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Chemical Reactions in Aqueous Chemical Reactions in Aqueous SolutionsSolutions
How do we know whether a reaction occurs? What observations indicate a reaction has occurred?
In your groups, make a list of changes that indicate a chemical reaction has occurred.
22
33
Ag+ + Cl- AgCl
Pb2+ + CrO42-
PbCrO4
Cr3+ + 3OH- Cr(OH)3
returnreturn
44
Ba(OH)2.8H2O + NH4Cl
Thermite: Al + Fe2O3
returnreturn
Cesium in a bathtub
Brainiac Thermite movie
2Al + 3Br2 2AlBr3
55
2Na + Cl2 2NaCl
P4 + 5O2 P4O10
returnreturn
(NH4)2Cr2O7(s) Cr2O3(s) + 4H2O(g) + N2(g)
CuSO4.5H2O CuSO4 + 5H2O(g)
2NI3 N2 + 3I2
66
Heat CuSO4
NI3
returnreturn
77
Na + 2H2O NaOH + H2(g)
Cu + 2H+ Cu2+ + H2(g) Mg + 2HCl
MgCl2 + H2
returnreturn
88
Cu + 2Ag+ Cu2+ + 2Ag Zn + Sn2+ Zn2+ + Sn
returnreturn
99
Cesium in a bathtub
Exploding WhaleBuilding Demolition returnreturn
Substances behave differently when they are placed in water, specifically ionic versus co- valent compounds.
One breaks apart in water, the other does not.
Which one is more likely to be pulled apart by water molecules?
Electrolytes are ionic and strong acid solutions (e.g., GatoradeTM); Nonelectrolytes are covalent compounds (e.g., sugar); weak electrolytes are in between.
Strong/WeakElectrolytes
Strong electrolyte: substance that, when dissolved in water, results in a solution that can conduct electricity (NaCl)
Weak electrolyte: substance that is a poor conductor of electricity when dissolved in water (CH3COOH – vinegar)
Nonelectrolyte: substance that doesn’t conduct electricity when dissolved in water (CH3OH – methanol)
Strong/Weak Electrolytes
3 substances: A2X, A2Y, and A2Z. Which one is the strongest electrolyte? The weakest? (Water has been omitted for clarity.)
Most reactions in general chemistry take place in an aqueous environment. What does that mean?
Terms:◦ Solution: homogeneous mixture of two or more
substances◦ Solute: substance present in smaller amount◦ Solvent: substance present in greater amount◦ Aqueous solution: solvent is water
Three general categories:◦ Precipitation: insoluble (solid) product is formed
from aqueous solutions◦ Acid-base neutralization: acid and base react to
form water and a salt (ionic compound)◦ Oxidation-Reduction: electrons are transferred
between atoms in reaction Combination Decomposition Single-replacement (metal or hydrogen)
Precipitation reactions always begin with two ionic compounds.
Example: NaCl (aq) + AgNO3 (aq) ? Draw these compounds in two separate
aqueous environments. What are the possible products when they are combined?
+
Ag+ NO3-
Ag+
Ag+
NO3-
NO3- Cl-
Cl-
Cl-
Na+
Na+
Na+
Write formulas of products (based on charges), predict phases (Solubility Rules), and balance the equation.
If not covered by the rules, it is probably If not covered by the rules, it is probably insolubleinsoluble.. 1919
Determine if the following ionic compounds will be soluble (aq) or insoluble (s) in water:
K2CO3
BaSO4
PbI2 NaClO4
Ag2S (NH4)3PO4
Cu(OH)2
Determine if the following ionic compounds will be soluble (aq) or insoluble (s) in water:
K2CO3 soluble (aq) BaSO4 insoluble (s) PbI2 insoluble (s) NaClO4 soluble (aq) Ag2S insoluble (s) (NH4)3PO4 soluble (aq) Cu(OH)2 insoluble (s)
There are 3 ways to represent ppt reactions: ◦ As whole compounds (molecular equation)◦ As ionic species (ionic equation) – more accurate◦ As participants in reaction (net ionic equation)
Any aqueous ionic substance is written as a compound (e.g., AgNO3), but this isn’t accurate. What does this look like in water?
