Acids and Bases
Word
/ DefinitionArrhenius Acid / An electrolyte that ionizes in aqueous solution to yield H+ as the only positive ion in solution.
Arrhenius Base / An electrolyte that ionizes in aqueous solution to yield OH- as the only negative ion in solution.
Electrolyte / A compound that ionizes in water, allowing the solution to conduct electricity.
Salt / An ionic compound formed when an acid and base neutralize each other. This compound consists of the anion of the acid and the cation of the base.
Nonelectrolytes / A molecular compound that does not ionize in water, preventing the solution from conducting electricity.
Indicator / A substance whose color is sensitive to the pH of a solution to which it is added.
Bronsted-lowry / an alternate way to describe acids and bases
Titration / A process of controlled acid-base neutralization, carried out in burets.
pH / The negative log of the hydrogen ion concentration. A pH less than 7 indicates an acidic solution, a pH of greater than 7 indicates a basic solution and a pH of 7 indicates a neutral solution.
Neutralization / A double-replacement reaction where an acid and base react to form water and a salt.
A. Defining Acids, Bases, and Salts
1. Arrhenius acids and bases are electrolytes.
2. An electrolyte, dissolved in water, has the ability to conduct electricity. The ability to conduct electricity depends on the concentration of the ions.
3. Arrhenius acids yield hydrogen ions (H+), hydronium ion (H3O+), as the only positive ion in an aqueous solution.
4. Arrhenius bases yield hydroxide ions (OH-) as the only negative ion in an aqueous solution.
5. Describe properties of Acids, Bases, and Salts.
a.) Given properties, identify substances as Arrhenius acid or Arrhenius base.
Acid Properties Base Properties
pH: less than 7 greater than 7
Taste: Sour Bitter
Reacts w/Metal Yes (metals must be No
above **H2 on
Ref Table J)
Effect on
Litmus Paper Turns Red Turns Blue
Effect on
Phenolpthalein Colorless Pink
6. Bronted-Lowry theory states that an acid is a proton donor
and a base is a proton acceptor.
7. The acidity or alkalinity(basicity) of a solution can be measured by its pH value.
8. On the pH scale, each decrease of one unit of pH indicates a tenfold increase in the hydronium ion concentration.
a.) Identify solution as acid, base, or neutral based upon the pH.
Acids = pH > 7 (More H+/H3O+ ions than OH- ions)
Bases = pH < 7(More OH- ions than H+/H3O+ ions)
Neutral = pH = 7 (Equal H+/H3O+ ions and OH- ions)
9. The relative level of acidity in a solution can be shown with indicators.
Interpret changes in acid-base indicator color.
Reference Table M
B. Reactions of Acids and Bases
1. In the process of neutralization, an acid and a base react to form a salt and water.
a.) Write simple neutralization reactions when given the reactants. Double Replacement Reaction
Acid + Base à Salt + H2O
2. Titration is a process in which a volume of solution of known concentration is used to determine the concentration of another solution.
3. Calculate the molarity of an acid or base.
4. Solve titration problems.
a.) Calculate the concentration, or volume of a solution, using titration data.
MAVA=MBVB
1) ACIDS AND BASES HOMEWORK
A) Identify each as an acid or base based on their formulas and properties.
Property / Acid or Base? / Property / Acid or Base?Turns litmus red / Turns phenolphthalein clear
Tastes sour / Tastes bitter
Hydrolyzes fats into soap / Reacts with active metals to form H2
HCl (aq) / KOH (aq)
pH of 12 / Forms H3O+ in water
B) Which of the following metals will react in the presence of an acid?
1) Cu b) Ag c) Zn d) Au
C) Name the following acids:
1) HCl (aq) ______
4) HNO3 (aq) ______
3) H2SO4 (aq) ______
4) HBr (aq) ______
5) HC2H3O2 (aq)______
D) Write the formulas of the following acids:
1) Hydrofluoric acid ______
2) Phosphoric acid ______
3) Hydrobromic acid ______
E) Name the following bases:
1) KOH (aq)______
2) Ca(OH)2 (aq)______
3) LiOH (aq)______
F) Write the formulas for the following bases:
1) aluminum hydroxide______
2) barium hydroxide______
3) sodium hydroxide______
G) What is the pH of a solution that turns methyl orange to yellow, phenolphthalein to clear, bromcresol green to blue and thymol blue to yellow?
a) 2.7 b) 5.6 c) 9.0 d) 10.2
Explain how you arrived at your answer, using the process of elimination to show how you used Reference Table M to eliminate each choice.
