EQUALIBRIUM - Acid-Base Equilibria
16 important questions on EQUALIBRIUM - Acid-Base Equilibria
What are Bronsted-Lowry Acids and Bases?
- BLAcids are proton donors (give)
- BLBases are proton acceptors (taking)
What are Lewis Acids and Bases?
- Lewis acids are electron acceptors
- Lewis base are electron donors
What are 5 strongest acids?
- HCl
- HBr
- HI
- HClO4
- HNO3
- H2SO4
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What are the Strong bases?
- LiOH
- NaOH
- KOH
- RbOH
- CsOH
- Mg(OH)2
- Ca(OH)2
- Sr(OH)2
- Ba(OH)2
What kind of equilibrium constants do strong bases and acids have?
What kind of equilibrium constants do weak acids and bases have?
- They typically have small or intermediate K values because they do not dissociate completely
How do you determine the degree of dissociation of weak acids and bases?
- Ka for Acids
- Kb for Bases
How to determine if a salt dissolved in water will behave as an acid or a base in solution?
- Case 1 (salts that lead to neutral solutions)
- both ions are conjugate to a strong acid or a strong base
- neutral pH
- EX: LiCl, NaCl, KNO3
- Case 2
- one is conjugate of a strong acid or strong acid and the other is a weak acid or base
- ***ONLY WEAK SPECIES IS ACTIVE AND WILL DETERMINE PH***
- EX: NaNO2, KF
- Case 3
- If the cation is a weak acid and the anion is a weak base
- pH is determined by the largest equilibrium constant (Ka or Kb)
Which of these have the weaker acid?
- Ka = 1.77*10^-4
- Ka = 6.21*10^-10
.'. The lower the Ka value = weaker the acid
.'. The higher the Ka value = the stronger the acid
Which one has the weaker pKa value?
- pKa = 3.70
- pKa = 9.15
.'. Lower = acidic
.'. Higher = basic
What is the relationship of Kb, Ka, and Kw?
Kw = 1*10^-14
Which of these polyprotic acids are weaker?
- H2CO3(aq) + H2O(l) ⇋ HCO3 - (aq) + H3O+ (aq)
- Ka,1 = 4.4*10^-7
- HCO3 - (aq) + H2O(l) ⇋ CO3 2- (aq) + H3O+ (aq)
- Ka,2 = 4.7*10^-11
- Ka,1 = 4.4*10^-7
- Ka,2 = 4.7*10^-11
ANS: #2 is the weaker acid because the more you break it down and dissociate the weaker it becomes
What is the leveling effect?
- the inability to tell the differences in strength among strong acids in water
- In solvents less basic than water, the strength of the strong acids are hard to tell!
T/F Do all strong acids exhibit the same strength in water? If so, why?
- Because of the leveling effect, water is a strong base compared to other conjugate bases.
In the chemistry table, which area would be increasing acid strength?
A 0.00250 M solution of a weak base n-propylamine CH3CH2CH2NH2 (C3H7NH2) has a pH of 10.89. What is the Kb for n-propylamine?
- List relevant reactions and compare K values
- Make ICE table
- Determine pH
- Solve for Kb
ANS: 3.5*10^-4
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