Chapter 4- Reactions in Aqueous Solutions

What is an aqueous solution?

When the solute of a solution is a liquid or solid and the solvent is water

What is an electrolyte?

A substance whose aqueous solutions contains ions (give electrically conducting solution)

What are strong and weak electrolytes?

• Strong- Dissociates completely in water, single reaction arrow

• Weak- Only dissociates partially when dissolved in water, half arrows and produces state of chemical equilibrium

What does to it mean to precipitate?

Insoluble solid formed by a reaction in a solution

What are acids, monoprotic acids and diprotic acids?

• Acids- substances that ionize in aqueous solutions to form hydrogen ions H+, increasing concentration of H+

• Monoprotic- yielding on H+ per molecule of acid

• Diprotic- yields two H+ per one molecule

What is a net ionic equation?

Eliminates spectator ions and shows the actual chemical change occurring

What is the difference between arrhenius, bronsted-lowry and lewis acids/bases?

• Arrhenius- acid increases the amount of hydrogen ions/base increases the hydroxide ions

• Bronsted Lowry- acids donate H+ ions/bases accept H+ ions

• Lewis- acids accept electron pairs/bases donate electron pairs

What is the relationship between acids/bases and conjugate pairs?

• Stronger acids= form weaker conjugate bases

• Stronger bases= form weaker conjugate acids

What are neutralization reactions?

When a strong acid reacts with a strong base

What occurs during oxidation and reduction?

• Oxidation- loss of electron

• Reduction- gain of electron