Module 5 Intro
1. Module 5 Intro
1.6. Page 4
Module 5—Acids and Bases
Self-Check
SC 1. Earlier, you examined a table listing the empirical properties of acids and bases. Discuss any benefits, limitations, or concerns with using each of the tests listed in the table to categorize a solution as being acidic, basic, or neutral.
SC 2. Write a balanced equation for the change associated when each of the following substances is dissolved in water. Indicate which changes involve dissociation and which involve ionization.
- HF(g) →
- Ba(OH)2(s) →
- HNO3(aq) →
SC 3. Complete the following table.
Common Name |
Systematic IUPAC Name |
Formula |
|
aqueous hydrogen borate |
H3BO3(aq) |
benzoic acid |
benzoic acid |
|
barium hydroxide |
barium hydroxide |
|
|
aqueous hydrogen phosphate |
H3PO4(aq) |
hydrosulfuric acid |
aqueous hydrogen sulfide |
|
|
aqueous hydrogen chlorite |
HClO2(aq) |
hydroiodic acid |
aqueous hydrogen iodide |
|
carbonic acid |
aqueous hydrogen carbonate |
|
|
aqueous hydrogen nitrite |
HNO2(aq) |
|
aqueous hydrogen fluoride |
HF(aq) |
acetic acid |
|
|
|
aqueous hydrogen chromate |
H2CrO4(aq) |
sulfurous acid |
aqueous hydrogen sulfite |
|
|
|
NaHCO3(aq) |
SC 4. Complete “Practice” questions 1 and 2 on page 251 of your textbook.
Self-Check Answers
SC 1.
Conductivity: It’s useful for separating out neutral molecular solutions, but it cannot distinguish between acids, bases, and neutral ionic solutions.
Litmus: It can be used to distinguish between acids, bases, and neutral solutions, but it does not give an exact pH value.
Taste: Taste may be used to recognize acids and dissolved salts (such as table salt), but solutions must never be tasted in the lab for safety reasons.
Feel: Feel may help distinguish between an acid and a base, but, again, this should never be carried out in a lab for safety reasons.
pH: The pH of a solution can be used to distinguish between acids, bases, and neutral solutions, but it requires the use of indicators (which you will learn later in this module) or an expensive pH meter.
SC 2.
- HF(g) → H+(aq) + F−(aq), ionization
- Ba(OH)2(s) → Ba2+(aq) + 2 OH−(aq), dissociation
- HNO3(aq) → H+(aq) + NO3−(aq), ionization
- H2SO4(aq) → 2 H+(aq) + SO42−(aq), ionization
SC 3.
Common Name |
Systematic IUPAC Name |
Formula |
boric acid |
aqueous hydrogen borate |
H3BO3(aq) |
benzoic acid |
benzoic acid |
C6H5COOH(aq) |
barium hydroxide |
barium hydroxide |
Ba(OH)2(aq) |
phosphoric acid |
aqueous hydrogen phosphate |
H3PO4(aq) |
hydrosulfuric acid |
aqueous hydrogen sulfide |
H2S(aq) |
chlorous acid |
aqueous hydrogen chlorite |
HClO2(aq) |
hydroiodic acid |
aqueous hydrogen iodide |
HI(aq) |
carbonic acid |
aqueous hydrogen carbonate |
H2CO3(aq) |
nitrous acid |
aqueous hydrogen nitrite |
HNO2(aq) |
hydrofluoric acid |
aqueous hydrogen fluoride |
HF(aq) |
acetic acid |
ethanoic acid |
CH3COOH(aq) |
chromic acid |
aqueous hydrogen chromate |
H2CrO4(aq) |
sulfurous acid |
aqueous hydrogen sulfite |
H2SO3(aq) |
sodium hydrogen carbonate |
sodium hydrogen carbonate |
NaHCO3(aq) |
SC 4. “Practice” questions 1 and 2 on page 251
- HI(aq) + H2O(aq) → H3O+(aq) + I–(aq)
A reaction with water produces a hydronium ion, making the solution acidic.
- HOCl(aq) + H2O(aq) → H3O+(aq) + OCl–(aq)
A reaction with water produces a hydronium ion, making the solution acidic.
- H3PO4(aq) + H2O(aq) → H3O+(aq) + H2PO4–(aq)
A reaction with water produces a hydronium ion, making the solution acidic.
- Na2SO4(aq) dissociates into sodium ions and sulfate ions. Sulfate ions can react with water to form hydroxide ions, as shown in the following reaction:
SO42–(aq) + H2O(aq) → HSO4–(aq) + OH–(aq)
- NaCH3COO(aq) dissociates into sodium ions and ethanoate ions. Ethanoate ions can react with water to form hydroxide ions, as shown in the following reaction:
CH3COO–(aq) + H2O(aq) → CH3COOH(aq) + OH–(aq)
- Sr(OH)2(aq) dissociates into strontium ions and hydroxide ions.
Sr(OH)2(aq)→ Sr2+(aq) + 2 OH–(aq).