· 2) Acid and Base Neutralization Homework
A) Write the formula of the salt formed in each reaction:
1) H2SO4 (aq) + Mg(OH)2 (aq) à 2 HOH + ______
2) H3PO4 (aq) + 3 NaOH (aq) à 3 HOH + ______
3) H2CO3 (aq) + 2 KOH (aq) à 2 HOH + ______
4) H2SO4 (aq) + 2 KOH (aq) à 2 HOH + ______
B) Write the formula of the acid used in each reaction:
1) 3 ______(aq) + 2 Al(OH)3 (aq) à 6 HOH (l) + Al2(SO4)3 (aq)
2) 2 ______(aq) + Ba(OH)2 (aq)® 2 HOH (l) + Ba(C2H3O2)2 (aq)
3) ______(aq) + 2 NH4OH (aq) à 2 HOH + (NH4)2CO3
C) Write the formula of each base used in each reaction:
8) H2SO3 (aq) + ______(aq) ® 2 HOH (l) + MgSO3 (aq)
9) 2 H3PO4 (aq) + 3 ______(aq) ® 6 HOH (l) + Ca3(PO4)2 (aq)
10) 2 HCl + ______® CaCl2 (aq) + 2 HOH (l)
C) Solve the following titration problems:
1) How many moles of KOH are needed to neutralize 1.5 moles of H2SO4?
2) How many moles of NaOH are needed to neutralize 3.0 moles of HCl?
3) How many moles of H3PO4 are required to exactly neutralize 5.0 moles of KOH?
4) What volume of 0.80 M HCl will exactly neutralize 100. mL of 0.40 M KOH?
5) If exactly 5.0 mL of HNO3 will neutralize 15 mL of 2.0 M NaOH, what is the molarity of the HNO3 solution?
6) What volume of 0.25M HCl is needed to neutralize 1.5 L of 4.0 M NaOH?
7) What volume of 5.0 M NaOH is needed to neutralize 40. mL of 2.0 M HCl?
8) What is the molarity of an H2CO3 solution if it takes 50. mL of H2CO3 to exactly neutralize 100. mL of
0.50 M NaOH?
9) What is the molarity of a NaOH solution if it takes 100. mL of NaOH to neutralize 50. mL of 0.10 M H2SO4?
10) What is the molarity of a 2.0 L sample of HCl that exactly neutralizes 1.0 L of a 2.00 M sample of NaOH?
11) 50. mL of H2SO4 of unknown concentration is titrated with 25 mL of 5.0 M NaOH. What is the molarity of the H2SO4?
12) How many mL of 0.50 M HCl are required to neutralize 30. mL of 2.0 M Mg(OH)2?
13) How many mL of 1.0 M H3PO4 are required to neutralize 50. mL of 3.0 M NaOH?
14) 200. mL of KOH are required to neutralize 100. mL of 0.10 M H2SO4. What is the molarity of the KOH?
15) How many moles of HCl can be neutralized by 0.50 L of 0.10 M NaOH?
16) How many moles of H2SO4 can be neutralized by 0.10 L of 0.50 M NaOH?
3) The Power of Hydronium Homework
1) A pH of 4 is how many times more acidic than a pH of 6?
2) A pH of 11 is how many times more basic than a pH of 8?
3) Which of the following solution pH values is the most acidic?
a) 5 b) 7 c) 9 d) 11
4) A pH of 14 is how many times more basic than a pH of 12?
a) 10 times b) 100 times c) 1000 times b) 10000 times
5) Which of the following solutions can have a pH of 5?
a) a 10-5 M solution of HCl b) a 10-5 M solution of NaOH
c) a 10-5 M solution of NaCl d) a 10-5 M solution of CH4
6) What is the color of methyl orange in a solution whose pH is 9?
Is this an acid or a base?
7) What is the color of litmus in a solution whose pH is 10?
Is this an acid or a base?
8) What is the color of bromcresol green in a solution with a pH of 2?
Is this an acid or a base?
9) What is the color of thymol blue in a solution with a pH of 13?
Is this an acid or a base?
10) What is the pH of a solution formed when equal volumes of 0.1 M HCl and 0.1 M NaOH are added to a beaker?
a) less than 7 b) more than 7 c) exactly 7
4) Alternate Theory of Acids and Bases
For each of the following systems, identify the acid and base:
1. HBr + H2O <====> H3O+ + Br-2. H2O + H2O <====> H3O+ + OH-
3. NH3 + OH- <====> NH2- + H2O
4. H2O + HPO42- <====> PO43- + H3O+
5. H3PO4 + H2O <====> H2PO4- + H3O+
6. CH3COO- + H3O+ <====> HCH3COO + H2O
7. H2PO4- + CH3COO- <====> HCH3COO + HPO42-
8. H2O + S2- <====> HS- + OH-
9. CN- + HCH3COO <====> HCN + CH3COO-
10. OH- + NH4+ <====> H2O + NH3