Mass Relationships
By
Doba Jackson, Ph.D.
Balancing Chemical Equations
A balanced chemical equation shows that the law of
conservation of mass is adhered to.
In a balanced chemical equation, the numbers and
kinds of atoms on both sides of the reaction arrow are
identical.
2Na(s) + Cl2(g)
2NaCl(s)
left side:
right side:
2 Na
2 Cl
2 Na
2 Cl
Chemical Symbols on a
Different Level
2H2(g) + O2(g)
microscopic:
2H2O(l)
2 molecules of hydrogen gas react with
1 molecule of oxygen gas to yield 2
molecules of liquid water.
Chemical Symbols on a
Different Level
2H2(g) + O2(g)
2H2O(l)
microscopic:
2 molecules of hydrogen gas react with
1 molecule of oxygen gas to yield 2
molecules of liquid water.
macroscopic:
0.56 kg of hydrogen gas react with
4.44 kg of oxygen gas to yield 5.00 kg
of liquid water.
Chemical Arithmetic:
Stoichiometry
How many grams of each reactant is needed and
how many grams of the product are expected?
Chemical Arithmetic:
Stoichiometry
Molecular Mass: Sum of atomic masses of all atoms
in a molecule.
Formula Mass: Sum of atomic masses of all atoms in
a formula unit of any compound, molecular or ionic.
C2H4:
HCl:
2(12.0 amu) + 4(1.0 amu) = 28.0 amu
1.0 amu + 35.5 amu = 36.5 amu
Chemical Arithmetic:
Stoichiometry
One mole of any substance is equivalent to its
molecular or formula mass.
C2H4:
1 mole = 28.0 g
6.022 x 1023 molecules = 28.0 g
HCl:
1 mole = 36.5 g
6.022 x 1023 molecules = 36.5 g
Chemical Arithmetic:
Stoichiometry
How many moles of chlorine gas, Cl2, are in 25.0 g?
25.0 g Cl2
x
1 mol Cl2
70.9 g Cl2
= 0.353 mol Cl2
Chemical Arithmetic:
Stoichiometry
How many grams of sodium hypochlorite, NaOCl, are in
0.705 mol?
0.705 mol NaOCl
74.5 g NaOCl
x
Na = 22.99 amu
O = 15.99 amu
Cl = 35.45 amu
1 mol NaOCl
= 52.5 g NaOCl
Chemical Arithmetic:
Stoichiometry
Stoichiometry: The relative proportions in which
elements form compounds or in which substances
react.
aA + bB
Grams of
A
Molar Mass
of A
Moles of
A
cC + dD
Moles of
B
Mole Ratio
Between A
and B
(Coefficients)
Grams of
B
Molar Mass
of B
Chemical Arithmetic:
Stoichiometry
Aqueous solutions of sodium hypochlorite (NaOCl), best
known as household bleach, are prepared by reaction of
sodium hydroxide with chlorine gas:
2NaOH(aq) + Cl2(g)
NaOCl(aq) + NaCl(aq) + H2O(l)
How many grams of NaOH are needed to react with 25.0 g
Cl2?
Grams of
Cl2
Molar Mass
Moles of
Cl2
Mole Ratio
Moles of
NaOH
Grams of
NaOH
Molar Mass
Chemical Arithmetic:
Stoichiometry
Aqueous solutions of sodium hypochlorite (NaOCl), best
known as household bleach, are prepared by reaction of
sodium hydroxide with chlorine gas:
2NaOH(aq) + Cl2(g)
NaOCl(aq) + NaCl(aq) + H2O(l)
How many grams of NaOH are needed to react with 25.0 g
Cl2?
25.0 g Cl2
x
1 mol Cl2
70.9 g Cl2
= 28.2 g NaOH
2 mol NaOH
x
1 mol Cl2
40.0 g NaOH
x
1 mol NaOH
Concentrations of Reactants in
Solution: Molarity
Molarity (M): The number of moles of a substance
dissolved in each liter of solution. In practice, a
solution of known molarity is prepared by weighing an
appropriate amount of solute, placing it in a container
called a volumetric flask, and adding enough solvent
until an accurately calibrated final volume is reached.
Solution: A homogeneous mixture.
Solute: The dissolved substance in a solution.
Solvent: The major component in a solution.
