Chemistry - Chapter 19 Flashcards by Hannah Griffis

conjugate acid

the ion or molecule formed when a base gains a hydrogen ion

How well did you know this?

Not at all

Perfectly

conjugate base

the ion or molecule that remains after an acid loses a hydrogen ion

How well did you know this?

Not at all

Perfectly

conjugate acid-base pair

consists of two ions or molecules related by the loss or gain of one hydrogen ion

How well did you know this?

Not at all

Perfectly

amphoteric

give an example

a substance that can act as either an acid or a base

ex. HCl = water accepts a proton –> base

NH4 = water donates a proton –> acid

How well did you know this?

Not at all

Perfectly

hydronium ion

(H3O) the positive ion formed when a water molecule gains a hydrogen ion

How well did you know this?

Not at all

Perfectly

Bronsted Lowry Theory

where an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor

How well did you know this?

Not at all

Perfectly

self-ionization

a term describing the reaction in which two water molecules react to produce ions

How well did you know this?

Not at all

Perfectly

neutral solution

what is the pH of this solution?

an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal

has a pH of 7.0

How well did you know this?

Not at all

Perfectly

ion-product constant for water

(Kw) the product of the concentrations of the hydrogen ions and hydroxide ions in water

it is 1 x 10^-14 at 25°C

How well did you know this?

Not at all

Perfectly

acidic solution

any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration

How well did you know this?

Not at all

Perfectly

basic solution

any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration

How well did you know this?

Not at all

Perfectly

number used to denote the hydrogen-ion concentration, or acidity, of a solution

-log[H+] = pH

How well did you know this?

Not at all

Perfectly

strong acid

an acid that is completely (or almost completely) ionized in an aqueous solution

How well did you know this?

Not at all

Perfectly

weak acid

an acid that’s only slightly ionized in an aqueous solution

How well did you know this?

Not at all

Perfectly

acid dissociation constant

(Ka) the ratio of the concentration of the dissociated form of an acid to the undissociated form

stronger acids have larger Ka values than weaker acids

How well did you know this?

Not at all

Perfectly

strong base

a base that completely dissociates into metal ions and hydroxide ions in aqueous solutions

How well did you know this?

Not at all

Perfectly

weak base

a base that reacts with water to form the hydroxide ion and the conjugate acid of the base

How well did you know this?

Not at all

Perfectly

base dissociation constant

(Kb) the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base

neutralization reaction

a reaction in which an acid and a base react tin an aqueous solution to produce a salt and water

titration

process used to determine the concentration of a solution (often an acid or base) in which a solution of known concentration (the standard) is added to a measured amount of the solution of unknown concentration until an indicator signals the end point

standard solution

a solution of known concentration used in carrying out a titration

equivalence point

the point in a titration where the number of moles of hydrogen-ions equals the number of moles of hydroxide ions

end point

the point in titration at which the indicator changes color

List 3 rate of reaction factors:

Temperature

Concentration

Catalyst

What is the equilibrium-constant equation?

Keq = [D^d} [C^c} / [B^b] [A^a}

Arrhenius's definition of acids and bases? (2)

acids are hydrogen containing compounds that ionize to yield hydrogen ions in aqueous solutions bases are compounds that ionize to yield hydroxide ions in aqueous solutions

What is Le Chatelier's Principle?

if a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress

How are [H+] and [OH-] related in an aqueous solution?

the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals 1.0 x 10^-14 ** ion-product constant for water (Kw)

Equation to find the ion-product constant for water (Kw)

Kw = [H+] x [OH-] = 1.0 x 10^-14

Properties of water molecules (5)

highly polar constantly in motion +1 H2O molecule = H3O -1 H2O molecule = [OH-] Concentration of [H+] and [OH-] ions = 1.0 x 10^-7 M in pure water @ 25°C

What is the direction of the shift in equilibrium with the addition or loss of water

The equilibrium shifts towards the formation of water [H+] ^ = v [OH-]

What can possibly change when finding the ion-product constant for water? (Kw) What definitely won't change?

Concentrations may change Product stays the same

basic solutions are also called...?

alkaline solutions

How do you calculate the acid dissociation constant (Ka)?

Ka = [H+][A-] / [HA] *equilibrium concentrations found with equilibrium constant formula

How do you calculate the base dissociation constant (Kb)?

Kb = [conjugate acid] x [OH-] / [base] *equilibrium concentrations found with equilibrium constant formula

what do the words concentrated and dilute indicate? what do they refer to?

they indicate how much of an acid or base is dissolved in solution the number of moles of the acid or base in a given volume

how to find the pH of a substance?

pH = -log[H+]

how to find the [H+] of a substance? (when pH is not a whole number)

[H+] = 10^-pH (antilog)

low pH = high pH =

more acidic more basic

what is pH often measured with? (2)

acid-base indicators or a pH meter

how to find [OH-]? how to find pOH?

[OH-] = 10^-pOH pOH = -log v10[OH-]

Since [H+][OH-] = 1.0x10-14.... ?

pH + pOH = 14 (@25°C)

at what point in a titration does neutralization occur?

when the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions

define salts

ionic compounds consisting of an anion (-) from an acid and a cation (+) from a base