Chapter 4: Reactions in Aqueous Solutions

This set of flashcards covers key definitions, concepts, and processes related to reactions in aqueous solutions, electrolytes, solubility, acid-base reactions, and analytical techniques.

What is a solution?

A homogeneous mixture of 2 or more substances.

What is a solute?

The substance present in the smaller amount in a solution.

What is a solvent?

The substance present in the larger amount in a solution.

Define electrolyte.

A substance that, when dissolved in water, results in a solution that can conduct electricity.

Define nonelectrolyte.

A substance that, when dissolved, results in a solution that does not conduct electricity.

What is a strong electrolyte?

An electrolyte that completely dissociates into ions in solution.

What is a weak electrolyte?

An electrolyte that does not completely dissociate into ions in solution.

What is hydration?

The process in which an ion is surrounded by water molecules arranged in a specific manner.

What is a precipitate?

An insoluble solid that separates from a solution.

What are the solubility rules for common ionic compounds regarding nitrates?

All nitrates are soluble.

What does the term solubility refer to?

The maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature.

What is required to write a net ionic equation?

1. Write the balanced molecular equation. 2. Write the ionic equation. 3. Cancel spectator ions. 4. Ensure charges and atoms are balanced.

How does a Brønsted-Lowry acid differ from a Brønsted-Lowry base?

Acids are H+ donors, while bases are proton acceptors.

What defines a neutralization reaction?

An acid and a base react to produce a salt and water.

What is titration?

A method where a solution of known concentration is gradually added to a solution of unknown concentration until the reaction is complete.

What is the definition of molarity?

The number of moles of solute divided by the volume of solution in liters.

Define dilution in the context of solutions.

The process of reducing the concentration of a solute in solution, usually by adding more solvent.