1. Chapter 14 Acids and Bases
14.8 Acid−Base Titration
Learning Goal Calculate the molarity or volume of an acid or a base from titration information.
© 2014 Pearson Education, Inc.

2. is a laboratory procedure used to determine the molarity of an acid
Acid−Base Titration
Titration
is a laboratory procedure used to determine the molarity of an acid
uses a base such as NaOH in the buret to neutralize an acid
A measured amount of acid is placed in
a flask with an indicator.
© 2014 Pearson Education, Inc.

3. is added to the acid in the flask
Acid−Base Titration
An indicator
is added to the acid in the flask
changes the color of the solution when the acid is neutralized
The acid solution briefly turns pink when the base is added. The pink quickly disappears once the solution is mixed.
© 2014 Pearson Education, Inc.

4. the indicator has a permanent pink color
Acid−Base Titration
At the endpoint,
the indicator has a permanent pink color
the volume of the base used is measured
the molarity of the acid is calculated using the neutralization equation for the reaction
The acid solution turns a permanent pink when the endpoint is reached.
© 2014 Pearson Education, Inc.

5. Guide to Calculations for Acid−Base Titrations
© 2014 Pearson Education, Inc.

6. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Learning Check
What is the molarity of 10.0 mL of HCl solution if 18.5 mL of M NaOH are required to neutralize the HCl?
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
© 2014 Pearson Education, Inc.

7. Step 1 State the given and needed quantities and concentrations.
Solution
What is the molarity of 10.0 mL of HCl solution if 18.5 mL of M NaOH are required to neutralize the HCl?
Step 1 State the given and needed quantities and concentrations.
Given
Need
10.0 mL (0.010 L) of HCl solution
Molarity of HCl solution
18.5 mL ( L) of M NaOH solution
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
© 2014 Pearson Education, Inc.

8. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Solution
What is the molarity of 10.0 mL of HCl solution if 18.5 mL of M NaOH are required to neutralize the HCl?
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Step 2 Write a plan to calculate molarity or volume. L of
NaOH
Molarity
moles of
NaOH
Mole-Mole factor
moles of
HCl
Divide by liters
molarity of
HCl
© 2014 Pearson Education, Inc.

9. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Solution
What is the molarity of 10.0 mL of HCl solution if 18.5 mL of M NaOH are required to neutralize the HCl?
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
Step 3 State equalities and conversion factors, including concentrations.
© 2014 Pearson Education, Inc.

10. Solution
What is the molarity of 10.0 mL of HCl solution if 18.5 mL of M NaOH are required to neutralize the HCl? HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l) Step 4 Set up the problem to calculate the needed quantity.
© 2014 Pearson Education, Inc.

11. Learning Check
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
© 2014 Pearson Education, Inc.

12. Solution
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH. Step 1 State the given and needed quantities and concentrations.
Given
Need
2.00 M HCl solution
Volume of HCl solution
L of 1.00 M KOH solution
H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
© 2014 Pearson Education, Inc.

13. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Solution
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH.
H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Step 2 Write a plan to calculate molarity or volume. L of
KOH
Molarity
Mole-Mole factor
moles of
KOH
moles of
H2SO4
Molarity
volume of
H2SO4
© 2014 Pearson Education, Inc.

14. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Solution
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH.
H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Step 3 State equalities and conversion factors, including concentrations.
© 2014 Pearson Education, Inc.

15. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Solution
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH.
H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Step 3 State equalities and conversion factors, including concentrations.
© 2014 Pearson Education, Inc.

16. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Solution
Calculate the milliliters of 2.00 M H2SO4 needed to completely neutralize L of 1.00 M KOH.
H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
Step 4 Set up the problem to calculate the needed quantity.
© 2014 Pearson Education, Inc.