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Unit 8 Review
Acids & Bases
In addition to this packet, be sure to review:!
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1. Text sections 14.1-14.3, 15.1, 15.2
2. All notes
3. pH Calculations packet (white)
4. Acid-Base packet (blue)
5. Weak Acid Calculations packet (buff)
Terms you should know:
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binary acid! !
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monoprotic acid
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oxyacid !
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polyprotic acid
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Arrhenius acid !
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Lewis acid
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Arrhenius base !
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Lewis base
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strong acid ! !
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conjugate acid-base pair
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weak acid!
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amphoteric
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Brønsted-Lowry acid!
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neutralization
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Brønsted-Lowry base!
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ligand
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1. Use section 14.1 of your textbook to list five properties associated with acids and with bases.
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Acids:!
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Bases:!
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2. Write balanced chemical equations for the following:
a. Hydrobromic acid + aluminum metal
b. Carbon dioxide + water
c. Acetic acid + calcium hydroxide
d. Chloric acid + sodium bicarbonate
3. Write a net ionic equation that explains each of the following observations, circle the type(s) of acid or base being
illustrated, then write the formula of the acid or base next to what was circled.
a. When aluminum chloride is dissolved in water, the complex ion Al[H2O]63+ forms.
! Arrhenius Acid!
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Bronsted-Lowry Acid!
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Lewis Acid!
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! Arrhenius Base!
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Bronsted-Lowry Base! !
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Lewis Base!
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b. When sodium cyanide is dissolved in water, the solution becomes basic.
! Arrhenius Acid!
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Bronsted-Lowry Acid!
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Lewis Acid!
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! Arrhenius Base!
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Bronsted-Lowry Base! !
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Lewis Base!
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c. When ammonia is dissolved in water, the solution becomes !
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! Arrhenius Acid!
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Bronsted-Lowry Acid!
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Lewis Acid!
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! Arrhenius Base!
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Bronsted-Lowry Base! !
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Lewis Base!
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d. When ammonium chloride dissolves in water, the solution becomes !
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Arrhenius Acid!
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Bronsted-Lowry Acid!
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Lewis Acid!
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! Arrhenius Base!
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Bronsted-Lowry Base! !
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Lewis Base!
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e. When NaOH is added to HClO3 acid and the equivalence point reached , the solution becomes !
! Arrhenius Acid!
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Arrhenius Base!
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Bronsted-Lowry Acid!
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Bronsted-Lowry Base! !
Lewis Acid!
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Lewis Base!
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4.) Label and connect the conjugate acid-base pairs in the following reaction:
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SO42- !
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H2O! !
HSO4-!
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+ !
OH-
5.) With the help of the acid ionization constant table, correctly place the following compounds in
order from strongest acid to strongest base:
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HNO2 !!
Ba(OH)2 !
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Strong Acid!
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NaNO3!
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KC3H5O3!
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HClO4!!
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Strong Base
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Which of the following compounds would have little effect on the pH of a solution?
(Circle one or more...)
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HClO2
KClO4 !
NH4Br !
N a N O 2!
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H C N! !
Na2SO4
7.) In a titration, 33.21 mL of 0.3020 M rubidium hydroxide solution is required to exactly neutralize
20.00 mL hydrofluoric acid solution. What is the molarity of the hydrofluoric acid solution?
8.) A 35.00 mL-sample of NaOH solution is titrated to its equivalence point by 14.76 mL of 0.4122 M
HBr solution. What is the molarity of the NaOH solution?.
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9.) a. Label each of the following acid-base titration curves as
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! 1) strong acid - strong base!
3) weak acid-strong base
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! 2) strong acid-weak base!!
4) weak acid-weak base
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b. Draw an arrow indicating the equivalence point for each curve.
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c. Phenolphthalein changes color (clear to pink) at pH 8.2. Circle the titration curve(s) that could
use phenolphthalein as an indicator to determine the equivalence point.
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d. What is the term used to mean the point in a titration when the indicator changes color?
10. Calculate the pH of the following solutions.
a. [H+] = 2.5 x 10-5 !
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b. [OH-] = 2.5 x 10-5!
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b. pOH = 1.250
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11. Calculate the [H+] of the following solutions.
a. pH = 8.500 ! !
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12. A 500.0 mL solution contains 15.0 grams of HCl (a strong acid). What is the pH of this solution?
13. A student requires 1.50 liters of 1.25 M HClO4 (a strong acid). How many grams of HClO4 will
needed?
14.) When the equivalence point is reached during the titration of a strong acid and a strong base, the
solution has a pH = 7. However, when the equivalence point is reached during the titration of a weak
acid and a strong base, the solution has a pH > 7. Offer an explanation for these results by filling in
the missing words:
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During a strong acid - strong base titration, at the equivalence point only ! !
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are !present. However, in a weak acid - strong base titration, at the equivalence point the acidʼs
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is present, which makes the solution basic.
15.) Weak acid calculations. Show all steps and use the 5% rule to verify approximations.
a. Calculate the pH of a 0.400 M solution of benzoic acid.
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b.) Calculate the pH of a 1.50 M solution of iodic acid.
c.) Calculate the concentration of acetic acid needed to produce a solution with a pH = 2.80.
d.) A 0.060 M solution of an unknown acid was determined to have a pH of 5.25. Calculate the acid
dissociation constant for this solution.
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