Upload
vine
View
30
Download
3
Embed Size (px)
DESCRIPTION
CHEMICAL RXNS IN AQUEOUS SOLNS (4.4). Chem. Rxns are driven by energetic forces. Precipitation (formation of solid is the driving force). Acid-Base neutralization (formation of water is the driving force). - PowerPoint PPT Presentation
Citation preview
CHEMICAL RXNS IN AQUEOUS SOLNS (4.4)
• Chem. Rxns are driven by energetic forces.• Precipitation (formation of solid is the
driving force).• Acid-Base neutralization (formation of water
is the driving force).• Oxidation-Redox (redox; transfer of
electrons to reduce electrical potential is the driving force).
PRECIPITATION (4.5, 4.7)
• The formation of a solid (precipitate) when two aqueous solutions are mixed; we say that the product cmp is insoluble or only slightly soluble in water.
• Sol. salt I (aq) + Sol. salt II (aq) Solid cmp (s)• Table 4.1 Solubility Rules for Salts in Water
(memorize)• Ion interchange or metathesis (switch
cation/anion partners)
T4.1 SOLUBILITY RULES
1. Most nitrates are soluble2. Most salts with Grp 1A ions and NH4
+ are soluble.
3. Most salts with Cl-, Br-, I- are soluble EXCEPT those with Ag+, Pb2+, Hg2
2+
4. Most sulfates are soluble EXCEPT those with Ba2+, Pb2+, Hg2
2+, Ca2+.5. Most hydroxides are slightly soluble EXCEPT
the strong bases.6. Most sulfides, carbonates, chromates and
phosphates are slightly soluble.
CHEMICAL EQUATION (4.6)
• Identify reactants, products, states of matter [g, s, aq, ℓ].
• Balance equation to conserve mass.
• Calculate quantitative or stoichiometric relationships between rxn participants (R or P) based on balanced chemical rxn.
CHEMICAL EQUATION (2)
• Formula Equation: write all reactants and products as “neutral molecules”, show state of each.
• Complete Ionic Equation: write strong electrolytes as ions (aq).
• Net Ionic Equation: cancel out spectator ions.
SOLUTION STOIOCHIOMETRY
• Typical stoichiometric calculation for reactions taking place in aq soln.
1. Write balanced net ionic eqn to identify the chem reaction
2. Calculate mols of known A from VA and MA
3. Calculate mols of unknown B, then VB
4. VA, MA #mol A #mol B VB if MA and MB are known
5. Determine LR after Step 1 if appropriate.
STOICHIOMETRIC PROBLEMSProb 48, 50
ACID + BASE RXNS
• Acids donate protons, i.e. provide H+(aq) or H3O+ (aq, hydronium) ions in water (Arrhenius).
• Polyprotic acids: sulfuric, phosphoric.
• Bases accept protons.
ACID + BASE RXN: NEUTRALIZATION
• Acid + Base → Salt + Water
• SA + SB: HCl (aq) + NaOH(aq) → NaCl(aq) + H2O(ℓ)
– Net ionic: H+(aq) + OH-(aq) → H2O(ℓ)
• WA + SB: HF(aq) + KOH(aq) → KF(aq) + H2O(l)
– Net ionic: HF(aq) + OH-(aq) → F-(aq) H2O(ℓ)
• SA + WB: Problem 4.57c
ACID-BASE TITRATION (volumetric analysis)
• Exptal technique for determining quantity of an unknown substance (analyte in beaker) by reacting a measured volume of it with another reactant (titrant in buret) of known concentration.
• This method works when the rxn is 100% complete (reaches equivalence pt) and that there is an indicator (color change, pH) that signals the rxn completion (endpoint).
NEUTRALIZATION TITRATION
• Write the balanced acid (assume to be analyte) + base (use strong base) rxn for the titration.
• Use an indicator (e.g. phenolphthalein) that signals the equivalence point.
• The molarity and volume of the titrant (SB) must be known accurately.
• Fig 4.18
NEUTRALIZATION TITRATION Prob 4.66, 64
OXIDATION-REDUCTION REACTIONS
• A redox reaction involves the transfer of electrons between reactants
• Electrons gained by one species must equal electrons lost by another
• Oxidation states or numbers are assigned to atoms and they change in a redox rxn.
• Both oxidation and reduction must occur simultaneously.
2
OXIDATION STATES OR NUMBERS (OX#)
• Actual or imaginary charge on atom: single atom, atom in molecule or atom in polyatomic ion
• We use these to keep track of electrons ub redox rxns.
• We will study rules for assigning OX# and then use this information to balance redox equations
DETERMINING OX# (T4.2)
• OX# of an atom in an element is 0 [Fe, O2]
• If the species is neutral, sum of OX# is 0 [NaCl, SnO4]
• If the species is charged, sum of OX# is value of charge (NH4
+; SO42-)
• OX# of a monatomic ions is its charge: 1A atoms have OX# = +1; 2A atoms have OX# = +2; 7A atoms have OX# = -1, etc
OX# (2)
• In molecular (covalent) cmps O has OX# = -2; sometimes -1 (with metal)
• In molecular (covalent) cmps H has OX# = +1; sometimes -1 (peroxide)
• F always has OX# = -1; other halides can have other OX#s
• There are exceptions
OXIDATION
• If atom X in compound A loses electrons and becomes more positive (OX# increases), we say X (with charge) or A is oxidized.
• Also, we say that A is the reducing agent (RA) or is the electron donor.
REDUCTION
• If atom Y in compound B gains electrons and becomes more negative (OX# decreases), we say Y (with charge) or B is reduced.
• Also, we say that B is the oxidizing agent (OA) or is the electron acceptor.
ACTIVITY SERIES (Expt 7)
• Redox participants have varying capacities to gain or lose electrons.
• The Activity Series lists metal elements in order of decreasing strength as a reducing agent; ie. ability to lose electrons and undergo oxidation.
• A particular rxn in the list will cause the reduction of any rxn below it.
Activity Series of Metals in Aqueous Solution
INTERPRETATION OF ACTIVITY SERIES
• The strongest RA is at the top (Li) meaning that Li loses electrons and is oxidized. Therefore, the other metal must be reduced.
• When Lithium and Calcium react,
• 2Li(s) + Ca2+(aq) 2Li+(aq) + Ca(s)
• We say that Li displaces calcium ion from soln. Li(s) dissolves and Ca(s) forms
BALANCING REDOX EQNS Half-Rxn Method (acid)
• Write half chem eqn for reduction
• Write half chem eqn for oxidation
• Balance all atoms except H and O
• Balance O with H2O and H with H+
Half-Reaction Method (acid, 2)
• Add electrons to balance charge (I.e. show loss or gain of electrons)
• Balance the number of electrons between the two half-rxns by multipying by appropriate factor (i.e. #e- gained by by atom Y = #e- lost by atom X)
• Add two half-rxns and cancel identical species.
• Check for atom and charge balance
The Half-Reaction Method (Acidic Solution)
Half-Reaction Method (base)
• Follow steps for acidic solution
• Add OH- ions to cancel out the H+ ions, thus forming water.
• Cancel out water molecules
• Check for atom and charge balance. Make sure there are no H+ ions remaining.