Chemistry Unit 6

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Description and Tags

Solubilit, Concentration, pH/pOH, Colligative Properties, Acids, Bases, Neutralization, and Equilibrium.

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42 Terms

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A Solution

A homogeneous mixture of one or more solutes dissolved in a solvent.

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Homogeneous Mixture

A mixture in which the composition IS uniform throughout the mixture

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Heterogeneous Mixture

A mixture in which the composition is NOT uniform throughout the mixture

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Three things that will help solutions/reactions form

Agitation, Temperature, Size of particles of the solute

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Solute

The substance that dissolves in a solvent to produce a homogeneous mixture.

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Solvent

The substance in which a solute dissolves to produce a homogeneous mixture.

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Solubility

The amount of solute that can be dissolved in an given amount of solvent at a set temperature and pressure

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when the max amount of solute has been reached

Saturated

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Density

The mass of a substance per unit of volume

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Supersaturated solution

A solution that contains more dissolved solute than required for preparing a saturated solution

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Concentration of a solute

A measure of the amount of solute that is dissolved in a given quantity of solvent

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Concentration = ?

Molarity

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Dilution

Lowering the concentration of the solute by adding more solvet (usally H20)

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Colligitave Properties

Vapor-Pressure Lowering, Freezing-Point Depression, & Boiling-Point Elevation

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Vapor-Pressure

The pressure created by gas that is at equilibrium with its gas

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Vapor-Pressure Lowering

Adding solute lowers the number of gas particles made by \n a liquid solution.

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Freezing-Point Depression

Adding solute blocks solvent particles from gathering \n together and forming a solid.

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Freezing Point

the temperature at which a substance changes to a sold

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Boiling-Point Elevation

Adding solute holds particles together with more force, \n making it harder for individual particles to escape into the gas \n phase.

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Boiling Point

the temperature at which a liquid turns into a gas

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Molality

A measure of solute concentration in a solution (used for colligative property calculations)

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Mole Fraction

The ratio of the # of moles in a solution to the total # of moles in both the solvent & solute

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Acid

pH =1 - 6.9

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Base

pH = 7.1 - 14

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Arrhenius acids/bases

Acids produce H+ & Bases produce OH-

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Bronsted-Lowry acids/bases (primary model we use)

Acids donate protons (H+) & Bases accept protons (H+)

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Lewis acids/bases

Acids accept a pair of electrons & Bases donate a pair of electrons

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Equation for pH

pH = -log[H+]

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Equation for pOH

pOH = -log[OH-]

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What does pH+pOH equal?

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Equation for [H+]

[H+] = 10^-pH

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Equation for [OH-]

[OH-] = 10^-pOH

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Neutralization reactions

Whem a strong acid and a strong base react

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What does a Neutralization reaction contain?

Water and a salt (such as NaCl or KCl)

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Titration

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

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What is the goal of titration

To find the Equivalence Point

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Equivalence Point

point in titration at which the amount of titrant added is just enough to completely neutralize the solution

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Half Equivalence Point

the point at which exactly half of the acid in the buffer solution has reacted with the titrant. ( [HA-]=[A-] )

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Buffer Region

 A region where the pH of a solution remains constant

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Le Chatelier’s Principle

If you mess with a system, it will automatically try to move back to equilibrium

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Chemical Equilibrium

 A state in which the rate of the forward reaction equals the rate of the backward reaction. (aka balanced)

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Concentration & Temperature Changes in Equilibrium

Increase will make it shift away, decrease will make it shift toward