Solids, liquids, and gases remain as compounds.
2222
Molecular equation:NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)
Ionic equation (write separate ions for soluble (aq) compounds):Na+(aq) + Cl-(aq) + Ag+(aq) +NO3
-(aq) AgCl(s) + Na+(aq) + NO3
-(aq) Net ionic equation (cancel any identical
ion on both sides of the equation, called spectator ions): Ag+(aq) + Cl-(aq) AgCl(s)
Note: s, l, and g stay together!!!!!
Ag+/Cl- ions
Chemistryhumor, ha ha!
Reaction of lead (II) nitrate and potassium iodide. What is the precipitate?
Write the molecular, ionic, and net ionic equations.
Acid: substance that breaks apart in water to form H+ (e.g., HCl, HNO3, CH3COOH, lemon, lime, vitamin C).◦ HA(aq) H+(aq) + A-(aq)
Base: substance that breaks apart in water to form OH- (e.g., NH3, DranoTM, Milk of MagnesiaTM)◦ MOH(aq) M+(aq) + OH-(aq)
2626
acid base
weak acidstrong acid
You need to KNOW these!!!
Strong acids: HCl, HBr, HI, HClO4, HClO3, H2SO4, HNO3
Strong bases: LiOH, KOH, NaOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
2727
What does “neutralization” mean? How might these two solutions react when
combined?
+OH-
Na+
Na+
OH-
H+
H+ Cl-
Cl-
Neutralization reaction: reaction between acid and base; products are salt (ionic compound) and water
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Acid + base salt + water What are the ionic and net ionic equations
for these reactions? HF(aq) + NaOH(aq) KOH (aq) + H2SO4 (aq)
Acid + Base → H2O + Salt
2HCl(aq) + Mg(OH)2(s) → 2H2O(l) + MgCl2(aq)
Water is created from H+ and OH-
The salt is created from spectator ions
HCl
Mg(OH)2
Complete and balance these equations. Write ionic and net ionic equations, if applicable.
Na2S(aq) + CuCl2(aq) MgSO4(aq) + BaCl2(aq) KNO3(aq) + CaCl2(aq) CuSO4(aq) + NaOH(aq) HF(aq) + NaOH(aq) KOH(aq) + H2SO4(aq)
3131
If not covered by the rules, it is probablyIf not covered by the rules, it is probably insoluble insoluble.. 3232
Na2S(aq) + CuCl2(aq) 2 NaCl(aq) + CuS(s)◦ Cu2+(aq) + S2-(aq) CuS(s)
MgSO4(aq) + BaCl2(aq) MgCl2(aq) + BaSO4(s)◦ Ba2+(aq) + SO4
2-(aq) BaSO4(s)
2 KNO3(aq) + CaCl2(aq) 2 KCl(aq) + Ca(NO3)2(aq)◦ No reaction
CuSO4(aq) + 2 NaOH(aq) Cu(OH)2(s) + Na2SO4(aq)◦ Cu2+(aq) + 2 OH-(aq) Cu(OH)2(s)
HF(aq) + NaOH(aq) H2O (l) + NaF (aq)◦ H+ (aq) + OH- (aq) H2O (l)
2KOH(aq) + H2SO4(aq) 2H2O (l) + K2SO4 (aq)◦ H+ (aq) + OH- (aq) H2O (l)
3333
Determine the products of the reaction. Identify the phase of each compound, and balance the equation. Also write the ionic and net ionic equations.
Molecular: Na2S + Cr(NO3)3
Complete Ionic:
Net Ionic:
Oxidation-Reduction (redox) reactions: electron-transfer reactions
When iron rusts, it loses electrons to form a cation, oxygen gain electrons to form an anion: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)
Use oxidation number rules to determine gain and loss of electrons.
Oxidation numbers are assigned as if elements in compounds completely transferred electrons (like in ionic compounds).
1) An atom (or molecule) in its elemental state has an oxidation number of 0.
2) An atom in a monatomic ion (Na+, Cl-) has an oxidation number identical to its charge.
3a) Hydrogen has an oxidation number of +1, unless it is combined with a metal, in which case it has an oxidation number of –1.
