Unit 4 - Acids and Bases & Solubility Flashcards Preview

SCH 3UI > Unit 4 - Acids and Bases & Solubility > Flashcards

Flashcards in Unit 4 - Acids and Bases & Solubility Deck (21):

Difference between monoprotic, diprotic, and polyprotic acids

Monoprotic acids can donate 1 proton (H+), diprotic acids can donate up to 2 protons, polyprotic acids can donate more than 2 protons


What is an amphiprotic compound?

A compound that acts as both an acid and base


T/F: Solutions are homogenous.

True, there is only one visible phase.


Is the solute dissolved in the solvent or the solvent dissolved in the solute?

The solute is dissolved in the solvent.


Define dissociation.

the separation of ions that occurs when an ionic compound dissolves in water


How do you prepare a standard solution (from a solid)?

1. Calculate and measure the mass of solid needed using concentration equation (C = n/V)
2. Dissolve solid in small amount of pure water.
3. Transfer the solution into a volumetric flask and add pure water until desired volume is reached.


How do you perform a dilution?

1. Calculate the volume of standard solution (vi, Ci) required to prepare the desired concentration and volume (Cf, vf) of diluted solution.
2. Add a small amount of pure water into a volumetric flask.
3. Measure and transfer the appropriate amount of initial solution into the flask.
4. Add the remaining water to reach desired volume.


Define concentration.

The quantity of a given solute in a solution.


Another term for molar concentration

Molarity - the number of moles that can be dissolved in 1L solution


T/F: Solid ions do not dissociate into ions.



What is the purpose of ionic equations?

Ionic equations show the dissociation of soluble ionic compounds in solution.


What is a net ionic equation?

Ionic equations without the spectator ions


Level of saturation is the point on the solubility curve is a) above the curve, b) below the curve, c) directly on the curve

a) supersaturated
b) unsaturated
c) saturated


miscible & immiscible

Liquids that mix well are miscible.
Liquids that do not mix well are immiscible.


Properties of acids

- pH lower than 7
- sour taste
- form hydronium ions (H3O+ or H+=H2O) in aqueous solutions
- react with many metals to form hydrogen gas
- electrolytes
- form H+ ions or protons in solution


Properties of bases

- bitter taste
- feel slippery
- form hydroxyl ions (OH-) in solution
- pH higher than 7


Define titration

A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution.


Svante Arrhenius theory of acids and bases

Acids: any compound which produces hydrogen ions (H+) in solution
Bases: any compound which produces hydroxide ions (OH-) in solution


Bronsted-Lowry definition of acids and bases

Acids: a proton (H+) donor
Bases: a proton (H+) acceptor


Lewis definition of acids and bases

Acids: electron pair donors
Bases: electron pair acceptors


Define electrolyte

A compound that conducts electricity in aqueous solution