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ACIDS
BASES
POTPOURRI
pH
TITRATIONS
100
Lewis defined an acid as anything that _____.
accepts an electron pair
100
_____ stated that bases are compounds that ionize to yield hydroxide ions in aqueous solutions.
Arrhenius
100
_____ is defined as the species that remains after an acid has donated a proton.
conjugate base
100
pH + pOH = ?
14
100
Compounds that change in different pH environments are called _____.
Indicators
200
Acids can be easily recognized because they have the element _____ as the first element in their chemical formula.
H
200
According to _____, a base is an electron pair donor.
Lewis
200
Metal oxides are referrred to as ______ anhydrides.
basic or base
200
What is the [H3O+] in a solution with a pH equal to 9.37?
[H3O+] = 4.27 x 10^-10
200
In the titration process, the point at which neutralization occurs is called the _____ point.
equivalence
300
_____ defined an acid as anything that donates a proton.
Bronsted-Lowry
300
In the reaction NH3 + H2O --> NH4+ + OH- _____ is behaving a as a base.
NH3
300
True or False When titrating, [H3O+] = [OH-] at the neutralization point.
FALSE moles H3O+ = moles OH- at the neutralization point
300
Calculate the pH of a solution having a hydronium ion concentration equal to 2.36 x 10^-4.
pH = 3.63
300
When titrating, the solution of known concentration is called the _____.
Standard
400
Any substance that can behave as an acid or a base is said to be _____.
Amphoteric
400
What is an amphoteric substance?
A substance that can behave as an acid or a base.
400
The following reation is an example of a _____ reaction. HCl + NaOH --> NaCl + H2O
neutralization
400
What is the hydronium ion concentration in a solution with a hydroxide ion concentration equal to 5.39 x 10^-8?
[H3O+] = 1.85 x 10^-7
400
How many milliliters of a .0947M NaOH solution will neutralize 21.4 ml of .106M HCl?
24.0 ml NaOH
500
Consider the following reaction: NH3 + H2O --> NH4+ + OH- What is the conjugate acid?
NH4+
500
Consider the fact that Al(OH)3 is a strong base. What is the molarity of hydroxide ions in a 2.81M solution of Al(OH)3?
[OH-] = 8.43
500
How many moles of H3PO4 (a strong acid) are required to neutralize .2890 moles of Ba(OH)2 (a strong base)?
.1927 moles
500
Calculate the [H3O+] in a solution with a pOH equal to 2.57.
[H3O+] = 3.72 x 10^-12
500
A 25 ml solution of H2SO4 is neutralized by 18 ml of 1.0M NaOH. What is the molarity of the H2SO4 solution?
[H2SO4] = .36