3b) Oxygen usually has an oxidation number of -2. Oxygen in peroxides (O2
2-) has an oxidation number of -1.
3636
3c) Halogens usually have an oxidation number of -1 (except when bonded to oxygen or in polyatomic ions).
4) The sum of oxidation numbers is 0 for a neutral compound and is equal to the net charge for a polyatomic ion. (Example: NaCl = 0, SO4
2- = -2)◦ 4a) For binary ionic compounds, the position
of the element in the periodic table may be useful:
◦ Group IA: +1; Group IIA: +2; Group VIIA: –1; Group VIA: –2; Group VA: –3
3737
H2SO4
H = +1; O = –2 S is unknown, so leave this for last.
◦ The overall charge on this compound is 0.◦ Use algebra to solve for S:◦ 2(+1) + 1(x) + 4(-2) = 0
Solve for each element: MgCr2O7
3838
Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2
CCl4 H2O2
Fe3(PO4)2 MnO4-
NaNO3 KClO4
3939
Determine values of the oxidation number of each element in these compounds or ions:
H2O H: +1, O: -2
SO2 S: +4, O: -2
CCl4 C: +4, Cl: -1
H2O2 H: +1, O: -1
Fe3(PO4)2 Fe: +2, P: +5, O: -2
MnO4- Mn: +7, O: -2
NaNO3 Na:+1, N:+5, O: -2
KClO4 K: +1, Cl: +7, O: -24040
Oxidized: atom, molecule, or ion becomes more positively charged◦Loss of electrons is oxidation (LEO)
Reduced: atom, molecule, or ion becomes less positively charged (reduced charge)◦Gain of electrons is reduction (GER)
Or: OIL RIG (oxidation is loss; reduction is gain)
Redox 2Redox 1
The substance oxidized causes the other substance to be reduced and is called the reducing agent.
The substance reduced causes the other substance to be oxidized and is called the oxidizing agent.
4 Fe(s) + 3O2(g) 2Fe2O3(s)
Identify the element or ion oxidized/reduced. Also identify the oxidizing agent and the reducing agent.
Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)
Oxidized
Reduced
Identify the oxidation number of each element in the compounds or ions below:
Ba(ClO3)2
SO32-
For the reaction below, identify what has been oxidized and reduced; identify the oxidizing agent and the reducing agent.
Cu(s) + 2AgNO3(aq) 2Ag(s) + Cu(NO3)2(aq)
Combination (1 product)◦ Na(s) + Cl2(g)
Decomposition (1 reactant) – usually give off gases◦ CuCO3(s)
Single Replacement (or Displacement) (start and end with an element and a compound)◦ Zn(s) + HCl(aq)
4646
Metals tend to react with water to form bases:◦ 2Na (s) + 2H2O 2NaOH + H2
◦ MgO (s) + H2O Mg(OH)2
Nonmetals tend to react with water to form acids:◦ 2F2 (g) + 2H2O 4HF + O2
◦ CO2 (g) + H2O H2CO3
Alkali metals+ water
CO2 (s) + H2O (l) H2CO3 (aq)
element + element compound◦ H2(g) + O2(g)
metal + nonmetal ionic compound◦ Na(s) + Cl2(g)
nonmetal + nonmetal covalent compound◦ C(s) + O2(g)
Why are these redox reactions?
4949
Mg + O2 K + Cl2
Compound 2 elements; element + compound; or 2 compounds
Oxides, peroxides ◦ Give off O2
Nitrates ◦ Give off NO2 , NO2
-
Carbonates◦ Give off CO2
Ammonium salts ◦ Give off NH3
5151
NH4Cl (s) NiCO3(s) CuO(s)
element + compound compound + element(The more metallic/active element in the compound is displaced.)
Metal Displacement◦ Zn(s) + Cu(NO3)2(aq) Cu(s) + Zn(NO3)2(aq)
Hydrogen Displacement◦ Mg(s) + HCl(aq) MgCl2(aq) + H2(g)
5353
Alkali Metals Zn+SnCl2
5454
The higher the metal on the activity series, the more active that metal.
