Week 5 Review

What is an aqueous solution?

What is an aqueous solution?

Solution where water is solvent.

Nonionic solutes - if compound is polar, solubility is ___ in water

high

Nonionic solutes - if compound is nonpolar, solubility is ___ in water

low

What happens with ionic solutes in water?

Dissolving forces of water is stronger than bonding forces of ionic solute, leading to dissolved ions

Arrhenius Acid

substance that prodcues H+ (H3O+) in water

Arrhenius Base

substance that produces OH- in water

Bronsted Acid

substance that donates H+ proton, reverse is conjugate base

Bronsted Base

substance that accepts H+ proton, reverse is conjugate acid

Label each reactant and product from left to right.

Base, Acid, Conjugate Acid, Conjugate Base

Lewis Acid

substance that accepts e pair

Lewis Base

substance that donates e pair

When are acids/bases defined by Lewis?

when describing reactions in nonaqueous environments

Is water acid or base?

Both, but weak.

Label each reactant and product from left to right.

Base, acid, conjugate acid, conjugate base

Kw=

Kw=[H+][OH-], 1.0x10^-14 at 25C

From top to bottom, identify the acidity or basicness of the solution.

neutral, acidic, basic

What is the relationship between bond strength and acid strength?

the stronger the bond, the weaker the acid

What conditions would make H+ break off and why?

If Z is very electronegative or in a high oxidation state. High electronegativity and oxidation state mean Z has a fuller valence, so H+ will not have a strong pull.

For oxoacids with different Z but same oxidation number and group, what is the relationship between acid strength and electronegativity?

the stronger the electronegativity, the stronger the acid strength

For oxoacids that have the same central atoms but different numbers of attached groups, what is the relationship between oxidation number of Z and acid strength?

HIgher oxidation of Z leads to more acid strength.

7 Strong Acids

HBr, HI, H2SO4, HNO3, HCl, HCLO4, HCLO3

Strong acids…

almost completely dissoves in water into H+ cations and anions

Weak acids…

partially dissolves in water into H+cations and anions, reaction will be reversible as there is both reactants and products coexisting

Strong Bases

almost completely dissolves into OH- anion and cations

Weak Bases

partially dissolve into OH- and cations, reaction is reversible because reactants and products coexist

conjugate acid-base pair relationship

the stronger the acid/base, the weaker its conjugate base/acid

What is Ka =, what is the trend?

Ka=[H+][A-]/[HA], high Ka is strong acid, small Ka is weak acid

What is Kb=, what is the trend? Remember to not include…

Kb=[NH4+][OH-]/[NH3], Kb is large for strong bases, small for weak, water