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

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)

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

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

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 = 0.005 moles NaOH This is the amount of NaOH used and its also the amount of hydroxide ions needed to neutralize the acid.

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

Titration macid * Vacid = mbase * Vbase

Titration Strong acid with strong base 14 Equivalence point pH 7 mL

Titration Weak acid with strong base 14 Equivalence point pH 7 mL

Titration strong acid with weak base 14 pH 7 Equivalence point mL