Translation: higher metals on the chart will form ions as products.
5656
Na + H2O Fe + H2O Fe + Cr(NO3)2
Ni + Pb2+
Ag + Mg2+
Zn + Co2+
5757
React w/ coldwater
React w/ steam
React w/ acid
Four metals (A, B, C, and D) are tested and the following observations are recorded.
A + B+ no reaction C + B+ reaction occurs D + A+ reaction occurs D + B+ no reaction
Burning hydrocarbons CxHyOz + O2 (g) CO2 (g) + H2O (g)
Methanol, CH3OH _CH3OH (l) + _O2 (g) _CO2 (g) + _H2O (g)
Precipitation: use Solubility Rules (AB + CD AD + CB)
Acid-Base Neutralization: acid + base salt + water (AB + CD AD + H2O)
Combination: start with elements (A + B AB)
Decomposition: often produces gas (AB A + B)
Single Displacement: use Activity Series to predict if a reaction occurs (A + BC B + AC)
Combustion: ◦ Hydrocarbon + O2(g) CO2(g) + H2O(g)
+
Na Na Na
NaNa Na
Cl Cl
ClCl Cl Cl
+
Ca Ca Ca CaCa Ca Ca
H+
Cl-
Cl-
Cl-
Cl-
H+
H+
H+
+
Cl-
H+
K+
OH-
OH-K+
H+
Cl-
1. Co(s) + AgNO3(aq)
2. Fe(s) + HCl(aq) 3. Na2CO3(s)
4. Ca(s) + H2O(l) 5. CaCO3(s)
6. HClO4(aq) + KOH (aq)
7. BaCl2(aq) + Na2SO4(aq)
6464
8. HgO(s) 9. LiOH(aq) + H2SO4(aq) 10. Na2CrO4(aq) + Ni(NO3)2(aq) 11. Li(s) + O2(g) 12. Mg(OH)2(aq) + 2HCl(aq) 13. NH3(g) + HCl(g) 14. NiCO3(s) 15. Ca(s) + F2(g)
Single disp. 1. Co(s) + 2AgNO3(aq) Co(NO3)2(aq) + 2Ag(s)Single disp. 2. Fe(s) + 2HCl(aq) FeCl2(aq) + H2(g)Decomp. 3. Na2CO3(s) Na2O(s) + CO2(g)Single disp. 4. Ca(s) + 2H2O(l) Ca(OH)2(aq) + H2(g)Decomp. 5. CaCO3(s) + heat CaO (s) + CO2(g)Acid-base neut. 6. HClO4(aq) + KOH(aq) KClO4(aq) + H2O(l) Precip. 7. BaCl2(aq) + Na2SO4(aq) BaSO4(s) + 2NaCl(aq) Decomp. 8. 2HgO(s) 2Hg(l) + O2(g)
Acid-base neut. 9. 2LiOH(aq) + H2SO4(aq) Li2SO4(aq) + 2H2O(l)Precip. 10. Na2CrO4(aq) + Ni(NO3)2(aq) 2NaNO3(aq) + NiCrO4(s)Combo. 11. 4Li(s) + O2(g) 2Li2O(s)Acid-base neut. 12. Mg(OH)2(aq) + 2HCl(aq) 2MgCl2(aq) + H2O(l)Combo. 13. NH3(g) + HCl(g) NH4Cl(s)Decomp. 14. NiCO3(s) NiO(s) + CO2(g)Combo. 15. Ca(s) + F2(g) CaF2(g)
Predict products of the following reactions. Write correct phases for the products and
balance each equation: ___ Al (s) + ___ NaNO3 (aq) ___ Na (s) + ___ O2 (g) ___ Na2SO4 (aq) + ___ Pb(NO3)2 (aq)
Sections 8.4-8.5
We use the balanced chemical equation to determine relative amounts of reactants and products.
How can we predict the amount of product we should get?
6969
Mass to mass conversions Given mass of reactant, find mass of precipitate: MgCl2 + 2 AgNO3 2 AgCl + Mg(NO3)2
1.2482 g MgCl2 and excess AgNO3
◦ Convert grams of MgCl2 to moles using molar mass
◦ Convert moles of MgCl2 to moles of AgCl using mol-mol ratio
◦ Convert moles of AgCl to grams using molar mass
NaOH + Al(NO3)3 Al(OH)3 + NaNO3
10.54 g xs ?
