1. Titration
A standard solution is used to determine the concentration of another solution

2. Titration Usually this is a neutralization reaction.
Acid + Base  salt + water
We use an indicator to tell when all the acid has reacted with all of the base (noted by a color change).
Color change tell you it’s the end point (all acid is neutralized)

3. Neutralization Is the key idea Acid + Base  salt + water
at the neutralization point moles of acid equal moles of base (Hydronium =hydroxide)
at the neutral point (end point) the indicator changes color.
Moles acid = moles base

4. Start with a Standard Solution
This is a solution of known concentration (Molarity).

5. Ex. If 25ml of a .2M solution of NaOH are used to titrate 18ml of HCl, what’s the molarity of the HCl?
Find the moles of base used.
.2 moles
1 L
NaOH
25 ml 1L
1000 ml
= moles
NaOH
This is the amount of NaOH used and its also the amount of hydroxide ions needed to neutralize the acid.

6. Ex. If 25ml of a .2M solution of NaOH are used to titrate 18ml of HCl, what’s the molarity of the HCl?
Moles of base = moles of acid.
0.005 mol
NaOH
1000 ml
1 L
HCl
= 0.28
mol L
= 0.28 M
18 ml

7. Titration
macid * Vacid = mbase * Vbase

8. Titration Strong acid with strong base14
Equivalence
point pH 7 mL

9. Titration Weak acid with strong base14
Equivalence
point pH 7 mL

10. Titration strong acid with weak base14 pH 7
Equivalence
point mL