Phase Diagram Worksheet
For each of the questions on this worksheet, refer to the phase diagram for
mysterious compound X.
1)
What is the critical temperature of compound X? ~7700 C
2)
If you were to have a bottle containing compound X in your closet, what
phase would it most likely be in?
Extrapolating from this diagram, it’s most likely a gas.
3)
At what temperature and pressure will all three phases coexist?
3500 C, ~51 atm
4)
If I have a bottle of compound X at a pressure of 45 atm and temperature
of 1000 C, what will happen if I raise the temperature to 4000 C?
It will sublime
5)
Why can’t compound X be boiled at a temperature of 2000 C?
It does not form a liquid at this temperature. It only exists as a liquid
at temperatures above 3500 C.
6)
If I wanted to, could I drink compound X?
No. At the temperatures and pressures that it forms a liquid, you’d
probably die.
1. What is the concentration of lead (II) chromate if 8.6 x 10-5 g are used to
make 2 L of solution?
1.33 x 10-7 M
2. How many grams of sulfuric acid are contained in .8 L of .05 M solution?
3.92 g
3. What volume of .839 M acetic acid contains 1.25 mols of acetic acid?
1.49 L
4. What is the concentration of solution that results from diluting 25 mL of
2.04 M solution of methanol (CH3OH) to 500 mL?
.102 M
5. What volume of .12 M hydrobromic acid can be prepared from 11 mL of
.45 M hydrobromic acid?
.04125 L
6. A laboratory experiment calls for .125 M nitric acid. What volume of .125
M solution can be prepared from .250 L of 1.88 M nitric acid?
3.76 L
7. What volume of 1.59 M potassium hydroxide is required to prepare 5 L of
.1 M potassium hydroxide?
.314 L
8. What volume of a .575 M solution of glucose can be prepared from 50 mL
of 3 M glucose?
.261 L
9. What volume of .75 M solution of hydrochloric acid can be prepared from
the hydrochloric acid produced from the reaction of 25 g of sodium
chloride with an excess of sulfuric acid?
.57 L
10. What volume of .2089 M potassium iodide contains enough potassium
iodide to react exactly with the copper (II) nitrate found in 43.88 mL of a
.3842 M solution of copper (II) nitrate?
.161 L
Write the total and net ionic equations for the following using the
procedure above.
1. ___Zn (s) +___ HCl (aq) ----->___ ZnCl2 (aq) + ___H2 (g)
Zn + 2 H+1  Zn+2 + H2
2. ___FeCl3 (aq) +___ AgNO3 (aq) ------>___ AgCl (s) +___ Fe(NO3)3 (aq)
3 Ag+1 + 3 Cl-1  3 AgCl
3. ___KOH (aq) + ___H3PO4(aq) ------>___ K3PO4(aq) +___ H2O (l)
H+ + OH-1 H2O
4. ___HCl (aq) + ___ Na2CO3 (aq) -----> ___ H2O(l) + ___CO2(g) + ___NaCl
(aq)
2 H+1 + CO3-2  H2O + CO2
5. ___KOH (aq) + ___Fe2(SO4)3 (aq) -----> ___ Fe(OH)3 (s) + ___ K2SO4
(aq)
2 Fe+3 + 6 OH-1  2 Fe(OH)3
1:3:1
6. ___Mg (s) + ___AgNO3 (aq) -----> ___Ag (s) + ___ Mg(NO3)2 (aq)
Mg + 2 Ag+1  2 Ag + Mg+2
7. ___NaOH (aq) + ___CO2 (g) -----> ___Na2CO3 (aq) + ___H2O (l)
2 OH-1 + CO2  CO3-2 + H2O
8.
_____Al + _____H2SO4  _____Al2(SO4)3 + _____H2
2 Al + 6 H+  2 Al+3 + 3 H2
Colligative Properties:
1. What are the boiling and freezing points of 115 g of sucrose (C12H22O11)
in 350 g of water?
Kb of water = .512 °C/m Kf of water = 1.86 °C/m
B = 100.491 °C ; f = -1.79
2. Determine the vapor pressure of a solution of 92.1 g of glycerin
C3H5(OH)3 in 184.4 g of ethanol C2H5OH at 40 °C. The vapor pressure of
pure ethanol at 40 °C is .178 atm.
P’= (.80)(.178 atm)=.142 atm
3. What is the boiling point of a solution of 1 g of glycerin in 47.8 g of water?
100.116 °C
4. A solution contains 5 g of urea CO(NH2)2 per .1 kg of water. What is the
vapor pressure of the solution at 26 °C?
24.84 mmHg
5. 15 g of aluminum chloride are added to 350 mL of water at 20 °C. What
are the boiling point and vapor pressure of the solution?
B = 100.66 °C, P’ = (.977)(17.5 mmHg) = 17.1 mmHg
6. 100 g of ethanol are mixed with 100 g of water at 40 °C. What is the vapor
pressure of the solution?
P=PH2O + Pethoh = 55.3 mmHg + 140 mmHg =195.3 mmHg
Osmotic Pressure:
1. What is the osmotic pressure of an aqueous solution of 1.64g of calcium
nitrate in water at 25 °C? The volume of the solution is 275 mL.
2.67 atm
2. The osmotic pressure of a solution that contains 7 g of insulin per liter is
23 torr at 25 °C. What is the formula mass of insulin?
5700 g/mol
Misc:
1. The vapor pressure of methanol CH3OH is 94 Torr at 20 °C. The vapor
pressure of ethanol C2H5OH is 44 Torr at the same temp. Both of these
are volatile substances. If a solution contain 50 g of each, what is the
vapor pressure of each? What is the total pressure in the container?
Xtot = 2.65 moles
P’meoh = 55.33 torr P’etoh = 18.1 torr Ptot = 73.43 torr
2. A solution of barium hydroxide is .1055 M. What volume of .5 M nitric
acid is required in the neutralization of 15.5 mL of barium hydroxide?
6.54 mL
3. The sulfate in 50 mL of dilute sulfuric acid was precipitated using excess
barium chloride. The mass of barium sulfate formed was .482 g.
Calculate the molarity of the sulfuric acid.
.041 M
4. An organic compound has a composition of 93.46% C and 6.54% H by
mass. A solution of .090 g of this compound in 1.10 g of camphor melts at
158.4 °C. The melting point of pure camphor is 178.4 °C. Kf for camphor
is 37.7 °C/m. What is the molecular formula of the solute?
C12H10