How many grams of aluminum hydroxide can be made by starting with 10.54 grams of sodium hydroxide? (Hint: Is the equation balanced?)
The mass calculated is the theoretical yield (the most that can theoretically be made in lab).
If you ran that reaction in lab and only obtained
4.9548 g (actual yield) of Al(OH)3, what percent of the maximum did you obtain?
Percent yield = Actual / Theoretical x 100%
Theoretical will be calculated; actual yield will be given in a problem (or obtained in lab)
Analogy: making martinis I have 7 martini glasses, 36 olives, 12 shots
of vodka, and 8 stirrers Each martini requires 1 glass, 2 olives, 2
shots of vodka, and 1 stirrer How many martinis can I make?
7373
Limiting Reactant
7474
How would you define limiting reagent?
7575
2H2 + O2 2H2O
What is the limiting reactant?
7676
2H2 + O2 2H2O
What is the limiting reactant?
2H2 + O2 2H2O
What is the limiting reactant?
7878
2H2 + O2 2H2O
What is the limiting reactant?
7979
2H2 + O2 2H2O
What is the limiting reactant?
8080
2H2 + O2 2H2O
What is the limiting reactant?
8181
Al(s) + Cl2(g) AlCl3(s) Begin with 1.67 g Al (s) and 1.67 g Cl2 (g). Calculate mass of product that can be made
from each reactant? 1) Which reactant produces less product? 2) How many grams of AlCl3(s) will be produced,
theoretically? 3) What is the percent yield if you obtained 1.76
g AlCl3 in the lab? 4) How many grams of the excess reagent will
be left over?
Hydrogen and chlorine react to yield hydrogen chloride. How many grams of HCl are formed from reaction of 3.56 g of hydrogen and 8.94 grams of chlorine?
Sections 9.5-9.6
Consider the reaction:◦ 3CaCl2(aq) + 2Na3PO4(aq) Ca3(PO4)2(s) +
6NaCl(aq) If we mix 25.0 mL of 0.200 M CaCl2
solution with 50.0 mL of 0.250 M Na3PO4 solution, what mass of precipitate is formed?
8585
Complete the equation below (with phases) and balance it.
K2S(aq) + AgNO3(g)
If you combine 10.21 mL of 0.152 M K2S with 1.0092 g AgNO3, how much solid product can be formed?
If 0.2744 g of product were actually formed, what is the percent yield?
Titration: method of determining the concentration (or volume) of an unknown solution by using a solution with a known concentration (standard)◦ moles = M * V
Equivalence point: point at which acid has completely reacted with and been neutralized by base (moles acid = moles base)
End point: point at which the indicator changes color (slight change in solution’s pH)
Titrant in buret (usually) Unknown in flask (usually) Can’t use dilution calculation! Need mol-mol ratio of acid-base Solution stoichiometry: use molarity
to convert between volume and moles (instead of molar mass)◦ M = mol / L
23.78 mL of 0.2500 M NaOH neutralized 20.00 mL of HCl. What is the concentration of HCl? Start with a balanced equation.
Worked Ex. 3.14, Problems 3.20, 3.21, 3.22
How many mL of 1.018 M H2SO4 are needed to neutralize 20.00 mL of 0.9989 M NaOH?◦ Write balanced equation◦ Determine number of moles of known◦ Calculate mole ratio to determine moles of
unknown◦ Divide by concentration to find volume
23.48 mL of lithium hydroxide are required to neutralized 15.39 mL of 1.20 M phosphoric acid. What is the concentration of base?
Concentration: amount of solute present in a given amount of solution
Molarity: moles of solute in 1 L of solution◦ moles solute / liters solution; M = mol / L
1.00 M NaCl = 1.00 mol NaCl in 1 L solution
Knowing concentration, volume, and/or mass allows us to calculate: ◦ 1) mass of solid needed to make a solution of a
certain concentration, or ◦ 2) concentration of solution if mass and volume
are known.
