acids/bases lesson 14 buffers. buffer solutions buffer solutions are equilibrium systems, which...
TRANSCRIPT
Acids/BasesLesson 14
Buffers
Buffer Solutions
Buffer solutions are equilibrium systems, which maintain a relatively constant pH when small amounts of acids or bases are added.
How can you prepare a buffer?
You need a high concentration of weak acid or a weak base, and add to it its conjugate acid or its conjugate base also in high concentrations. This combination is known as a BUFFER.
Buffer Solutions
Acid Buffer Recipe
Weak Acid + Salt (conjugate base) HF NaF
*Na+ is a spectator
Buffer Equation Same as weak acid
HF ⇋ H+ + F-
HF ⇋ H+ + F-
[High] [low] [High]
[HF] is high and [H+] is low because HF is a weak acid.
[F-] is high due to adding the salt NaF.
This buffer solution can shift left or right and the [H+] and the pH remains fairly constant.
Note on buffersA solution of CH3COOH by itself cannot act as a buffer because the concentration of CH3COO- would be too small and will not satisfy the conditions of a buffer system.
A buffer requires large amounts of both the acid and its conjugate.
This is why we mix the weak acid or base with its conjugate salt.
Acidic buffer Mix 1.0 mol of acetic acid (CH3COOH ) and 1.0 mol of sodium acetate (NaCH3COO) and dilute to 1.0 L of solution
Base Buffer Recipe
Weak Base + Salt (conjugate acid)
NH3 NH4Cl *Cl- spectator
Buffer Equation Same as weak base
NH3 + H2O ⇋ NH4+ + OH-
[High] [High] [Low]
Fill in the blanks to get buffer solutions.Acid conjugate Base from a salt
HCN NaCN
H2CO3 NaHCO3
H3PO4 NaH2PO4
CH3COOH KCH3COO
NaHCO3Na2CO3
NaH2PO4Na2HPO4
How buffers work…
The ‘buffering effect’ works due to the fact that the value of the ratio:[conjugate acid] remains fairly constant.
[conjugate base]
* This ratio does not change much when a small amount of either an acid or a base is added to the buffer system. Why ???
The conjugate acid present can react with the added OH to neutralize it, and the conjugate base present can react with the added H3O to neutralize it.
Buffer Animation 1
Buffer Application
1. Pick the two buffer solutions
A. NH4Cl and HCl
B. NaCl and NaOH
C. HCN and NaCN
D. NH4Cl and NH3
2. Write the equations for the above two buffer solutions. Label the concentrations as high or low.
3. A few drops of 0.10 M NaOH is added to a buffer solution at pH = 5.00. The new pH could be:
A 4.98
B. 5.02
C. 8.05
D. 2.11
Buffers in biological systems
HomeworkRead page 182 and 183 for “Buffers in biological systems”, must know these systems and how they work.
Page 181: #132,133,138,139
Page 183: #143 on buffers…interesting story/question.