Acid/Base Definitions
According to the arrhenius definitions are the following acids or bases?
HBr
Ca(OH)2
KOH
H2S
Acid
Base
Base
Acid
What is the pH of a acidic solution, basic solution, and neutral solution?
Acid: <7
Basic: >7
Neutral: =7
Calculate [H+] and [OH-].
pH = 9.36
[H+]=4.37x10-10 M
[OH-]= 2.29x10-5 M
What are always the products of a neutralization reaction?
water and salt.
Write two fractions to represent the concentration of a 4.35 M solution of H3PO4.
(4.35 mol H_3PO_4)/(1L H_3PO_4)
(1L H_3PO_4)/(4.35 mol H_3PO_4)
Acids contain more ______ ions while bases contain more ______ ions.
hydrogen, hydroxide
Determine the pH and pOH of the following solution and determine if it is acidic or basic.
[H+] = 6.70 x 10-6 M
pH=5.17
pOH=8.83
acidic
Calculate [H+] and [OH-].
pH = 7.8
[H+]=1.6x10-8 M
[OH-]= 6.3x10-7 M
Write and balance the neutralization reaction between hydrochloric acid and sodium hydroxide.
HCl + NaOH --> H2O + NaCl
balanced
Write two fractions to represent the ratio of hydrogen ions to H3PO4 in a 4.35 M solution of H3PO4.
(3 mol H^+)/(1 mol H_3PO_4)
(1 mol H_3PO_4)/(3 mol H^+)
(CH3)3N + H2O → (CH3)3NH + OH-
B, A, CA, CB
Determine the pH and pOH of the following solution and determine if it is acidic or basic.
[OH-]= 7.25 x 10-5 M
pOH=4.14
pH=9.86
basic
Calculate [H+] and [OH-].
pOH = 3.91
[H+]=8.128x10-11 M
[OH-]= 1.23x10-4 M
Write and balance the neutralization reaction between nitric acid and aluminum hydroxide.
3 HNO3 + Al(OH)3 --> 3 H2O + Al(NO3)3
Write two fractions to represent the ratio of hydrogen ions and hydroxide ions at the equivalence point when mixing a 3.0M solution of H2SO4 and a 1.25M solution of KOH.
(1 mol H^+)/(1 mol OH^-)
(1 mol OH^-)/(1 mol H^+)
H2SO4 (aq) + H2PO4- (aq) → H3PO4 (aq) + HSO4- (aq)
A, B, CA, CB
Determine the pH and pOH of the following solution and determine if it is acidic or basic.
[H+] = 1.5 x 10-12 M
pH=12
pOH=2
basic
Calculate [H+] and [OH-].
pH = 3.5
[H+]=3.2x10-4 M
[OH-]= 3.16x10-11 M
Write and balance the neutralization reaction between sulfuric acid and magnesium hydroxide.
H2SO4 + Mg(OH)2 --> 2 H2O + MgSO4
What is the goal of a titration?
To find the concentration (or molarity or mol/L) of an unknown acid or base.
Explain the benefit of using the Arrhenius definitions of acids and bases. Then explain the benefit of using the Bronsted-Lowry definition.
Arrehenius definitions are easy (H for acid OH for base).
Bronsted Lowry definitions are broad (cover all acids and bases).
Determine the pH and pOH of the following solution and determine if it is acidic or basic.
[OH-]=4.31 x 10-11 M
pH = 3.6
acidic
Calculate [H+] and [OH-].
pOH = 10.53
[OH-]= 2.951x10-11M
[H+]= 3.39x10-4M
Write and balance the neutralization reaction between phosphoric acid and calcium hydroxide.
2 H3PO4 + 3 Ca(OH)2 --> 6 H2O + Ca3(PO4)2
What is the difference between an equivalence point and an end point.
Equivalence point of the point when [H+]=[OH-]. End point is the point when the indicator causes a color change in your solution.
Ideally, these points will be the same.
28.55 mL of 0.1200 M LiOH solution is required to neutralize 25.00 mL of a perchloric acid (HClO4) solution. What is the molarity of the HClO4 solution?
0.1370M