reactivity 3

ib chem sl

acids are neutralized by

bases

bases are neutralized by

acids

acids taste

sour

bases taste

bitter

acids react with

some metals and carbonates

Arrhenius acid

covalently bonded polar molecules that dissociate into H+ ions and anions in water

strong acids

fully dissociate

weak acids

partially dissociate

weak acids are written with

a double arrow for incomplete reaction

Arrhenius base

produce OH- ion in water

alkali

water soluble base

common strong bases

LiOH, NaOH, KOH, Ba(OH)2

acids and bases

neutralize one another

acid and bases form

a salt and water

arrhenius theory does not explain

how a substance like ammonia (NH3) is a base

why shouldn’t ammonia be a base

because it does not have a OH- ion

bronsted-lowry acid

proton (H+) donor

bronsted-lowry base

proton (H+) acceptor

when a base accepts the H+ it becomes

a conjugate acid

when an acid donates the H+ it becomes

a conjugate base

amphiprotic species can

both accept and donate a proton

an example of an amphiprotic species is

water (H2O)

water can

self-ionize

in pure water

[H+] = [OH-]

water’s pH is

7

pH formula

-log [H+]

for log sig figs

the number of decimal places in the logarithm (left of decimal point not counted)

[H+] x [OH-]

1 × 10^-14

pOH

-log[OH-]

pH + pOH

14

can determine pH using

pH meters

indicators

pigments which respond to differenced in H+ concentration

one of the first indicators was

litmus made from lichen

universal indicator

a liquid that contains a blend of several indicators

pH paper/pH strips

blend of indicators dried on paper

you can make a homemade indicator using

red cabbage juice

acid + metal react to make

salt + H2

for a acid and metal reaction metal must be

an active metal

active metal

above H on activity series

acid + metal gives off H2 gas through

effervescence

effervescence

bubbling

salt

a compound formed when the H+ in an acid is replaced by a metal cation or ammonium

acid + metal carbonate react to make

salt + water + CO2

acid + ammonia react to make

ammonium salt

acid + base react to make

salt + water

acid + base reactions are

exothermic

in acid + base reactions, base can be

metal hydroxide or metal oxide

acid + base reactions are what type of reaction

neutralization

titration

a method for determining the concentration of a solution by reacting it with another solution with a known concentration

solutions

homogenous mixtures of two or more substances

solute

what is being dissolved

solvent

liquid doing the dissolving

when dissolves the solute separates into

individual particles

types of solutions

gaseous, liquid, solid

concentration

the amount of solute dissolved in a solvent

dilute

relatively small amount of solute

concentrated

relatively large amount of solute

unsaturated

less than the maximum concentration of dissolved solute

saturated

maximum concentration of dissolved solute

supersaturated

more than maximum amount of dissolved solute

supersaturated solutions usually require

heating then cooling a solution

supersaturated solutions are

uncommon

once a solution reaches the saturation point the additional solute

remains undissolved at the bottom

solubility

the amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution

polar and ionic solutes dissolve in

polar solvents

nonpolar solutes dissolve in

nonpolar solvents

miscible liquids can

easily dissolve in one another

immiscible liquids are

not soluble in each other

gases are _____ miscible in any proportions

always

for solids, as solubility increases, temperature

increases

for gases, as solubility decreases, temperature

increases

solubility curves

show the maximum amount of solute which can be dissolved in an amount of solvent

solubility curves are used to determine

if a solution is saturated or unsaturated

molarity

concentration in mole per cubic decimeter (mol cm^-3)

molarity formula

mole solute / dm³ solution

c

n/v

stock solution

a solution of known concentration that is available for diluting

dilution formula

c1v1 = c2v2

combustion reaction of sulfur

S (s)+ O2 (g) → SO2 (g)

further combustion of SO2

2SO2 (g) + O2 (g) → 2SO3 (g)

creation of sulfuric acid

SO3 (g) + H2O (l) → H2SO4 (aq)

nitrogen oxides produce

acid rain

only type of acids that can produce acid rain

-ic acids

ph higher than 7 means temp

decrease

pH lower than 7 means temp

increase

amines are always

bases