: 1.Neatly recopied data table 2.Summary chart of your solubility rules 3.Questions a.Where did your results disagree with the book’s solubility rules? b.Why might this have occurred? c.List three questions you or another student still may have after completing this experiment.