Acid, Bases, and Salts Test

Hydronium Ion

Instead, a species called the hydronium ion, H3O+, forms when the dissociated H+ ion combines with a water molecule, H2O.

Conjugate Acid

A conjugate acid is the ion or molecule formed when a base gains a hydrogen ion.

Conjugate Base

A conjugate base is the ion or molecule that remains after an acid donates a hydrogen ion.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two ions or molecules related by the loss or gain of one hydrogen ion.

Lewis Base

A Lewis Base is a substance that donates a pair of electrons to form a covalent bond

Lewis Acid

A Lewis acid is a substance that accepts a pair electrons to form a covalent bond.

Neutral solutions

Any aqueous solution in which [H3O*] and [OH-] are equal is a neutral solution.

Ion-Product constant for water

In water or aqueous solutions at 25°C, the product of the hydronium-ion concentration and the hydroxide-ion concentration, known as the ion-product constant for water (Ku), equals 1.0 × 10^-14.

Kw = [H30+]x[OH] = 1.0 × 10-14

Thus, every unit decrease in ph corresponds to a tenfold increase in [H3O+].

True

Neutralization Reaction

A reaction in which an acid and a base in an aqueous solution produce a salt and water is called a neutralization reaction.

Acid + Base → Salt + Water

HCI(ag) + KOH(aq) → KCI(aq) + H2O(L)

Salt Hydrolysis

Salt hydrolysis is a process in which the cations or anions of a dissociated salt accept hydrogen ions from water or donate hydrogen ions to water.

Titration

An important method for investigating the interactions of acids and base is a titration, in which a volume of a solution of known concentration is added to a solution of known volume but unknown concentration.

Equivalence Point

Neutralization occurs when the numbers of moles of H3O+ and OH- are equal, and the point in a titration where neutralization occurs is called the equivalence point.

Titration Curve

The graph of the unknown solution's pH versus the volume of standard solution added during a titration is called a titration curve.

Buffer

A solution in which pH remains relatively constant when small amounts of acid or base are added is called a buffer.

Buffer Capacity

Buffer capacity is a measure of the amount of acid or base that may be added to a buffer system before a significant change in ph happens.

Buffer Range

Buffer range is the overall ph range in which a buffer system is effective at maintaining a relatively constant pH.

Arrhenius

Acid is H3O+ ion donor(if has H3O-, is an acid)

Base is an OH- donor( if has OH, it’s a base)

Bronsted Lowry

Acids are hydrogen donors.

Bases are hydrogen ion acceptors- one exception: Ammonia

NH3(Base)+H=NH4(Acid)

Lewis

Acids are electron pair acceptors.

Bases are electron pair donors.

Above midpoint

Base

Below midpoint

Acid

Mid point

Neutral