1Aqueous Reactions Acid/Base Reactions

What types of reaction are acid base reactions (3)

double-replacement

aqueous

neutralization

What are acid-base reactions considered to be

one of the most fundamental, yet most important, reactions in chemistry

List examples of how acids and bases are ubiquitous

found in foods (vinegar,lemons)

cleaning supplies (sodium hydroxide and ammonia)

cooking (break down proteins)

critical biological roles (proteins and DNA)

what do aqueous reactions involve

water as a reactant or product and as the solvent

What are various definitions used for

to identify species as acids and bases

List 5 example of biological relevance of acid-base reactions

amino acid coupling (protein synthesis)

protein denaturation (digestion)

ester synthesis (fragrances)

antibiotics (synthesis and the mechanism of activity)

innumerable additional synthetic applications

What is the acid-base definition of arrhenius

Acid is H+

Base is HO-

What is the acid-base definition of Bronsted-Lowry

Acid is an H+ donor

Base is an H+ acceptor

What is the acid-base definition of Lewis

Acid is an electron pair acceptor

Base is an electron pair donor

For Bronsted-lowry acids, how do acidic solutions form

upon ionization of certain hydrogen-containing molecules in H₂O

H+ being a proton makes it strongly attracted to what

H2O

H+ (aq) is more accurately written as what and is called?

H₃O⁺

hydronium ion or solvated proton

H₃O is one of many?

forms the solvated protons can take

What may protons associate with

multiple water molecules

List 3 other forms of the solvated proton

H₅O₂⁺, H₇O₃⁺, H₉O₄⁺

What will we strictly use to represent the proton in an aqueous solution

H₃O⁺

What are strong acids and strong bases also strong?

strong electrolytes

What do strong acids feature easily

broken Hydrogen-Nonmetal bonds

What do strong acids feature faciliate

H+ transfer

How do strong acids ease the loss of H+

polarized bonds and long bond lengths

Describe the relationship between losing a proton and the strength of an acid

the stronger the acid, the easier it is to lose a proton

How do strong acids react when they come in contact in an aqueous solution

ionize completely

Give an example of bond length and acid

HF (hydrofluoric) vs. HI (Hydriodic) acids

I is much larger then F; the bond is longer and easier to break

Name some common strong bases

metal hydroxides

Name some weak bases

nitrogen compounds such as ammonia (NH₃) and amines, compounds containing -NH₂ 

What happens when strong bases come in contact in an aqueous solution

ionized completely

Explain how weak bases interact with water

very little and ionize to a small extent

What are the typical groups that represent strong inorganic bases

group 1 and 2 metal hydroxides

How do strong inorganic bases react when they come in contact in an aqueous solution

ionize completely

Why do we have to be careful with the formula including strong inorganic bases

may produce multiple equivalents of hydroxide per mole ionized

Explain what it means to be weak electrolytes

weak acids/bases that do not completely ionize in solution

What can be calculated with effort with concentration of ions

the concentrations of species in solutions of weak acids/bases

For strong acids and bases, what concentrations are more readily determined

the concentrations of hydronium and hydroxide

What else does the stated molar concentration of the acid/ base represent

it is also the concentration of hydronium/hydroxide (for
hydroxide, this is true for Group I metal hydroxides)