Concentrations of Reactants in
Solution: Molarity
Molarity converts between mole of solute and liters of
solution:
Moles of solute
Molarity =
Liters of solution
1.00 mol of sodium chloride placed in enough water to
make 1.00 L of solution would have a concentration
equal to:
1.00 mol
1.00 L
= 1.00
mol
L
or 1.00 M
Concentrations of Reactants in
Solution: Molarity
How many grams of solute would you use to prepare
1.50 L of 0.250 M glucose, C6H12O6?
Molar mass C6H12O6 = 180.0 g/mol
1.50 L 0.250 mol
x
= 0.375 mol
1L
0.375 mol
x
180.0 g
1 mol
= 67.5 g
Diluting Concentrated
Solutions
concentrated solution + solvent
dilute solution
initial
final
Mi x Vi = Mf x Vf
Since the number of moles of solute remains constant,
all that changes is the volume of solution by adding
more solvent.
Diluting Concentrated
Solutions
Sulfuric acid is normally purchased at a concentration of
18.0 M. How would you prepare 250.0 mL of 0.500 M
aqueous H2SO4?
Vi =
Mi = 18.0 M
Mf = 0.500 M
Vi = ? mL
Vf = 250.0 mL
Mf
Mi
x
Vf
0.500 M
=
18.0 M
250.0 mL
x
= 6.94 mL
Add 6.94 mL 18.0 M sulfuric acid to enough water to
make 250.0 mL of 0.500 M solution.
Solution Stoichiometry
aA + bB
Volume of
Solution of A
Molarity of
A
Moles of
A
cC + dD
Moles of
B
Mole Ratio
Between A
and B
(Coefficients)
Volume of
Solution of B
Molar Mass
of B
Solution Stoichiometry
What volume of 0.250 M H2SO4 is needed to react with
50.0 mL of 0.100 M NaOH?
H2SO4(aq) + 2NaOH(aq)
Volume of
Solution of H2SO4
Molarity of
H2SO4
Moles of
H2SO4
Na2SO4(aq) + 2H2O(l)
Moles of
NaOH
Mole Ratio
Between H2SO4
and NaOH
Volume of
Solution of NaOH
Molarity of
NaOH
Solution Stoichiometry
H2SO4(aq) + 2NaOH(aq)
Na2SO4(aq) + 2H2O(l)
Moles of NaOH available:
50.0 mL NaOH
0.100 mol
x
1L
1L
x
1000 mL
= 0.00500 mol NaOH
Volume of H2SO4 needed:
0.00500 mol NaOH 1 mol H2SO4
1 L solution
1000 mL
x
x
x
2 mol NaOH 0.250 mol H2SO4
1L
10.0 mL solution (0.250 M H2SO4)
Titration
Titration: A procedure for determining the concentration
of a solution by allowing a carefully measured volume to
react with a solution of another substance (the standard
solution) whose concentration is known.
HCl(aq) + NaOH(aq)
NaCl(aq) + 2H2O(l)
Once the reaction is complete you can calculate the
concentration of the unknown solution.
How can you tell when the reaction is complete?
Titration
buret
Erlenmeyer
flask
standard solution
(known concentration)
unknown concentration solution
An indicator is added which changes
color once the reaction is complete
Titration
48.6 mL of a 0.100 M NaOH solution is needed to react
with 20.0 mL of an unknown HCl concentration. What is
the concentration of the HCl solution?
HCl(aq) + NaOH(aq)
Volume of
Solution of NaOH
Molarity of
NaOH
Moles of
NaOH
NaCl(aq) + 2H2O(l)
Moles of
HCl
Mole Ratio
Between NaOH
and HCl
Volume of
Solution of HCl
Molarity of
HCl
Titration
HCl(aq) + NaOH(aq)
NaCl(aq) + 2H2O(l)
Moles of NaOH available:
48.6 mL NaOH 0.100 mol
1L
x
x
= 0.00486 mol NaOH
1L
1000 mL
Moles of HCl reacted:
0.00486 mol NaOH 1 mol HCl
= 0.00486 mol HCl
x
1 mol NaOH
Concentration of HCl solution:
0.00486 mol HCl
20.0 mL solution
1000 mL
x
1L
= 0.243 M HCl
Problem: What is the molecular mass
of table sugar (sucrose, C12H22O11), and
what is its molar mass in g/mol?
Problem: How many moles of
sucrose are in a tablespoon of
sugar containing 2.85 g?
Problem: How many grams are
in 0.0626 mol of NaHCO3, the
main ingredient of Alka-Seltzer
tablets?
Problem: Cisplatin, an anticancer agent used for
the treatment of solid tumors, is prepared by the
reaction of ammonia with potassium
tetrachloroplatinate. Assume that 10.0 g of
K2PtCl4 and 10.0 g of NH3 are allowed to react.
(a) Which reactant is limiting, and which is in
excess?
(b) How many grams of the excess reactant are
consumed, and how many grams remain?
(c) How many grams of cisplatin are formed?