1. Equilibrium in Acids and Bases
Main Concept:
Chemical equilibrium reasoning can be used to describe the proton-transfer reactions of acid-base chemistry.

2. Equilibrium in Acids and Bases
pH vs [H+]
Strong Acids and Bases
Examples
Properties
Weak Acids and Bases
Properties
Acid-Base Reactions
Titration Curves

3. - concentrations of hydronium ion (H3O+) and hydroxide ion (OH-) are often reported as pH and pOH, respectively.
H2O(l) + H2O(l) ↔ H3O+(aq) + OH-(aq)
- Water autoionizes with an equilibrium constant, Kw. For pure water, pH=pOH, and this condition is called “neutrality,” or a neutral solution

4. H2O(l) + H2O(l) ↔ H3O+(aq) + OH-(aq)
- At 25°C, pKw=14  pH + pOH add up to 14. In pure water at 25°C, pH=pOH=7.

5. Strong versus Weak Acids POGIL

6. - Common strong acids include HCl, HBr, HI, HClO4, H2SO4, and HNO3
- molecules of strong acids completely ionize in solution to produce hydronium ions; 100% of molecules of strong acid are ionized in a solution (assuming concentration is not extremely high)
- As such, concentration of H3O+ in strong acid solutions are equal to initial concentration of strong acid  pH of strong acid solution is easily calculated

7. - Common bases include group I and II hydroxides; when dissolved in solution, strong bases completely dissociate to produce hydroxide ions
- Some group II hydroxides are slightly soluble in water. However, 100 percent of the dissolved base is ionized

9. - Weak acid molecules react with water to transfer a proton to the water molecule, however, weak acid molecules only partially ionize - only a small percentage of molecules of a weak acid are ionized in a solution (assuming initial concentration is not extremely low)  concentration of H3O+ does not equal the initial concentration of the molecule acid, and most acid molecules remain un-ionized

10. -A solution of a weak acid involves equilibrium between an un-ionized acid and its conjugate base
-The equilibrium constant for this reaction is Ka, often reported as pKa. The pH of a weak acid solution can be determined from the initial acid concentration and the pKa
-Common weak acids include carboxylic acids
- relative magnitudes of Ka’s are influenced by structural factors such as bond strength, solvation, and electronegativity of atom bonded to labile proton
HA + H2O(l) ↔ H+ + A-

11. - Common weak bases include ammonia, amines and pyridines, other nitrogenous bases, and conjugate bases
- Weak base molecules in aqueous solutions react with water molecules to produce hydroxide ions, however, only a small percentage of molecules of a weak base in solution ionize (assuming initial concentration is not extremely low)

12. -concentration of OH- in weak base solutions do not equal initial concentration of molecular base, and most base molecules remain un-ionized
-weak base solution thus involve an equilibrium between an un-ionized base and its conjugate acid
-The equilibrium constant for this reaction is Kb, often reported as pKb
-pH of a weak base solution can be determined from initial base concentration and pKb
B + H2O(l) ↔ HB+ + OH-

13. - When an acid molecule loses its proton, it becomes a base, since resultant ion could react with water as a base -The acid and base are referred to as a conjugate acid-base pair
- ionization constants for acid-base pair are related to Kw, and at 25°C, pKa + pKb = 14  relationship can be used to determine relative strengths of conjugate acids and bases
-For example, conjugate base of a strong acid is a much weaker base than H2O, and therefore does not react as a base in aqueous solutions

14. - pH of an acid solution depends on both strength and concentration of acid
-comparing solutions of a weak acid and of a strong acid at same pH, both solutions have same concentration of H3O+ (aq)
-strong acid completely dissociates into ions, but weak acid only partially dissociates into ions
- many more un-ionized acid molecules in weak acid solution than in strong acid solution at same pH

15. -to achieve solutions of equal pH, weak acid solution must be a much greater concentration than strong acid solution
-comparing solutions of a weak acid and of a strong acid of same initial concentration, concentration of H3O+ in strong acid solution is much larger (and thus pH lower) since strong acid is 100 percent ionized

17. - Reactions of acids and bases are called neutralization reactions
 generally have K>1, considered to go to completion
- For a mixture of a strong acid with a strong base, neutralization reaction is H3O+ + OH- → H2O
- K for this reaction is 1014 at 25°C, so reaction goes to completion
-This allows pH of mixtures of strong acids and bases to be determined from limiting reactant, either the acid or the base

18. conjugate acid + OH- → conjugate base + H2O
- When strong base is added to weak acid, a neutralization reaction occurs:
conjugate acid + OH- → conjugate base + H2O
- When strong acid is added weak base, a neutralization reaction occurs:
conjugate base + H3O+ → conjugate acid +H2O

19. - For weak acids and strong acids with same pH  takes much more base to neutralize weak acid because initial acid concentration is much larger
- weak acid solutions contain large amounts of un-ionized acid molecules  weak acid solutions resists changes in pH for a much greater amount of added base

20. - titration technique for neutralization
reactions  using known solution to
determine concentration of unknown
solution
- At equivalence point, moles of titrant
and moles of titrate are present in
stoichiometric proportions
- near equivalence point, pH rapidly changes  can be used to determine concentration of titrant
- As base is added to either strong acids or weak acids solution, H3O+ (aq) concentration does not change much
- change in pH is less than ~1.5 for the region where 10 to 90 percent of the base needed to reach the equivalence point has been added.

21. - pKa of acid can determined from pH at half equivalence point of titration if equivalence point is known (ie. the concentration of both the titrant and analyte are known)
- For polyprotic acids, titration curves can be used to evaluate number of labile protons, as well as knowing which species are present in large concentrations at any region along the curve

22. - Halfway to equivalence point, contents of a solution formed by titrating a weak acid, is different from one formed by titrating a strong acid
- For a strong acid, main species in a solution halfway to equivalence point are H3O+ (aq), anion from the acid (eg. Cl-, NO3-), and cation from the base (eg. Na+); total positive charge = total negative charge
- For a weak acid, main species in a solution halfway to equivalence point are H3O+ (aq), anion from the acid (eg. CH3COO-, F-), cation from the base (eg. Na+), and undissociated acid, HA. The total positive charge is equal to the total negative charge, and [HA] = [A-]

24. strong base (titrant) added into weak acid (analyte/titrand)
equivalence point > 7
weak base (titrant) added into strong acid (analyte/titrand)
equivalence point < 7

25. strong base (titrant) added into strong acid (analyte/titrand)
equivalence point = 7
weak acid (titrant) added into weak base (analyte/titrand)
NOT COMMON!!!
equivalence point = 7

26. acids (titrant) added into bases (titrate)