WKS 18
1a. substance present in smaller amount, and substance being dissolved
1b. substance present in larger amount, and is doing the dissolving
1c. the solute and solvent together
2. Water breaks up ionic compounds by using its dipole. The partial positive and negative ends of the
water molecules makes hydrogen bonds to the ionic compounds to break them up and keep them in
solution.
3. Like dissolves like. So, polar things will dissolve polar thing and nonpolar dissolves nonpolar
4. NaCl – solute, water – solvent, Ca- solute, HCl – solvent
5. Electrolyte – produces ions in solution and is a really good conductor of electricity, nonelectrolyte –
does not produce ions in solution and is a really bad conductor of electricity
6. Strong electrolytes fully dissociate into its parts and weak electrolytes only partially dissociate into ions
7. Ca- 2, S- 2, FCl3 -6 overall, KF -2, Mg3P2 – 12.
WKS 19
1. Supersaturated – holding more solute than possible, saturated – holding all solute possible, unsaturated
– more solute can go into solution.
2. 6.1%
3. 7.6%
4. 10.32M
5. new concentration = 7.4M
6. solutions – homogenous mixtures made of small particles, suspensions – large particles that can settle
out, colloids – medium sized particles that can partially disperse light.
7. size of the particles
8. a- sol, b- emulsion, c- foam, d-Aerosol, e –aerosol
WKS 20
1. 0.53 moles NaBr
2. Same number of moles are present, but the concentration changes because diluting the solution
3. 0.65L is the new volume
4. 2798 grams of CaBr2, and 350 is the percent concentration by mass/volume
5. Number 2 is being diluted and if something is being diluted you are dispersing the amount of
solute
6. Osmosis – flow of water through a semipermeable membrane. Isotonic – equal amounts of solute
of either side of the membrane. Hypertonic - more concentration outside than inside. Hypotonic –
low concentration outside, higher inside
7. Water flows from low concentration to high concentration
WKS 21
1. Ability to do work, potential and kinetic
2. Energy is neither created or destroyed, but is transformed
3. Energy needed for a reaction to occur
4. Delta h = Hproducts – Hreactants
5. 22.07 kcal
6. 8.8 kcal
7. Skip number 7 because we didn’t do this one Si, if you want the answer email me
8. Progression of a reaction over time
9. Increase temperature, increase quantity, or add a catalyst
10. A catalyst is something that decreases the activation energy and is not used up in a reaction.
WKS 22
1. Products can become reactants again and vice versa
2. Rate of forward reaction = rate of reverse reaction
3. Factors can shift equilibrium closer to reactants/products.
a. Temp, pressure, and quantity can shift quilibrium
4. Arrhenious – Acids form H+ and bases form OH- in water. Bronsted-Lowry – acids donate an H+
and bases accept a H+
5. Naming acids:
a. Hydrobromic acid
b. Carbonic acid
c. Sulfurous acid
d. Sulfuric acid
e. Hydrochloric acid
6. HClO4, H2SO4, HI, HBr, HCl, HNo3
7. LiOH, NaOH, KOH, Ca(OH)2
8. String acids fully dissociate and weak acids only partially.
9. H30+, when water acts as a Bronsted-Lowry base by accepting a proton.
WKS 23
1. When a pair of molecules are related by the loss or gain of a proton
2.
a. HF (g) + H2O (l)  F- (aq) + H3O+ (aq)
Acid--------------------Base
Base--------------------------Acid
b. NH3 (g) + H2O  NH4+ (aq) + OH-(aq)
Base-------------------acid
Acid-------------------------base
c. H2CO3 (aq) +H2O (l)  H3O+ (aq) + HCO3- (aq)
Acid--------------------------------------------base
Base----------Acid
3. Strong Acids – HClO4, H2SO4, HI, HBr, HCl, HNO3
Strong bases – NaOH, LiOH, Ca(OH)2, and KOH
4. Naming Acids
a. Hydrobromic acid
b. Nitric acid
c. Sulfurous acid
d. Hydrosulferic acid