Chapter 18 Review Sheet Acids and Bases
1.
How do acids usually taste? sour
2.
Name five properties that aqueous acids share.
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3.
4.
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Electrolytes
Sour taste
React with indicators
* react with metals to form H2
* react with bases to neutralize
Give the formula or name for each of the following:
H2SO4 _Sulfuric acid
Nitric Acid _HNO3
H2S _Hydrosulfuric acid
Phosphoric Acid _H3PO4_
What are the five properties of a base?
Electrolytes
* react with acids to neutralize
Bitter taste
* slippery feel
React with indicators
What is the definition of an Arrhenius acid? Give an example of one.
Any compound that contains a hydrogen and ionizes into a hydrogen ion in waterHCl
5.
6. What is an Arrhenius base? Give an example of one?
Any compound that contains a hydroxide and dissociates into a hydroxide ion in
water
7. What makes an acid or base strong or weak? An acid or base is strong if it
ionizes 100% in water- weak acids and bases do not and you can use %
dissociation or KA or KB values to determine their relative strength ( larger
the KA or KB value the stronger it is)
8. List the three strong acids that you need to memorize. Hydrochloric
acid(HCl), Sulfuric acid (H2SO4) and Nitric acid (HNO3)
9. Explain a weak acid or base. Weak acids and bases have KA and KB values
are a % dissociation will accompany them because they do not completely
ionizes in water. If you have a strong acid it will produce a weak conjugate
base, thus if you have a weak acid it will produce a strong conjugate base;
the same holds true for strong and weak bases
10. What is the definition of a Bronsted-Lowry acid? Any compound that
donates a hydrogen
11. What is the definition of a Bronsted-Lowry base? Any compound that
accepts a hydrogen
12. What is the difference between a monoprotic and a polyprotic acid?
Monoprotic has one hydrogen, while polyprotic has more than one.
13. Label the conjugate acid-base pairs:
a) H3PO4(aq)
acid
b) CN- (aq)
base
c) HCN(aq)
acid
d) H2O(l) +
base
+ NO2-(aq) ---- HNO2(aq) + H2PO4-(aq)
base
c. acid
c. base
+ HCO3 (aq) -- HCN(aq) + CO32-(aq)
acid
c. acid
c. base
+ SO32-(aq)  HSO3-(aq) + CN-(aq)
base
c. acid
c. base
+
HF(aq)  F-(aq) + H3O (aq)
acid
c. base
c. acid
14. Explain why water is considered amphoteric. Water can act as either a
weak acid or a weak base
16. Base + Acid ---- Salt + Water
17. What occurs during a neutralization reaction? When a strong acid and a
strong base react then the solution of salt in water is neutral.
18. Complete and balance the following reactions, and label which resulting
solutions would be acidic, basic or neutral.
2HBr
+
Ba(OH)2 ------à 2H2O + BaBr2 Basic
2NaHCO3 +
H2SO4 ----à 2H2O + 2CO2 + Na2SO4 acidic
HCl + NaOH -----àH2O + NaCl Neutral
Hydrofluoric acid + potassium hydroxide --à water + potassium fluorideHF + KOH --à H2O + KF Basic
Magnesium + hydrochloric acid ---à Hydrogen gas + magnesium chloride
Mg + 2HCl --à H2 + MgCl2
Barium carbonate + nitric acid ---à carbon dioxide + water + barium
nitrate BaCO3 + 2HNO3 --à H2O + CO2 + Ba(NO3)2
19. Which of the following solutions would be neutral, acidic or basic?
a) [H+] = 1 x 10 -3- pH = 3 acidic
b) [OH-] = 1 x 10-4 pH = 10 basic
c) pH of 5 - acidic
d) pH of 8- basic
20. A solution contains 4.5 x 10-3 hydrochloric acid. Determine the following:
a) [H3O+] = 4.5 x 10 -3 M
b) [OH] = 1 x 10 -14 / 4.5 x 10 -3 = 2.22 x 10 -12 M
c) pH = -log(4.5 x 10 -3) = 2.35
21. A solution contains 0.025M sulfuric acid. Determine the following:
a) [H3O+]= 2 * 0.025 = 0.05 M
b) [OH-] = 1 x 10 -14 / 0.05 = 2 x 10 -13 M
c) pH = -log ( .05) =1.30
22. A solution contains 0.067 M of sodium hydroxide. Determine the following
a) [H3O+]= 1 x 10-14/ .067 = 1.49 x 10 -13 M
b) [OH-]= 0.067M
c) pOH = 1.17
d) pH= 14 – 1.17 = 12.8
23.
Ammonia will dissociate at a rate of 20%. What would be the pH, given a 0.78
M solution? Ammonia is a base*
20% = 0.20 * 0.78 = .156 M of [OH-] thus pOH = -log(.156) =.807
pH= 14 - .807 = 13.2
24.
What is the molarity of a solution of sulfuric acid with a pH of 4.56?
Antilog (-4.56) = 2.75 x 10 -5 but then you have to divide by 2 because sulfuric acid
has 2 hydrogens thus 1.38 x 10-5 M
What is the molarity of a solution of sodium hydroxide with a pH of 11.3? First
find the pOH = 14 -11.3 = 2.7 then take the antilog(-2.7)=
2.00 x 10 -3 M
25.
26.What is the molarity of a solution if 45.8 g of sodium hydroxide is added to
750 mL of water? What is its pH?
45.8 g of NaOH / 40g = 1.14 moles/ .750L =1.52 M
thus the –log(1.52) = -.182 pOH
14- (-.182) = 14.182 pH
Extra Credit: How many grams of calcium carbonate can be produced, when
235 mL of a 0.444M solution of sodium carbonate reacts with excess calcium
nitrate?
Na2CO3 + Ca(NO3)2 --à 2NaNO3 + CaCO3
235 mL
?g
.444M
(.235L) (.444M)= .104 moles of Na2CO3 * the ratio of 1 mole of Na2CO3 to 1 mole of
CaCO3 = .104 moles of CaCO3 * 100.g = 10.4 g