chem 20 acids and bases 5.1/5.2

matter - 2

pure substances and mixtures

pure substance

substance with one type of particle

mixture

substances with more than one type of particle

mixtures consist of - 2

homogeneous mixtures

heterogeneous mixtures

homogeneous mixture

particles are uniformly mixed; same properties throughout

heterogeneous mixture

particles are NOT uniformly mixed; different properties in small samples

Solutions are ________ mixtures or __________ solutions.

homogeneous

aqueous

solutions composed of

at least one solute and one solvent (can be solid, liquid, or gas)

aqueous solutions

the solute is dissolved in water (water is the solvent)

(aq)

aqueous solutions - precipitation reactions

require dossolving reactants in water before you can produce precipitate (one product is a solid)

acidic aqueous solutions - 2

included solutions with hydrogen bonded to an anion

starts with H or ends with COOH

acidic solution diagnostic test

blue litmus -> red

red litmus stays red

pH < 7

conducts electricity

basic aqueous solution

includes ionic compounds containing the hydroxide (OH^-) ion and ammonia gas (NH3) in solution

basic solution diagnostic test

red litmus -> blue

blue litmus stays blue

pH > 7

conducts electricity

neutral aqueous solution

may be neutral ionic

may be neutral molecular

neutral solution diagnostic test

no change in litmus colour

pH = 7

ionic conducts electricity

molecular DOES NOT conduct electricity

electrolytes

IONIC COMPOUND

aqueous solution that conducts electricity

electrolytes have ions in the solution

ex/ soluble ionic compounds, acids and bases

form ions in solutions

ionic particles "dissociate"

strong acids "ionize"

nonelectrolytes

MOLECULAR

aqueous solution that does NOT conduct electricity

ex/ solution with a molecular substance

form electrically neutral particles in solution

particles "dissolve/disperse"

entities list - elements have low solubility

leave them in original state

add water as second entity

ex/ nitrogen gas mixed in water -> N2 (g), H2O (l)

entities list - ionic compounds with low solubility

check solubility table for low/high solubility

ions will stay together when mixed with water - do not break compound apart

ex/ solid dilver sulfate in water -> Ag2SO4 (s), H2O (l)

entities list - ionic compounds with high solubility

check solubility table for high/low solubility

ions will dissociate when mixed with water - seperate compound and add charges (aq cuz mixed w water)

ex/ solid magnesium chloride in water -> Mg2+ (aq), Cl- (aq), H2O (l)

entities list - molecular substances with low solubility

non-polar compounds have LOW SOLUBILITY in water

keep them in original state - add water as second entity

ex/ octane (C8H18 (l)) in water -> C8H18 (l), H2O (l)

entities list - molecular substances with high solubility

polar compounds have HIGH SOLUBILTY (sugars, proteins, vitamins)

molecules dissolve/disperse when mixed with water - show as dissolved by changing state to (aq) - keep compound together

ex/ solid sucrose (C12H22O11 (s)) in water -> C12H22O11 (aq), H2O (l)

entities list - strong acids (top six)

full ionize/react with water to form ions

break them apart into H+ (aq) and anion - include water as another entity

ex/ nitric acid (HNO3 (aq)) -> H+ (aq), NO3- (aq), H2O (l)

entities list - weak acids (everything below top six)

do not fully ionize (leave them as molecules) - change state to (aq)

ex/ acetic acid (CH3COOH) in water -> CH3COOH (aq), H2O (l)

dissociation equations show as an equation what happens to

ionic compounds (all solid at room temp) when added to water

do dissociation equations include water?

no, but entities do

dissociation product states are

aqueous (aq)

dissociation of soluble ionic compounds

start with solid, seperate into ions

ex/ NaCl (s) -> Na+ (aq) + Cl- (aq)

(NH4)3PO4 (s) -> 3NH4 + (aq) + PO4 3- (aq)

dissociation of not soluble ionic compounds

show that it has dissolved, but do not break apart into ions

( (aq) all ionic compounds are soluble to a degree)

ex/ CaSO4 (s) -> CaSO4 (aq)

2 diagnostic tests - aqueous solution of a molecular substance

doesnt conduct

no change in litmus paper

2 diagnostic tests - aqueous solution of a neutral ionic compound

conducts electricity

no change in litmus paper

2 diagnostic tests - aqueous solution of an acid

conducts electricity

red litmus

2 diagnostic tests - aqueous solution of a base

conducts electricity

blue litmus

what is believed to happen when ionic compund dissolves in water

- cations of compound surrounded by negative ends of water and pulled away from crystal

- anions of compound surrounded by positive ends of water and pulled away from crystal

all reactancts of dissociation equations start as (state)

solid

when do you write charges for products/entities?

dissociaion products

entities of ionic with high solubulity

strong acids

when do you balance entities?

don't balance entities (balance compound tho if it does not break down)

aqueous means

it has water + very soluble

for entities, does water have a charge?

no charge on water (so its H2O (l))

for entities, elements -

have low solubilty so they stay in original state

don't add charge