Acid and Base Review Worksheet
Naming Acids: Nonmetal Anion “ide” hydro______ ic acid
Polyatomic Anion “ate” __________ ic acid
Polyatomic Anion “ite” __________ ous acid
Bases: cation (metal or polyatomic) and hydroxide OR memorize bases…Like ammonia
Properties of Acids and Bases
Measuring Acids pH < 7 and pOH > 7 pH = -log [H+] [H+] = 10x -pH
Bases pH > 7 and pOH < 7 pOH = -log [OH-] [OH-] = 10x -pOH
pH + pOH = 14 [H+][OH-]=1.0x10 M
Theories - Arrhenius: Acid (H+) + Base (OH-) salt + water (H2O)
Bronsted-Lowry: dissociation/ionization Reactions
Acid donates a H+ ion to the Base which accepts the H+ ion
Acid + Water (Base) Conjugate Base + Conjugate Acid (H3O+)
Base + Water (Acid) Conjugate Acid + Conjugate Base (OH-)
Neutralization Reactions: Strong Acid + Strong Base Neutral Salt Water
Strong Acid + Weak Base Acidic Salt Water
Weak Acid + Strong Base Basic Salt Water
Strong Acids and Bases – completely dissociate in water – weak bonds
Weak Acids and Bases – not all of the sample dissociates in water – strong bonds
Don’t Forget Molarity M = mol/liter 1L = 1000ml H2O = H+ + OH-
(+)(-) = 0 zero, neutral compound and Balancing Chemical Reactions
Converting form grams to moles using the periodic table
1. What are the chemical formulas for the following acids and Bases:
a. Perchloric Acid Aluminum Hydroxide
b. Sulfurous Acid Nitric Acid
c. Calcium Hydroxide Phosphoric Acid
d. Ammonia Hydrobromic Acid
2. What are three properties of an acid?
3. Write a balanced chemical reaction for calcium metal in hydrofluoric acid.
4. What are three properties of a base?
5. Write a dissociation equation for the reaction of perchloric acid in water. Label the acid, base,
conjugate acid, and conjugate base.
6. Define what it means to be a strong acid or strong base.
7. Fill in the table:
Acid or Base pH pOH [H+] [OH-]
8. Define what it means to be a weak acid or weak base.
9. Write a balanced chemical reaction for the neutralization of hydrophosphoric acid and beryllium
10. Define an amphoteric substance. Give an example.
11. Write the equation for the following neutralization reactions:
NaOH + H3PO4
LiOH + HNO3
Ca(OH)2 + HCl
12. As 0.1M HCl is added to 0.1M KOH, what happens to the pH of the basic solution? Does the
basicity or acidity decrease?
13. Which of the following solutions would contain the highest concentration of OH- ions if 1mol of
each was dissolved in water: H2SO4, NH4Cl, KNO3, NaOH?
14. As the H3O+ ion concentration of a solution increases, what happens to the pH?
15. What is produced by a neutralization reaction?
16. What is the pH of pure water?
17. Find the pH of the following and classify them as acidic (A), basic (B), or neutral (N)
a) [H ] = 2.5 x 10
b) 3.5 x 10-6 M H3P
c) [OH-] = 9.8 x 10-11
d) [H+] = 1.0 x10-7
e) 6.0 x 10-3 M Ba(OH)2
18. According to Bronsted-Lowry, when is H2O considered a base?
19. Complete and balance:
Mg + HNO3 →
Na + H2SO4 →
20. Use (A) to indicate an acid only, (B) to indicate a base only, and (C) to indicate both.
Turns litmus paper red _______ Is a good conductor _______
Has a pH of 3 _______ Produced when sodium reacts with water _______
Tastes sour _______ Reacts with zinc to produce hydrogen _______
Feels slippery _______ Turns pink with phenolphthalein _______
Tastes bitter _______ React with carbonates to produce CO2 _______
21. Name the following acids and bases:
a. CH3COOH Mg(OH)2
b. H2CO3 HNO2
c. H2SO4 KOH
d. HCl HClO
22. The pH of an aqueous solution of sodium hydroxide is 12.9. What is the molarity of the solution?
23. What is the pH of a 0.000460 M solution of Ca(OH)2? (10.96)
24. A student titrates a 20.00 mL sample of a solution of HBr with unknown molarity. The titration
requires 20.05 mL of a 0.1819 M solution of NaOH. What is the molarity of the HBr solution?
(0.1824 M HBr)
25. A 50.00 mL sample of a potassium hydroxide is titrated with a 0.8186 M HCl solution. The
titration requires 27.87 mL of the HCl solution to reach the equivalence point. What is the
molarity of the KOH solution? (0.4563 M KOH)