Proton Movement and Acid/Base Facts
What is the conjugate acid of HSO4-1?
What is...
H2SO4
Is the following acid monoprotic, diprotic, or triprotic?
H3PO4
What is...
triprotic
If the pH of a solution is 5, what is the pOH?
What is...
pOH = 9
Complete the following neutralization reaction (make sure to balance):
LiOH + HClO4 -->
(HClO4 is perchloric acid and completely dissociates)
What is...
LiOH + HClO4 --> LiClO4 + H2O
What is the name of the skinny piece of glassware that contained our titrant and helped us to perform the titration?
What is...
A buret
Which of the following is defined as being a proton donor?
Bronsted base, Arrhenius base, Bronsted acid, or Arrhenius acid?
What is...
A Bronsted acid
Which type of compound, acids or bases, dissociates into ions when in solution?
What is...
Both acids and bases dissociate into ions in solution.
A solution with a pOH of 10 is...
Acidic or Basic?
What is...
Acidic!
pOH of 10 means a pH of 4...anything with a pH of less than 7 is acidic.
What does it mean for a compound to be a binary acid?
What is...
The compound is an acid that contains only two types of elements.
What was the name of the acid and what was the name of the base that we used in our titrations lab?
What is...
hydrochloric acid and sodium hydroxide.
Complete the following reaction and label the compounds as acid, base, conjugate acid, and conjugate base:
HBr + H2O -->
What is...
HBr + H2O --> Br- + H3O+
A B CB CA
What are the 6 strong acids?
What are...
HCl, HBr, HI, HClO4, H2SO4, and HNO3
What is the pH of a solution with a [H3O+] concentration of 4.56 • 10-7?
What is...
pH = 6.34
What is the name of the following compound?
HNO2
What is...
Nitrous Acid
When phenolpthalein (the indicator that we used in the lab) is placed into an acidic solution, what color does the solution turn?
What is...
Clear
What is the difference between a strong acid and a weak acid?
What is...
A strong acid completely ionizes (100%) but a weak acid does NOT completely ionize.
What is the [OH-1] concentration in a 0.5M HCl solution?
What is...
[OH-1] = 2 • 10-14
What is special about the "equivalence" of a titration?
(What two quantities are equal at the equivalence point?)
What is...
When the moles of acid are equal to the moles of base.
What does it mean when a compound is considered amphoteric?
What is..
This compound can act as either a Bronsted Lowry acid or a Bronsted Lowry base
If 30 mL of 0.005 M HI is brought to the equivalence point while titrating with 20 mL of NaOH, what is the molarity of the base?
What is...
0.0075 M NaOH
Which of the following solutions has hydroxide ions present in solution? AND
Which of the following solutions has the largest hydroxide ion concentration?
pH = 4 0.005 HCl solution pOH = 2
What is...
They ALL have hydroxide ions in solution. Some will have just substantially more of those ions present than others. (Do the math to justify this answer if you need to).
pOH = 2 has the highest [OH-]
Complete the following reaction and label the compounds as acid, base, conjugate acid, and conjugate base:
HPO4-2 + H2O -->
(water is acting as a base)
What is...
HPO4-2 + H2O --> PO4-3 + H3O+
A B CB CA
What is the hydronium (H3O+) concentration of a 0.025M Ba(OH)2 solution? (write answer in scientific notation)
What is...
[H3O+] = 2 • 10-13 M
Complete the following double replacement neutralization reaction and balance the reaction. Then give the net ionic equation and make sure this is balanced as well.
H2SO4 + KOH -->
What is...
H2SO4 + 2 KOH --> K2SO4 + 2 H2O
Net: 2H+ + 2OH- --> 2 H2O
Which of the following solutions will conduct the strongest electrical current? (Think about which solution will produce the most ions).
0.5 M HCl solution 1 M HCl solution.
0.5 M HC2H3O2 solution 1 M HC2H3O2 solution
What is...
1M HCl solution.
Largest concentration of a strong acid. Remember. Strong acids completely dissociate and weak acids do NOT completely dissociate.