Chem 20 Chapter 5 unit test review

solubility

is the ability of a substance, known as the solute, to dissolve in a solvent to form a homogeneous solution. It is usually measured in terms of the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure. Can be affected by factors such as temperature, pressure, and the chemical nature of the solute and solvent.

Saturated Solution

A solution in which the maximum amount of solute has been dissolved at a given temperature and pressure. It is in a state of equilibrium between the undissolved solute and the dissolved solute.

In liquids how can you increase solubility?

Miscible ot Immiscable

In solids how can you increase solubility?

By increasing temperature, reducing particle size, and agitating the mixture.

miscible

When two or more substances are capable of mixing together to form a homogeneous solution. When a liquid dissolves in another liquid.

Immiscible

liquids that don’t dissolve in each other eg. oil and water.

elements

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Elements are substances made of atoms with the same number of protons. they have very low solubility and their solubility is therefore not very effected by other factors.

dynamic equilibrium

A state of balance in a system where the forward and reverse reactions occur at equal rates. The concentrations of reactants and products remain constant over time.

dissociation

name of reaction when an ionic compound dissolves in water.

molecular compounds

Type of compound formed by covalent bonding between non-metal atoms. They share electrons to achieve a stable octet configuration. They have low melting and boiling points, and do not conduct electricity in any state.

Ionic compounds

Type of chemical compound formed by the attraction between positively and negatively charged ions. They have high melting and boiling points, are usually soluble in water, and conduct electricity when dissolved or melted. Examples include NaCl (table salt) and CaCO3 (calcium carbonate).

Bases

Bases are a type of chemical compound that can accept protons from acids, producing hydroxide ions. They are usually slippery to the touch and have a bitter taste. Examples include sodium hydroxide (NaOH) and ammonia (NH3). Bases are IONIC.

Acids

Substances that donate hydrogen ions (H+) in a solution, resulting in a decrease in pH and the ability to react with bases to form salts. formula will either start with H- or end with COOH. They must be (aq to display acidic properties).

What entity rules do bases follow

Ionic

When will acids stay together in the entities?

When they are a weak acid.

What entity rules do c=molecular compounds follow?

never split up, change state if they have hydrogen bonding or are polar (high solubility).

endothermic

Process that absorbs heat from the surroundings. It requires energy input to occur, resulting in a decrease in temperature of the surroundings. Examples include melting ice and photosynthesis.

exothermic

A type of chemical reaction that releases heat energy to the surroundings.

when bonds break energy is

When bonds break, energy is __absorbed__.

when bonds form energy is

When bonds form, energy is __released__.

dissociation ____ __bonds which__ __ energy

Dissociation breaks bonds which requires energy

concentration

a ratio of solute compared to teh entire solution c=n/v

Parts per million units

Mg/Kg, Mg/L

Stock solution

an initial solution with a known concentration that samples are then taken from to make further solutions.

Standard solution

A less concentrated solution usually made from a stock solution. Has a known concentration.

solvent

disolver

Solute

Disolved

electrolytes

conduct electricity

non electrolytes

can not conduct electricity

Ammonia

NH3(g)

Hydrogen Peroxide

H2O2(l)

Glucose

C6H12O6

Sucrose

C12H22O11 (s)

Methane

CH4(g)

Methanol

CH3OH(l)

Ethanol

C2H5OH (l)

Propane

C3H8(g)

Hydrogen Sulfide

H2S (s)

Water

H20(l)