Solution Chemistry Lecture

These flashcards cover the key concepts and definitions in solution chemistry discussed in the lecture.

What is a solution?

A homogeneous mixture of two or more substances.

What are the components of a solution?

The solvent (present in the larger amount) and the solute (present in the smaller amount).

What is the most commonly used solvent in solution chemistry?

Water.

What do you call a solution where water is the solvent?

An aqueous solution.

What is molarity?

A way of expressing concentration, defined as moles of solute per liter of solution.

What is a 1 molar (1 M) solution?

A solution that contains 1 mole of solute in 1 liter of total solution.

How do you create a 1 molar sodium chloride solution?

Dissolve 1 mole of sodium chloride in enough water to make 1 liter of solution.

How do you calculate molarity?

Molarity = moles of solute / liters of solution.

What does disassociation in solutions refer to?

Ionic compounds breaking apart into their respective ions surrounded by water when dissolved.

In a titration, what is the point called where the amount of acid equals the amount of base?

The equivalence point.

What does a standard solution mean in titrations?

A solution with a known concentration used in titrations.

What kind of acid is hydrochloric acid considered?

A strong acid.

What is the function of an indicator in a titration?

It signals the endpoint of the titration by changing color.

What is the molar mass of potassium bromide (KBr)?

Approximately 119.00 g/mol.

How much sodium bicarbonate is required to neutralize sulfuric acid if 27 mL of 6 M sulfuric acid is spilled?

Approximately 27 grams of sodium bicarbonate.

What is the reaction when baking soda neutralizes acid?

It produces sodium ions and water, releasing carbon dioxide gas.

How do you figure out the concentration of an ion in a solution?

By determining how many moles of the ion are produced per liter of the solution.