G11 Chem - Unit 4 Solubility

Solution

homogenous mixture of 2+ substances

Phase

Distinct parts of a mixture

Aqueous solution

one that contains H2O

Heterogenous Mixture

One with 2+ Phases like a salad, Also all liquid or gas mixtures that are translucent or opaque

What type of mixture is a translucent/opaque gas/liquid

Heterogenous

Solvent

Component in solution that dissolves smth, present in greater amount

Solute

Gets dissolved, less amount e.g salt

Concentration

Ratio of quantity of solute/solvent

Concentrated solution

Solution with lots of dissolved solute per unit of solvent

Dilute solution

Solution with small quantity of dissolved solute per unit of solvent

Alloy

Solution of 2+ metals

Amalgram

Alloy with mercury and others used for teeth

Aqueous Solution

Solution where water = solvent

3 types of interaction to consider when forming solution

1) strength between solute-solute

2) strength between Solute- Solvent

3) strength between Solvent-Solvent

What has to happen for solution to form

solute & solvent must be more attracted to each other thans itself as solvent-solvent and solute-solute interactions must be distrupted

Steps in dissolving process and energy required

1) forces between solute (ENERGY)

• ionic solid = electrostatic attraction

• Cov solid - force of attraction

2 ) Forces between solvent (ENERGY)

3) Has to be interaction between solvent+solute (GIVES OFF ENERGY)

Hydrogen bond

Attraction between hydrogen atom and FON electroneg atom

ionic compounds soluble in H2O? why

Mostly are, Ions Attracts between ions nad dipoles of water pull ions away from surface of solid

Hydration

Process of H2O surrounding ions

Dissociation

Separation of indiv ions from ionic compound as dissolving in H2O

dissociation Equations

Shows how ionic compound dissociates w states and charges
e.g NaCl(s) —> Na+(aq) + Cl- (aq)

Do polyatomics dissociate

NOOO they stay tgt

2 things effecting force of attraction between ions

1) Charge of each ion

e.g O2- stronger than F- and less insoluble

2) bigger radii less strong

like AgCl is not soluble

Why don’t some ionic compound dissolve in H20

attraction between ions in compound is tooo strong

What can conductivity test indicate

• Only ionic compounds conduct electricity

• the dissociated ions carry charge

Miscible

Liquids that mix to form solution (water and alcohol)

Immiscible

Liquids that readily mix to form a solution like oil and h2o

sugar dissolve in h2o?

bc dispoles of sugar and h2o are stronger bc hydrogen bonding than dipoles of sugar with sugar

Why oil + water no mix

bc oils are long changes of fats/hydrocarbons with NP C-H and C-C bonds w no dipoles so they cannot interact with dipoles of H2O

Small Polar molecular compounds soluble?

YEs like CH3OH

Larger polar molecular compounds soluble in h2o? Butanol

No

Surfactant and Ex

Compound with NP (Hydrophobic) and P (hydrophilic) part like Sodium Stearate a detergent

Solubility

Max amount of solute that will dissolve in solvent at specific temp

Amount for Soluble

1g + dissolves in 100ml of solvent

Amount for insoluble

less than 1g dissolves in 100ml of solvent

Amount for Slightly Soluble

0.1g - 1g dissolves in 100ml of Solvent

Factors that affect solubility

Rate of dissolving - measure of time how quickly a solute dissolves

Thing you can do to speed up dissolving

Stir - Cause more collision and interaction

Heat - gives particles more kinetic energy for more collisions

Increase SA - Allows for more interaction

Unsaturated

More Solute can be dissolved - Below curve

Saturated

Contains max amount of solute

Supersaturated, Stability ?

Has more than max amount of solute
Unstable and will crystalize to remove excess solute if add a seed crystal

Like dissolves like true for gasses?

yess like HCL is polar and soluble in H2O whereas CO2 is NP and not soluble

Energy exchange between 2 gas or 2 liq

Very little energy exchange when forming a solution of two liq or gasses,

TEMP DOESNT EFFECT SOLUBILITY

Solubility of GASSES in LIquid

Vert effected by TEMP and PSI

Solubility curve of gasses in liquids

less Soluble as temp increases as they’ll have more kinetic energy e.g Coke loosing bubs

PSI effect on solubility of gasses in liquid

Its directly proportional to the psi pushing down gas

volumetric flask

To make liquid solution w Accurate volume when reach marked point

Volumetric pippet

Delivers single fixed volume very precicly

Graduated Pipette

delivers range of volume LESS accuracy

TIE

Second one seperating ions with charges and STATESSS

NIE

3rd, Removes spectator ions and keeps everything that has changed state, ADD CHARGES AND STATES

spectator ions

ions that are there must stay the same throughout reaction

Qualitative analysis

Identifying substances based off physcial or chemical characteristics
1. Precipitation reaction

2. Flame Test

   1. Color in solution

FID

Flame ionization Detector - passes samples into flame to determine metals present by light they give off

Quantitative Analysis

Determines how much of a substance is in a solution

4 Characterisitcs of acids

1. less than 7

2. conducts elec

3. sour

4. feels normal

4 Characterisitcs of bases

1. Ph = 7+

2. conducts elec

3. bitter

4. slipper

using the reactivity series, how do acids react with metals like Mg+ HCl

They can form H+ gass like —> MgCl + H2

Reaction of acids with carbonates

Ca(CO3) + 2HCl —>

—> CaCl + H2CO3 → CaCl + CO2 + H2O

name for x+1 O atoms for polyatomics

Per _ ate

name for x O atoms for polyatomics

_ate

name for x-1 O atoms for polyatomics

_ite

name for x-2 O atoms for polyatomics

Hypo_ite

How to name oxoacids

Per-ic
-ic

-ous

hypo-ous

Acid salt and naming

When an H+ in an acid is replaced with a cation e.g NaHSO4

sodium monohydrogen sulfate

How does base react w CO2, Ca(OH)2 + CO2 —>

—> CaCO3 + H2O, they form carbonates

Arrhenius main theory

Acids ionize in water to produce H+

Base dissociate to produce OH- as water pull its out

Ionization

forming ions in solution from uncharges molucules

Equation for autoionization of water

H2O+H2O—> H3O + OH-, happens very rarely

Arrhenius neutralization reaction

H+ + OH- —> H2O, all arrhenius neutralization reaction’s NIE can be written like this

problems with arrhenius’ theory

1) Limited to water solution

2) Doesnt explain how NH3 can be a base

3) H3O is not considered in dissociation or smth

Bronsted-Lowery theory

Acids donate H+

Base absorb H+

A, B, CB, CA

A after donating H+ = CB

B after receiving H+ = CA

pH equations

pH = -log[H+]

[H+] = 10^-pH

pH+ pOH = POH

What color does red limius paper turn in base

blue

What color does blue limius paper turn in acid

red

7 strong acids

HCl, HBr, HI,

H2SO4, HClO4,

HNO3

Strong acid

100% dissociation in water,

concentration of H+ is the concetration of acid

Weak acid and name 2

partially ionzaes in water like H2CO3, H3PO4

Strong base and name them

Dissociates completes in water

all group 1

all group 2 - release 2 moles of OH

Weak base and name 1

somewhat dissociates OH- Like NH3 + H2O —> NH4 + OH-

equimolar

equal moles relating to tritrations of strong acid and strong base when the indicator turns color, its neutral and moles=moles

Titration

exp to determine concentration of unkown acid or base along with an indicator

Titrant

solution with known concentration, often in burette bu

Equivience point

when neutralization is complete moles=moles

End point

When indicator turns color

Primary standard

reliable chem used in titration

Na2CO3 for aicd

KHP in base