Aim: What is Titration?
Do Now: Complete and balance the following neutralization reactions:
Neutralization: When _____________ and ______________ solutions are
mixed, the ____ of the acid and the _____ of the base combine to form
__________. The _________ of the acid and the _____________ of
the base come together to form a _________. This is a simple
______________________________ reaction. One mole of _____ ions
exactly neutralizes one mole of _____ ions.
_________ + _________  _________ + ___________
1. Hydrochloric acid is neutralized by sodium hydroxide.
2. Sulfuric acid is added to potassium hydroxide.
3. Nitric acid and calcium hydroxide undergo a neutralization reaction.
Titration: __________________________________________________
__________________________________________________________
Formula:
Titration Procedure: (Unknown base concentration)
1. Put a certain volume of the base into a ______________.
2. Place a certain volume of standardized solution acid with some
_______________________ indicator into an Erlenmeyer flask.
3) Add the base to the acid _______________ until the _______________
just begins to turn color.
4) Record the _______________ of the base necessary to
_______________ the acid.
5) Plug all known values into the formula and solve for MB.
Equivalence Point
_________________ occurs at the
equivalence point when the moles
______ = moles _______
Endpoint
The endpoint occurs when the
________________ change color.
The best indicators give an endpoint close to the equivalence point.
Example: If 20.0 mL of 1.5 M HCl is neutralized by 35.0 mL of NaOH. What is
the molarity of the base?
Titration Practice
1. How many milliliters of a 2.5M HCl solution are required to exactly
neutralize 1500mL of a 5.0M NaOH solution?
2. How many milliliters of a .2M HCl solution are required to neutralize
100mL of a .4M KOH solution?
3. How many mL of a .100M NaOH solution are required to neutralize
20.0mL of a .200M HCl solution?
Monoprotic vs. Diprotic vs. Triprotic
Monoprotic Acids:
Diprotic Acids:
Triprotic Acids:
Each mole of
Each mole of diprotic
Each mole of triprotic
monoprotic acid
acid produces ____
acid produces ____
produces ____ mole of mole of H+ ions.
mole of H+ ions.
H+ ions.
Example:
Example:
Example:
We need to modify the titration equation when dealing with ___________ and
___________ acids.
Let Let nA = moles of H+ produced per mole of acid.
 For HCl nA = _______
 For H2SO4 nA = _______
 For H3PO4 nA = _______
Let nB = moles of OH- produced per mole of base.
 For Ca(OH)2 nB = _______
 For Al(OH)3 nB = _______
Titration equation for diprotic and triprotic acids:
Practice:
1) 50.0 mL of 2.0 M NaOH neutralizes 25.0 mL of HCl. What is
the concentration of the HCl solution?
2) 50.0 mL of 1.5 M H2SO4 neutralizes a 2.0 M sample of NaOH. What volume
of NaOH was neutralized?
Aim: What is Hydrolysis?
Strong Acids
Weak Acids
Strong Bases
Weak Bases
Strong Acid + Strong Base  ________________
Strong Acid + Weak Base  _________________
Weak Acid + Strong Base  _________________
Weak Acid + Weak Base  __________________
General Equation: Salt + Water  Acid + Base
Examples: Complete the equations for each hydrolysis reaction. Determine
whether the following solutions will be acidic, basic, or neutral.
1. NaCl(aq) + H2O 
2. KC2H3O2(aq) + H2O 
3. NaF(aq) + H2O 
4. NH4Cl + H2O 
5. AlCl3(aq) + H2O 