1. Titration Chapter 19 section 4
Honors Chemistry

2. Neutralization Strong acid + strong base = salt +H2O
HCl (aq) + NaOH (aq)  NaCl (aq) + H2O (l)
2HNO3 (aq) + Ca(OH)2  Ca(NO3)2 (aq) + 2H2O (l)
How many moles of potassium hydroxide are needed to completely neutralize 1.56 moles of phosphoric acid?
H3PO4 (aq) + 3 KOH (aq)  K3PO4 (aq) + 3H2O (l)
1.56 moles H3PO4 x 3moles KOH/1mole H3PO4 = 4.68 moles KOH

3. Titration
A solution of unknown concentration (analyte) is placed in a flask.
A solution of known concentration (titrant) is placed in buret.
Titrant is added to analyte until indicator changes color

4. Titration The end point is when the indicator changes color.
The equivalence point is when the moles of H+ = moles of OH-

5. Strong Acid/Strong Base with Phenolphtalein

6. Calculating Concentration
How many milliliters of 0.45M HCl will neutralize 25.0ml of 1.00M KOH?
HCl (aq) + KOH (aq)  KCl (aq) + H2O (l)
25.0ml KOH x 1mol KOH x 1molHCl x 1000mL
1000ml molKOH mole HCl
= 56 mL HCl