1. Solutions Summary

3. Diluting a solution cDVD = cCVC Amount of moles of
solute after dilution
Amount of moles of solute before dilution =
cDVD = cCVC
Practice problems: p. 404, tutorial 1, p.405 # 1-4

4. Solubility Rules Song (by C. Watt)
The thing about solubility that is great,
It will always dissolve if it is a nitrate.
Something else that is helpful for you and I
It will be soluble if it is ammonium or an alkali.
When I think about chlorides, bromides, and iodides, it hurts my head
Because they are soluble, except with silver, mercury and lead
It gets a lot harder, with sulfates, its true
It’s soluble, except with calcium, strontium, barium, radium, and lead, which all have a charge of plus two.
Now there had to be the insolubles, they cannot hide
Except with cations from #2, carbonate, phosphate, and hydroxide.

5. Using solubility rules to …
Predict whether a salt is soluble or insoluble.
Predict the formation of a precipitate.
Write the net ionic equation

6. Write the balanced chemical, total and net ionic equations:
1. Solutions of sodium chloride and silver nitrate are mixed.
2. Hydrochloric acid and calcium hydroxide solution are mixed.

7. Ionic Dissociation
Definition: dissolving of ionic substances in which ions separate from each other and the crystal Examples: NaCl (s)  Na+(aq) + Cl-(aq) Na2SO4(s)  2Na+(aq) + SO42-(aq) (NH4)3PO4(s) 3NH4+(aq) + PO43-(aq)

8. Solution Stoichiometry
1. Write a balanced chemical equation.
2. Determine the number of moles of the reactants. You will need to use: c=n/V and n=m/M
3. Determine the limiting reagent.
4. Use the limiting number of moles in a ratio to find unknowns.
5. Convert back from moles to mass

9. Solution stoichiometry
NiSO4 + 2 NaOH = Ni(OH)2 + Na2SO4
When 50.0mL of 0.45 mol/L nickel(II) sulphate is reacted with 25.00mL of 1.00mol/L sodium hydroxide, how much precipitate in grams is formed? If 0.60 g is found experimentally, what is the percent yield?
mm: Ni: g/mol, S g/mol, Na g/mol
Hint: Limiting reagent
Ans: 1.16g, 51.7%

10. Electrical Conductivity Conducts electricity
Property
Acids
Bases
Taste
sour
bitter
Electrical Conductivity
Conducts electricity
Feel of solution
No characteristic feel
Feel slippery
Reaction with litmus paper
Turn litmus paper red
Turn litmus paper blue
Reaction with active metals
Produce hydrogen gas
Do not react
Reaction with carbonates
Produce CO2

11. Arrhenius vs Bronsted-Lowry
Arrhenius Acid Any substance that dissociates to form H+ in aqueous solution Base Any substance that dissociates to form 0H- in aqueous solution
Bronsted-Lowry Acid Any substance that provides a proton to another substance Base Any substance that receives a proton from an acid

12. Conjugate Acid-Base Pairs
HBr(aq) + H20(l) -> H30+(aq) + Br-(aq)
Acid – gives up a proton (H+)
Base – accepts a proton (H+)
Conjugate base – particle that has lost the proton.
Conjugate acid – particle that has gained a proton

13. Conjugate Acid-Base Pairs
HBr(aq) + H20(l) -> H30+(aq) + Br-(aq)
Acid – gives up a proton (H+) {HBr(aq) }
Base – accepts a proton (H+){H20(l) }
Conjugate base – particle that has lost the proton. {Br-(aq)}
Conjugate acid – particle that has gained a proton {H30+(aq) }

14. Calculating pH and pOH pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14
[H+] x [OH-] = 1 x 10-14

15. Calculating pH What is the pH of a 0.01M HBr(aq) solution?
What is the pOH and hydroxide ion concentration of the above solution?
What is the pH of a 0.03M HBr(aq) solution?

16. Neutralization Reactions
1. Reaction between an acid and a base produces an ionic compound (a salt) and water
acid + base -> a salt + water
2. Reaction between an acid and a carbonate produces an ionic compound, water and carbon dioxide
Acid + carbonate -> carbon dioxide + water + ionic salt

17. Calculations involving neutralization reactions
Write the balanced equation.
Calculate the number of moles of given acid or base.
Determine the number of moles of acid or base needed. (use mole ratio if necessary).
Calculate the final concentration of the required acid or base.

18. Calculations involving neutralization reactions
A burette is filled almost to the top at the 1.25 mL mark with M NaOH solution. In an Erlenmeyer flask, 20.00mL of hydrosulphuric acid of unknown concentration are placed along with a few drops of phenolphthalein. When the burette is at the 35.55mL mark, the solution in the Erlenmeyer turns light pink. Calculate the molar concentration of the acid and the % m/m. (Note the density of the acid is g/mL).