Balancing Redox Reactions in Basic Solutions

This video tutorial explains how to balance redox reactions in basic solutions, building on previous knowledge of acidic solutions. It covers determining oxidation states, writing half reactions, and balancing atoms, hydrogens, and charges. The tutorial emphasizes the importance of equalizing electrons and adjusting the reaction for basic conditions by adding hydroxide ions to neutralize protons.

What is added in step four to balance redox reactions in a basic solution?

• Electrons

• Water molecules

• Hydroxide ions

• Chloride ions

What is the oxidation state of chromium in Cr(OH)4?

• +6

• +4

• +2

• +3

What is the oxidation state of chlorine in the hypochlorite anion?

• 0

• +2

• -1

• +1

Which element is being oxidized in the reaction?

• Hydrogen

• Chromium

• Oxygen

• Chlorine

Which compound is reduced in the reaction?

• Hypochlorite

• Chloride

• Chromium hydroxide

• Chromate

What is the purpose of adding water in step three of the balancing process?

• To neutralize the solution

• To balance the electrons

• To balance the hydrogen atoms

• To balance the oxygen atoms

How many electrons are added to the right side of the oxidation half reaction to balance the charges?

• Six electrons

• Three electrons

• Two electrons

• Four electrons

How are the electrons balanced between the oxidation and reduction half reactions?

• By adding water

• By adding protons

• By adjusting coefficients

• By adding hydroxide ions

What is the final number of water molecules on the product side after balancing?

• Four

• Five

• Three

• Two

What is added to both sides of the equation to balance the protons in a basic solution?

• Protons

• Hydroxide ions

• Electrons

• Water molecules