Chapter 3B - Writing Half Equations

Question 1

Describe redox reactions in acidic conditions:

Answer 1

• solution with a greater concentration of hydrogen ions than hydroxide ions

Question 2

KOHES - acidic conditions

Answer 2

Key Elements
Oxygen atoms (add water)
Hydrogen atoms (add H⁺)
Electrons
States

Question 3

Describe redox reactions in basic conditions

Answer 3

• solution with a greater concentration of hydroxide ions than hydrogen ions

Question 4

KOHOHES - basic conditions

Answer 4

Key elements
Oxygen atoms (add H₂O)
Hydrogen atoms (add H⁺)
OH - add OH⁻ ions to both sides of the equation for every H⁺
Electrons
States

Question 5

What is the formula for pH?

Answer 5

pH = -log₁₀[H⁺]

Question 6

Describe pH changes in an acidic electrolyte:

Answer 6

• if H⁺ produced, pH decreases (more acidic)
• if H⁺ consumed, pH increases (less acidic)

Question 7

Describe the pH changes in a basic electrolyte:

Answer 7

• if OH⁻ produced, pH increases (more basic)
• if OH⁻ consumed, pH decreases (more acidic)