V. Acid-Base Titration Titration is the process of adding a measured volume of an acid or base of known molarity (the standard solution) to an acid or.

V. Acid-Base Titration

Titration is the process of adding a measured

volume of an acid or base of known molarity

(the standard solution) to an acid or base of

unknown molarity until neutralization occurs.

standard solution – known molarity (concentration)

unknown molarity

An indicator is added to the flask. It changescolor when neutralization has occurred.

Remember:

acid + base water + salt

The net ionic equation of what really reacts is:

H+ + OH- H2O

Neutralization occurs when the

number of moles of = number of moles ofH+ from the acid OH- from the base

molarity = moles solute liters of soln.

molarity = moles volume

molarity x vol. = moles

Remember:

acid + base water + salt

The net ionic equation of what really reacts is:

H+ + OH- H2O

Neutralization occurs when the

number of moles of = number of moles ofH+ from the acid OH- from the base

(molarity x volume)acid = (molarity x volume)base

MAVA = MBVB (in Table T)

Remember:

acid + base water + salt

The net ionic equation of what really reacts is:

H+ + OH- H2O

Neutralization occurs when the

number of moles of = number of moles ofH+ from the acid OH- from the base

(molarity x volume)acid = (molarity x volume)base

MAVA = MBVB (in Table T)

Volumes VA and VB must be in the same units (mL or L).

Ex. How many milliliters of 4.00 M NaOH are required to neutralize 50.0 milliliters of 2.00 M solution of HNO3?

MAVA = MBVB

(2.00 M)(50.0 mL) = (4.00 M) x

(2.00 M)(50.0 mL) = x 4.00 M

25 mL = x

Note: 2x the concentration ½ as much needed

Ex. What is the molarity of an HCl solution if 30. mL of the acid are needed to neutralize 10. mL of a 6.0 M NaOH solution?

MAVA = MBVB

x (30. mL) = (6.0 M)(10. mL)

x = (6.0 M)(10. mL) 30. mL

x = 2.0 M

Note: 3x as much needed 1/3 the concentration

In the equation MAVA = MBVB,

MA means moles of H+/liter

1 M HCl yields (gives) 1 mole of H+/liter

2 M HCl yields 2 moles of H+/liter

Note: Diprotic acids yield twice as many H+/liter

1 M H2SO4 yields 2 moles of H+/liter

2 M H2SO4 yields 4 moles of H+/liter

And: MB means moles of OH-/liter

1 M NaOH yields 1 mole of OH-/liter

2 M NaOH yields 2 moles of OH-/liter

Note: Dihydroxy bases yield twice as many OH-/liter

1 M Ca(OH)2 yields 2 moles of OH- /liter

2 M Ca(OH)2 yields 4 moles of OH- /liter

Ex. What is the concentration of a sulfuric acid solution if 50. mL of 0.40 M KOH are needed to neutralize 20. mL of the H2SO4 solution of unknown concentration?

MAVA = MBVB

x (20. mL) = (0.40 M)(50. mL) x = (0.40 M)(50. mL)

20. mL

x = 1.0 M

But H2SO4 is diprotic. Each molecule produces 2 H+ ions.So the concentration only needs to be half as much:

true x = 1.0 M/2 = 0.50 M

Experi-mental design:

2. A volume of known molarity is added to a burette and its initial volume is recorded.

1. A known volume of unknown molarity is measured and added to the flask. Then an indicator is added.

3. The burette solution is titrated into the flask solution until the indicator changes color

4. The volume of burette solution used is found by subtracting initial and final burette volumes

Ex. 75 mL of KOH of unknown concentration are added to a flask and some indicator is added. The burette contains 2.5 M HCl. Its initial volume readingis 19 mL. The acid is slowly added until the indicatorchanges color. The final burette volume is 61 mL.

Find the concentration (molarity) of the KOH.

MAVA = MBVB

(2.5 M)(61 - 19 mL) = x (75 mL)

(2.5 M)(42 mL) = x 75 mL

1.4 M = x