2011 MYP Chemistry Final Practice Questions Part 2
ANSWERS
THIS WAS DONE QUICKLY SO IF YOU ARE SURE YOU ARE CORRECT I
MAY HAVE MADE AN ERROR, CHECK WITH ME TOMORROW
These will help you to prepare for the types of questions on the Final Exam related to Solutions, Solubility, Acids and Bases.
PART V – Name the following
1.
Name the following:
2.
Write the formula for the following:
a. H2CO3(aq) = carbonic acid
a. Nitrous acid
= HNO2
b. HFO4(aq)
b. Sulfuric acid
= H2SO4
= perfluoric acid
c. H3PO3(aq) = phosphorous acid
c. Hypobromous acid = HBrO2
d. HF(aq)
= hydrofluoric acid
d. Fluoric acid
e. HClO(aq)
= perchloric acid
e. Hydrosulfuric acid = H2S
= HFO3
PART VI - Acid Reactions:
1.
Complete the general equation for each of the following:
a.
Acid + Base  Water + Salt
c.
Acid + Metal  H2 + Salt
where salt is just the same as an ionic compound
b.
Acid + Carbonate  CO2 + Water + Salt
2.
For the following acid reactions:
*Identify the reaction type
*Complete the equation and balance it.
a.
________H2SO4___________ + __________Li2O____________  H2O + Li2SO4
TYPE:________________Acid + Base Neutralization...also a double replacement reaction__________
b.
___________2HCl___________ + K2CO3  ________CO2__________ + 2KCl + ________H2O_________
TYPE:_____________Acid +Carbonate Reaction…also a double repleacement followed by a decomposition reaction
c.
Ca
+
2HNO3 __________Ca(NO3)2____________ + _________H2_____________
TYPE:_________________Acid + Metal…also a single replacement reaction___________
3.
For the above reactions, write the formula and name of the salt produced:
Formula
Name
a. ______Li2SO4_______ ____Lithium Sulfate_______
b. ______KCl__________ ____Potassium Chloride________
c. ______Ca(NO3)2_____ ____Calcium Nitrate________
E.
Draw the pH scale including the following:
1.) Label acidic/neutral/basic
2.) [H3O+] and [OH-] at neutral pH
3.) Explain how the ion concentrations fluctuate as pH increases and decreases
SEE THE BACK OF PAGE 2 OF YOUR Acids work packet for a chart that would work
A.
Complete the lettered areas of the table in the blanks provided:
1_________1 x
10-14__________
or [H+]
2_________ [ OH-] ______________
[H3O+]
1
2 [ OH]-
3_________-log [OH-]__________
4__________pOH = -log [OH-]___________
5__________pH + POH = 14___________
7
3
6__________pH _________
7__________[H3O+]
5
= 10-pH____________
6 pH
4 pOH
B.
1.
Complete each of the following:
[H3O+][OH-] = ___1 x 10-14_______
2.
pH + pOH = ___14_________
3.
pOH mathematically represents:__the power of the concentration of hydroxide ions___
5.
Explain how you would find pOH given pH: pOH = 14 – pH
6.
Show how you would determine the [H3O+] if you are given [OH-]: [H3O+] = (1 x
7.
Describe how you would find the pOH if you are given [OH-]: pOH = -log [OH-]
8.
Describe how you would determine [H3O+] if you are given pH:
9.
Explain how you would find the [OH-] if you are given pH: first pOH = -log [OH-], then pH = 14 - pOH
10-14) / [OH-]
[H3O+] = 10 –pH or [H+] = 10 -pH
PART VI – Perform the following calculations. If your answer is incorrect and you do not show your work,
you will not receive any credit for the problem.
A.
Calculate the pH of the following solutions and identify each solution as acidic or basic:
1. pOH = 9.27
2. [H3O+] = 2.35 X 10-4 M
3. [OH-] = 5.75 X 10-3 M
pH = 4.7 acid
B.
pH =3.7 acid
pH =11.8 base
Calculate the pOH of the following and classify each as acidic or basic:
1. 3.7 X 10-2 M KOH
2. [H3O+] = 5.45 X 10-6 M
3. 0.32 M HNO3
pOH = 1.4 base
pOH = 8.7 acid
pOH = 13.5 acid
C.
Determine the concentration of the indicated ion in each of the following:
1.
[OH-] for a solution of pH 8.2
= 1.6 x 10-6 M
2.
[H3O+] for a solution with a pOH of 4.8
= 6.3 x 10-10 M
3.
[H3O+] for 5.14 X 10-3 M KOH
= 1.9 x 10-12 M
4.
[H3O+] for a solution in which [OH-] = 6.3 X 10-3 M
= 1.6 x 10-12 M
D.
Calculate the pH of the following and classify as acidic or basic:
1.
0.02 M HNO3
pH = 1.7
2.
3.5 X 10-6 M KOH
3.
0.06 M HBr
pH = 1.2
E.
Complete the following table:
SUBSTANCE
pOH
Lemons
11.7
F.
1.
pH = 8.5
pH
[OH-]
-12
[H3O+]
Acid/Base/Neutral
2.3
2.0 x 10 M
.005M
acid
1.58 X10-11 M
base
Soap
3.2
10.8
6.3 x 10-4M
Milk
7.3
6.7
5 X10-8 M
Strawberries
10.5
3.5
3.2 x 10-11M
Sea Water
5.7
8.3
Slightly acidic
3.2 x 10-4M
acid
base
Titrations - Write balanced equations and show your work either by doing stoichiometry and Molarity equations or by
using MaVa = MbVb
How many mL of 0.5 M KOH would be required to neutralize 175 mL of 0.6 M nitric acid?
Vb = .21L or 210 mL
Calculate the pH of the original solutions: KOH = ____pH = 13.7_______
2.
Nitric acid = ____pH = 0.22 ______
If 50 mL of a 1.75 M hydrochloric acid solution are neutralized by 35.4 mL of NaOH, what is the molarity of the NaOH?
Mb = 2.47M NaOH
3.
If the concentration of a Ca(OH) 2 solution is 0.75 M, calculate how many mL would be required to neutralize 50 mL of
sulfuric acid with a pH of 2.2.
This type of titration WILL NOT BE ON THE TEST since it has a diprotic acid and a double
hydroxide base in Ca(OH)2
Ca(OH)2 + H2SO4  2H2O + CaSO4
if pH is 2.2 then [H+] = 10-pH so [H+] = .0063M, so [H2SO4] must be ½ as much since it is
diprotic so [H2SO4] = 0.00315M
Vb = 0.21L or 210mL