Acid and Base (not yet done)

Reactivity 3.1.

State the characteristics of acids

• TASTE: sour

• REACTS WITH: metal

• PRODUCES: salt + H₂ gas

• FORMED FROM: nonmetal oxide + water

• pH<7

State the characteristics of bases

• TASTE: bitter

• TEXTURE: slippery

• FORMED FROM: metal oxide + water

• pH>7

State between what is neutralization.

acid_(aq) + base_(aq)

State the product of neutralization.

Salt_(aq)+H₂O_(l)

State the product of acid_(aq) + Metal_(s)

Salt_(aq) + H_2(g)

State the products of acid_(aq) + metal oxide_(s)

same products as neutralization

State the products of acid_(aq) + metal carbonate_(s)/ metal bicarbonate_(s)

Salt_(aq) + H₂O_(l) + CO_2(g)

Explain why acid_(aq) + metal oxide_(s) reactions produce the same products as neutralization.

• acid is aqueous meaning there is H₂O

• metal oxide + H₂O → basic solution_(aq)

• basic solution_(aq) + acid_(aq) = neutralization → salt_(aq)+H₂O

State what acids produce.

Hydrogen ion (H⁺)

State what bases produce.

Hydroxide ions (OH^-)

Describe strong acids and bases in terms of dissociation

full/ complete/ 100% dissociation

Describe weak acids and bases in terms of dissociation

partial dissociation

State what acids are always weak

organic acids

State a characteristic of organic acids

contain carboxylic group (COOH)

State what bases are always weak.

organic bases

State a characteristic of organic bases.

contain amine group (NH₂)

State the general form of strong bases

group 1 or group 2 + metal hydroxide

State the type of reaction in strong acids and bases

irreversible

State the type of reaction for weak acids and bases

reversible

State the three theories on acids and bases

• Arrhenius

• Brønsted Lowry

• Lewis

State the Arrhenius definition of acids.

Capable of producing H⁺ because it has Hydrogen

State the Arrhenius definition of base

Capable of producing OH^- because it has hydroxide

State why acids and bases are only in aqueous state.

Acids and bases only show their properties when dissolved.

State the standard Arrhenius acid dissociation equation.

HA → H⁺ + A^-

State the standard Arrhenius base dissociation equation

OHB → OH^- + B⁺

State how many hydrogen ions can be formed for one reaction

one

Define brønsted lowry acid

• proton donator (PDA)

• has hydrogen

Define Brønsted Lowry base

• proton acceptor

• has lone pair

State what is equal to H⁺

H₃O⁺

State the standard Brønsted Lowry equation

A + H₂O → A^- + H₃O⁺

B + H₂O → B⁺ + OH^-

State the property of water in terms of acids and bases.

Can be both acid and base

State an example of a Brønsted Lowry base but not an Arrhenius base

NH₃

State the rules of the Brønsted Lowry conjugate pairs

• opposite in acid or base

• opposite in strength

• differ by one proton

Define amphiprotic species

can be both Brønsted Lowry acid or Brønsted Lowry base

What type of acids can be amphiprotic

diprotic and polyprotic acids

Define diprotic acids

• can go through 2 dissociation processes

• have 2 hydrogen

• can produce 2 H⁺

Define polyprotic acids

• can go through at least 3 dissociation processes

• have at least 3 hydrogens

• can produce at least 3 H⁺

State 3 examples of amphiprotic species

• H₂O

• HCO₃^- (from the dissociation of H₂CO₃)

• CH₃C(COOH)₃ (carboxyl group can donate one hydrogen per OH group, therefore 3 in this case)

Describe amphoteric species

can be can be both lewis acids or lewis bases

Define lewis bases

lone pair donors

Define lewis acids

lone pair acceptors (L.A.A.)

State why species with incomplete octet rules are all lewis bases

have spare space to accept lone pairs

Describe and explain what happens when lewis acids are added to a brønsted lowry acid-base reaction.

• the species will react with OH^- and OH^- will be converted into a new product, reducing [OH^-]

• the species will react with the reactant, receiving the lone pair, and the reactant will be used up; OH^- will no longer be produced, pH will go back to its neutral state and remain constant

State an example of a lewis acid

BCl₃

State the characteristics of BCl₃

• accepts lone pairs

• cannot donate protons because it does not have any hydrogen

State the bond between lewis acids and bases

native covalent

State the needed condition when comparing the properties of strong/ weak acids/ bases

equal/ same initial concentration

Describe the relative electric conductivity of strong acids and bases

high

Describe the relative rate of the reaction between strong acids and metal/ metal carbonates

• reaction rate: fast

• rate of solid disappearance: fast

• rate of gas formation: fast

State what the conjugates’ strengths are relative to

Water’s ability to produce H⁺ or OH^- (the Kc of water, or Kw)

Predict the pH of Strong Acid + Strong Base

• pH = 7 at 25ºC because reaction is at

  • titration equivalence point

  • complete neutralization

Predict the pH of Strong Acid + Weak Base

acidic pH>7 at 25ºC

Predict the pH of Weak Acid + Strong Base

Basic pH<7 at 25ºC

Predict the pH of Weak Acid + Weak base

cannot be generalized

Define hydrolysis of salt

breaking down of salt or ionic compounds in water

State the objective of hydrolysis of salt

finding the pH of resulting solution

State the general form of hydrolysis of salt

Acid + Base → Salt + Water

State the different types of acid and base combinations in hydrolysis of salt.

• strong acid + strong base

• strong acid + weak base

• weak acid + strong base

• weak acid + weak base

State the pH of a solution from: strong acid + strong base at 25ºC

pH = 7

Explain the reason behind the pH of a solution from strong acid + strong base at 25ºC

weak conjugate acid and base ∴ solution pH = water pH

State the pH of a solution from: strong acid + weak base at 25ºC

pH > 7

Explain the reason behind the pH of a solution from strong acid + weak base at 25ºC

weak conjugate acid, strong conjugate base∴ solution pH > water pH

State the pH of a solution from: weak acid + strong base at 25ºC

pH < 7

Explain the reason behind the pH of a solution from weak acid + strong base at 25ºC

strong conjugate acid, weak conjugate base ∴ solution pH < Water pH

Explain the reason behind the pH of a solution from weak acid + weak base at 25ºC

Cannot be generalized (based on SL)

Explain the reason behind the pH of a solution from weak acid + weak base at 25ºC

strong conjugate acid, strong conjugate base ∴ solution pH is unknown (don’t know if acid is stronger than base)

Define pH

-log[H⁺]

Define pOH

-log[OH^-]

Define p(x)

-log(x)

Explain why px is used instead of [x] value

to simplify small numbers for easier communication

State the number of H⁺ ions produced for each strong acid dissociation

one

State number of OH^- ions produced when a strong ionic compound base dissociates

number of charge

State the formula for finding unknown concentration or volume of a new solution when number of mols is the same.

C₁V₁=C₂V₂

State K_w value

10^-14

State pK_w value

14

metal oxide + H2O

basic solution(aq)

nonmetal oxide + water

acidic solution