The student will:
be able to explain the experimental
technique of titration.
math calculate the molarity or volume
of an unknown solution using the
titration formula.
ws.19.3
Neutralization Reaction
Strong acid + Strong Base
HCl + H20
NaOH + H20
salt + water
H+ + ClOH- + Na+
Put them together
HCl + NaOH
NaCl + H2O
Salt: a compound composed of
a cation+ from an base
and an anion- from a acid.
Stomach Ache
CaCO3 ….tums
HCl
+
Mg(OH)2 …milk of magnesia
NaCO3 …. Rolaids
Neutralize …………..salt + H20
HCl + CaCO3
CaCl + CO2 + H20
HCl + Mg(OH)2
MgCl + H20
HCl + NaCO3
NaCl + CO2 + H2O
Titration:
the controlled addition and measurement of of a
solution of known concentration required to react
completely with a measured amount of solution of
unknown concentration
Titration: an experiment, a laboratory technique
chemist use to determine concentration of an
unknown solution.
Resources :
ws 19. 3
Titration Problems
nMV1 = nMV2
1. Your company produces vinegar, acetic acid (HC2H3O2).
Acetic acid is monoprotic. You as the chemist do a quality
control experiment. What is the molarity of your company’s
vinegar if you titrate a 50mL sample with 30mL of 0.25M LiOH?
The vinegar must have a molarity of 0.67M before it can be sold
in grocery stores. Is your company’s vinegar ready for market?
2.
A flask contains 50ml sample of potassium hydroxide.
This solution is titrated and reaches an equivalence point
when 21.88ml of a 0.70M solution H2SO4 is added.
Calculate the molarity of this base sample.
3.
A solution of a triprotic acid H3PO4 is used to titrate
a 16.25mL sample of .5M RbOH solution. The
neutralization point required 25.72mL of the acid. What is
the concentration of the acid?
4.
The chemist used a known concentration of .5M HCl to
titrate an unknown solution of NaOH. Using a 50mL
sample of NaOH the end point was achieved at 32.75mL.
What is the molarity of the NaOH?
• 5.
A volume of 25mL of 2M aluminum hydroxide
neutralizes a 75-mL sample of nitric acid solution. What
is the concentration of the nitric acid?
6.
A 18.5 mL sample of 0.493M KOH solution required
27.7mL of Carbonic acid in a titration experiment.
Calculate the molarity of the acid.
7.
Suppose in a titration experiment it took 22.48mL of
0.454M calcium hydroxide is required to neutralize 10.7mL
of hydrofluoric acid. What is the molarity of the acid
solution?
8. If 25.02mL of a solution of Barium hydroxide requires
18.83mL of a 3.64 M solution of phosphoric acid for
complete titration, what is the molarity of the base solution?
9.
Find the molarity of a Magnesium hydroxide
solution, given that 442mL of it is neutralized in a titration
using 65.8mL of 0.0078M Nitric acid.
The student will:
be able to explain the experimental
technique of titration.
math calculate the molarity or volume
of an unknown solution using the
titration formula.
ws.19.3