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Worksheets11.1 - 11.2 Acids Bases
Total questions: 30
Worksheet time: 45mins
What is a binary acid?
H+ plus (a) more element(s).
How is a binary acid named?
(b) the (c) prefix and change the ending to (d)
What is an oxyacid?
H+ plus a (a) .
How is an oxyacid named?
(b) the hydro- prefix and the ending changes:
from -ate to (c)
or
from (d) to (e)
Name the following binary acids:
HCl (a)
HBr (b)
HF (c)
Name the following oxyacids acids:
hydro + polyatomic + ic or ous + acid
HClO (a)
HClO2 (b)
HClO3 (c)
HClO4 (d)
Name the following acids:
H2S (a)
H2SO3 (b)
H2SO4 (c)
Name the following acids:
HBr (a)
HBrO (b)
HBrO3 (c)
What is the conjugate base of HCl?
Cl-
Cl
C
H2Cl
What is the conjugate base of H2SO4?
HSO4-
SO4
H3SO4
HSO
What is the conjugate base of H2O?
OH-
H3O+
HO
HO2
What is the conjugate acid of H2O?
OH-
H3O+
HO
HO2
What is the conjugate acid of NH3?
NH4+
NH4
NH2
N
What is the conjugate acid of HSO4-?
H2SO4
SO42-
HSO
H2SO4+
Organize these molecules into the right categories
HCl
NaOH
H2O
NaCl
Organize these molecules into the right categories
HNO3
KOH
HSO4-
NaNO3
Organize these molecules into the right categories
HI
NH3
H2PO4-
KNO3
Complete this reaction in this order:
acid + base → c. base + c. acid
HNO3 + OH- → (a) + (b)
Complete this reaction in this order:
base + acid → c. acid + c. base
NH3 + H3O+ → (a) + (b)
The equilibrium expression for water, Kw, is: Kw = [H3O+][OH-]
and Kw = 1.0 x 10-14
Rearrange the equation two times:
[H3O+] = (a) / (b)
[OH-] = (c) / (d)
A solution has a hydroxide, OH-, concentration of [OH-] = 1.5 x 10-4 . What is the [H3O+] concentration?
Show work:
1.0 x 10-14 / (a) = (b)
If the [H3O+] in a nitric acid solution is 0.0025 mol/L, what is the [OH-]?
4 x 10-12 M
4 x 10-13 M
2.5 x 1011 M
2.5 x 10-17 M
Write the dissociation reaction for lithium hydroxide
LiOH → Li+ + OH-
LiOH → Li- + OH+
Li2OH → 2 Li+ + OH-
Li(OH)2 → Li+ + 2 OH-
Write the dissociation reaction for potassium hydroxide
KOH → K+ + OH-
KOH → K- + OH+
K2OH → 2 K+ + OH-
K(OH)2 → K+ + 2 OH-
Ten grams of LiOH is dissolved in 0.75 L of water. Calculate the molarity of OH- in the solution.
LiOH → Li+ + OH-
0.56 M
0.42 M
23.9 g/mol
13.3 g/L
Ten grams of LiOH is dissolved in 0.75 L of water. To calculate the molarity of OH- in the solution, follow this:
10g LiOH / (23.9 g/mol) = 0.4176 mols
0.4176 mols / 0.75 L = 0.56 M OH-
Calculate the [H3O+] in the solution.
0.56 M
1.8 x 10-14
23.9 g/mol
5.6 x 1013
Write the dissociation reaction for Ca(OH)2
Ca(OH)2 --> Ca2+ + 2 OH-
Ca(OH)2 --> Ca2+ + OH-
Ca(OH)2 --> Ca + 2 OH
Ca(OH)2 --> 2 Ca+ + OH2-
Write the dissociation reaction for hydrobromic acid
HBr + H2O → Br- + H3O+
HBr + H2O → Br- + OH-
HBr + H2O → Br + H3O
HBr + H2O → H2Br+ + OH-
Write the dissociation reaction for sulfuric acid
H2SO4 + H2O → HSO4- + H3O+
HSO4 + H2O → SO4- + H3O+
H2S + H2O → HS- + H3O+
H2SO4 + H2O → HSO4- + OH-
Acids (a) H+ and bases (b) H+
Organize these chemicals into the right categories
HCl
HF
HNO3
NH3
KOH
Ba(OH)2
Organize these chemicals into the right categories
HBr
H2S
HClO4
Ca(OH)2
NH3
NaBr
KF
