acid-base titration and ph
DESCRIPTION
Acid-Base Titration and pH. Chapter 16. Self-Ionization of water. Two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton. Pure water. Concentrations of hydronium and hydroxide ions of 1.0 x 10 -7 mol/L at 25 °C. Expressing concentrations. - PowerPoint PPT PresentationTRANSCRIPT
Acid-Base Titration and pH
Chapter 16
chemistry chapter 16 2
Self-Ionization of water Two water molecules produce a
hydronium ion and a hydroxide ion by transfer of a proton
chemistry chapter 16 3
Pure water Concentrations of hydronium and
hydroxide ions of 1.0 x 10-7 mol/L at 25 °C.
chemistry chapter 16 4
Expressing concentrations Brackets indicate concentration in
mol/L [H3O+] means
Hydronium ion concentration in moles per liter
or Molar hydronium ion concentration
chemistry chapter 16 5
Ionization constant of water
1.0 x 10-14 M2 or (mol/L)2
Constant over ordinary room temperatures
For pure water or dilute aqueous solutions
OHOHKw 3
chemistry chapter 16 6
Solutions Neutral
[H3O+]=[OH-] Acidic
[H3O+]>[OH-] Basic
[H3O+]<[OH-]
chemistry chapter 16 7
Strong bases Ionize completely in solution Molar concentration of hydroxide
ions is the same as the molarity of the solution times the subscript of hydroxide.
Example: A 1.0 x 10-3 M LiOH solution has [OH-] of 1.0 x 10-3 M
Example: A 1.0 x 10-3 M Ca(OH)2 solution has [OH-] of 2.0 x 10-3 M
chemistry chapter 16 8
Strong Acids Ionize completely in solution Molar concentration of hydronium ions
is the same as the molarity of the solution times the subscript of hydrogen.
Example: A 1.0 x 10-4 M HCl solution has [H3O+] of 1.0 x 10-4 M
Example: A 1.0 x 10-4 M H2SO4 solution has [H3O+] of 2.0 x 10-4 M
chemistry chapter 16 9
Using Kw
If you know the concentration of hydronium or hydroxide ions, you can use Kw to find the concentration of the other ion.
See page 484
OHOHKw 3
chemistry chapter 16 10
pH The negative of the common
logarithm of the hydronium ion concentration
OHpH 3log
chemistry chapter 16 11
pOH The negative of the common
logarithm of the hydroxide ion concentration
OHpOH log
chemistry chapter 16 12
relationship0.14 pOHpH
chemistry chapter 16 13
chemistry chapter 16 14
Discuss What is the concentration of hydronium
and hydroxide ions in pure water at 25 °C?
For each of the following properties, is the solution acidic or basic? [H3O+] = 1.0 x 10-3 M [OH-] = 1.0 x 10-4 M pH = 5.0 pH = 8.0
chemistry chapter 16 15
Acid-Base indicators Used to obtain an approximate
value for pH. Compounds whose colors are
sensitive to pH. Weak acids or weak bases
chemistry chapter 16 16
Transition interval The pH range over which an
indicator changes color See page 495
chemistry chapter 16 17
Universal indicators Use a combination of several
different indicators. pH paper has been soaked in a
universal indicator.
chemistry chapter 16 18
pH meters Used to find the exact pH Measures the voltage between two
electrodes placed in solution. Changes with hydronium ion
concentration
chemistry chapter 16 19
Titration The controlled addition and
measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration.
chemistry chapter 16 20
Equivalence point When the two solutions used in a
titration are present in chemically equivalent amounts Not always neutral
chemistry chapter 16 21
End point The point in a titration at which an
indicator changes color. Can be used to find equivalence
point. If the indicator changes color at the
equivalence point
chemistry chapter 16 22
Strong acid titrated with strong base
chemistry chapter 16 23
Weak acid titrated with strong base
chemistry chapter 16 24
Discuss P. 503 section review 1 and 2.
chemistry chapter 16 25
Standard solution The “known” solution Its concentration is known
precisely
chemistry chapter 16 26
Primary standard Highly purified solid compound Used to check the concentration of
the known solution
chemistry chapter 16 27
Titration process See pages 500 - 501
chemistry chapter 16 28
Calculating the unknown concentration1. Write the balanced chemical
equation.2. Determine the moles of the
known solute.3. Determine the moles of the
unknown solute.4. Determine the molarity of the
unknown solution.
chemistry chapter 16 29
Example A 25.00 mL sample of a solution of
RbOH is neutralized by 19.22 mL of a 1.017 M solution of HBr. What is the molarity of the RbOH solution?
0.7820 M
chemistry chapter 16 30
You try If 29.96 mL of a solution of Ba(OH)2
requires 16.08 mL of a 2.303 M solution of HNO3 for complete titration, what is the molarity of the Ba(OH)2 solution?
0.6182 M
chemistry chapter 16 31
You try You have a 0.83 M vinegar
solution. You are going to titrate 20.00 mL of it with a 0.519 M NaOH solution. At what volume of added NaOH solution would you expect to see an end point?
37 mL