Download Study Guide – Solutions, Acids, and Bases Solutions: Describe the

Study Guide – Solutions, Acids, and Bases
Solutions:
1.
Describe the difference between homogeneous and heterogeneous mixtures. OMIT
2. What is the solvent and solute of a solution? Solute is dissolved while the solvent does the
dissolving.
3. What does “like dissolves like” refer to? Explain the rule. Polar solvent dissolves polar solutes
while nonpolar solvents dissolves nonpolar solutes.
4. What kinds of things can alcohols dissolve? Polar and nonpolar, because alcohols have a polar
and nonpolar end.
5. How can you tell if something is polar or nonpolar? Polar- unequal sharing of electrons;
nonpolar- equal sharing of electrons
6. What are electrolytes? In general, what KINDS of things are electrolytes? Conduct electric
currents. Ionic compounds, acids, and bases.
7. What does solubility mean? Ability to dissolve in a solvent.
8. Describe the particles in a concentrated versus dilute solution. Same amount of particles, but
more solvent in dilute than concentrated solutions.
9. What do the words “unsaturated”, “saturated”, and “supersaturated” mean? Unsaturated- below
maximum capacity; saturated- at maximum capacity; supersaturated- above maximum capacity
10. How does temperature affect solubility? Increase solubility for solids; decreases solubility for
gases
11. If you wanted to speed up how fast something dissolves, how could you do it? Increase the
temperature, stir it, and crush it.
12. What is molarity? Unit for concentration. Moles/Liters
13. What equation do you use for dilutions? M1V1=M2V2
Acids & Bases:
14. Describe acids. Sour taste, release H+ ions in solution, pH< 7, turn litmus paper red
15. Describe bases. Bitter taste, release OH- ions in solution, pH >7, turn litmus paper blue
16. What are the Arrhenius definitions for acids and bases? Acids give up H+ ions, Bases give up
OH- ions
17. What is the general reaction for a neutralization reaction? Acid + base -> salt + water
18. What salt would form from the reaction of Ca(OH)2 and HBr? CaBr2
19. Write the reaction of H2SO4 + Al(OH)3  H2O + Al2(SO3)3
20. What are the Bronsted-Lowry definitions of an acids and a base? Acids are proton donors and
bases are proton acceptors.
21. Write the conjugate base for each ACID: OMIT
b. HCO3-
a. H2O
c. NH4+
d. HPO42-
22. Write the conjugate acid for each BASE: OMIT
b. HSO4-
a. H2O
c. HPO42-
d. OH-
23. Label the acid, base, conjugate acid and conjugate base for this reaction: OMIT
H2O + HCO3-  H3O+ + CO3224. Sketch the pH scale and label strong acids, weak acids, strong bases, weak bases and neutral.
0
2
Strong acid
4
6
Weak acid
7
8
Neutral
10
12
Weak base
14
Strong Base
25. A pH of 13 is how many times more basic than a pH of 10? OMIT
26. Describe how a strong acid is different from a weak acid. Strong acids completely ionize in
solution (completely let go of H+ ions) while weak acids only partially ionize/break apart.
27. How do you make a strong acid weak? OMIT
28. List the strong acids. HCl, HBr, HF
29. How do you know if a base is strong? Lets go off all of its OH- ions in solution
30. What is a titration? Uses a neutralization reaction to determine the concentration of an acid or
base.
31. What is the standard solution? The solution with a known molarity
32. Write the formula:
a. hydrofluoric acid HF
b. rubidium hydroxide RbOH
c.
sulfuric acid H2SO4
d. copper (II) hydroxide Cu(OH)2
33. Write the name:
a. HNO2 nitrous acid
b. H2SO3 sulfurous acid
c. Mg(OH)2 magnesium hydroxide
d. LiOH lithium hydroxide
Graphs and Problems
1. Which salt is the most soluble at 72oC?
KNO3
2. How much NaNO3 could you put into 300g of
water at 50oC? 336 grams
3. What kind of solution would you have if you
added 80 g of KNO3 to 100g of water at 60oC?
unsaturated
4. What molarity is a solution made from 20g of
NaCl in 400 mL of water? 0.86 M
5. What volume should be used to make a solution
that is 3.0 M if you only have 2 moles of a substance? 0.67 L
6. To what volume should you dilute a solution that has a concentration of 6 molar if you
want to end up with 500 mL of 2.0 M? 166.7 mL or 0.17L
7. What is the pH of a solution with a [H+] of 2.3 x 10-5M? 4.64
8. If a solution has a [OH-] of 4.5 x 10-3M, is it an acid, base, or neutral? pH= 11.66 basic
9. What is the [OH-] if the pH is 3.7? 1 x 10-10.3
10. A student did a titration using 30mL of Ca(OH)2 to neutralize 75mL of 3.4M HCl. What
is the concentration of the base? 8.5 M
State the direction in which each of the following equilibrium systems would be shifted upon the
application of the following stress listed beside the equation.
1. 2 SO2 (g) + O2 (g)
⇄
2 SO3 (g) + energy
decrease temperature
right
⇄
increase temperature
right
2 NO2 (g)
increase total pressure
left
4. CO (g) + H2O (g)
⇄
decrease total pressure
5. 2 NOBr (g) ⇄
2 NO (g) + Br2 (g)
2. C (s) + CO2 (g) + energy
3. N2O4 (g)
⇄
6. 3 Fe (s) + 4 H2O (g) ⇄
2 CO (g)
CO2 (g) + H2 (g)
Fe3O4 (s) + 4 H2 (g)
no shift
decrease total pressure
right
add Fe(s)
right
⇄
7. CaCO3 (s)
8. N2 (g) + 3 H2 (g)
9.
SO3(g)
+
CaO (s) + CO2 (g)
remove CO2 (g)
right
⇄
H2 is added
right
2 NH3 (g)
⇄
H2O(g)
At equilibrium [SO3] = 0.400M
H2SO4(l)
[H2O] = 0.480M
[H2SO4] = 0.600M
Calculate the value of the equilibrium constant.
3.125
10.
H2 (g) + I2 (g) ⇄ 2HI (g)
If at equilibrium [H2] = 0.200M and [I2] = 0.200M and Keq=55.6 at 250oC, calculate the
equilibrium concentration of HI.
1.49
11.
At equilibrium, a 2.0 L flask contains:
0.200 mol of PCl5
0.30 mol of H2O
0.60 mol of HCl
Calculate the Keq for the reaction:
PCl5
0.9
(g)
+ H2O
(g)
⇄ 2HCl
(g)
+ POCl3
(g)
0.300 mol of POCl3