Acid/Base Theory
Donates H+ in solution
What is an (Bronsted-Lowry) acid?
These fully dissociate to produce hydroxide (OH-) ions.
What is a strong base?
The solution delivered from a buret.
What is the titrant?
The Henderson-Hasselbalch equation states that these two species are equal to one another at the half-equivalence point.
What are the acid and its conjugate base
(or base & conj. acid)
pOH of 0.010 M HNO3.
What is 12?
Accepts a H+ in solution
What is a (Bronsted-Lowry) base?
A reasonable pH range for a 1.0 M weak acid.
What is 3-4?
The solution placed under a buret that usually has an unknown concentration.
What is the analyte?
A buffer can be made with equal concentrations of NH3 and a salt containing
What is NH4+?
The [H3O+] if [OH-] is 3.5 x 10-4. (w/correct sig figs)
What is 2.9 x 10-11?
(use Kw = [H3O+][OH-]
The pH for a neutral solution.
What is 7?
Only partially dissolve, producing a low [H+].
What is a weak acid?
Point on a titration curve where moles of acid = moles of base
What is the equivalence point?
What is CO2, HCO3- and H2CO3?
The pH of a mixture that contains 10 mL of 0.1 M HCl and 10 mL of 0.02 M NaOH.
What is 1.4?
(calculate M of excess HCl; use -log [H+]
The sum of pH and pOH
What is 14?
NH3: Type of compound and strength
What is a weak base?
Approximate pH range of the equivalence point when a weak acid is titrated with a strong base.
What is 8-9?
This is increased to increase a buffer's capacity.
What is molarity (or concentration)?
The molarity of 20 mL of NaOH that was titrated with 16 mL of 0.5 M HCl.
What is 0.4 M?
The pH for a solution with a [OH-] of 1.0 x 10-4.
What is 10?
(pOH = 4; 14-4 = 10)
pH for 1.0 x 10-2 M HCl
What is 2?
Point on a titration curve where the pH = pKa
What is the half-equivalence point?
What is the pKa of a buffer that contains 1L each of HC2H3O2 and NaC2H3O2 of equal molarities with a pH of 4.3?
The pH of 10 mL of 0.1 M HCl after an additional 990 mL of water has been added.
What is 3?