9292
1.00 M NaCl = 1.00 mol NaCl in 1 L solution
0.500 M NaCl = 0.500 mol NaCl in 1 L sol’n.
To find moles of solute: M * V = mol How many moles in 5.67 mL of 0.500
M NaCl? What volume is needed to make a
0.15 M solution using 5.67 mol of solute?
9393
What is the concentration of Cl- ions in a 0.150 M FeCl3 solution?
1 mol FeCl3 1 mol Fe3+ + 3 mol Cl-
0.150 M FeCl3 x (3 mol Cl- / 1 mol FeCl3) = 0.450 M Cl-
We can calculate concentration (molarity) if we know mass and volume.◦ Mass solute ÷ molar mass = moles solute◦ Moles solute ÷ volume solution = Molarity
Or we can calculate the mass of solute needed to make a solution of certain concentration (molarity).◦ Molarity * volume solution = moles solute◦ Moles solute * molar mass = mass solute needed
What is the concentration of a 1.00 L solution made by dissolving 5.00 g NaCl in water?
5.00 grams NaCl in a 500.0 mL solution? What mass of NaCl do we need to make 1.00 L of
a 0.500 M solution?
Dilution: lowering the concentration of solution (by adding water)◦ number of moles of solute stays the same,
amount of solvent increases The number of moles of solute stays the
same; volume increases (lower molarity)◦ moles = M * V◦ Mconc * Vconc = Mdil * Vdil or M1V1 = M2V2
Example: What is the final concentration of solution made by adding 100.0 mL of 3.00 M HCl to 300.0 mL of DI water?
9797
How would you prepare 500.0 mL of 0.500 M H2SO4 starting with concentrated (18.0 M) solution? (Hint: What variable are you solving for?)◦ Remember to add acid to water.
How much water do you need to add to 25.0 mL of a 4.50 M NaOH solution to make a 1.00 M NaOH solution?
1) 13.9 mL of 18.0 M H2SO4 2) 87.5 mL of water added to 25.0 mL of 4.50 M NaOH
Sections 5.8-5.10
Percent by mass: percent by mass of each element in a compound
H2O2
◦ 2 moles H, 2 moles O◦ H = 2 mol x 1.008 g/mol H = 2.016 g H ◦ O = 2 mol x 16.00 g/mol O = 32.00 g O◦ H2O2 = 2.016 g H + 32.00 g O = 34.02 g
◦ %H = 2.016 g H / 34.02 g H2O2 x 100% = 5.926%
What is %O? Solve 2 ways…..
What is the percent by mass of Cr, S, and O in Cr2(SO4)3?
Cr: (104 / 392.21) * 100 = 26.52% S: (96.21 / 392.21) *100 = 24.53% O: (192 / 392.21) * 100 = 48.95%
We can reverse this calculation. Know percentages, need to calculate
empirical formulas.
Calculate the empirical formulas:◦ 50% S, 50% O◦ 43.64% P, 56.36% O
Assume 100 g of the material:◦ 50 g O x 1 mol / 16.0 g = 3.125 mol O◦ 50 g S x 1 mol / 32.066 g = 1.559 mol S◦ mol O / mol S = 3.125 / 1.559 = 2.004 or 2◦ SO2
Assume 100 g of material: ◦ 43.64 g P mol P (1.4089 mol P)◦ 56.36 g O mol O (3.5225 mol O)◦ Ratio of two moles (2.5 O / 1 P); need whole numbers
103103
We just found the empirical formula to be P2O5. This compound has a molecular mass of 141.9 g/mol.
We know the molecular formula has a molar mass of 283.8 g/mol. How many multiples of P2O5 do we need to reach a mass of 283.8?
A compound contains 30.4 % nitrogen and 69.6 % oxygen. The molecular mass of the compound is 92 g/mol.◦ What is the empirical formula of the compound?◦ What is the molecular formula of the compound?
105105
A compound contains 40.00% C, 6.71% H, and the rest is O. Determine the empirical formula of this compound.
If the molar mass of the substance is 180.16 g/mol, determine the molecular formula of this substance.