Chapter 18: Acids and Bases
Base ionization constant
(Kb) the value of the equilibrium constant expression for the ionization of a base
ion product constant for water
(Kw) equals the product of the H+ ion concentration and the OH- ion concentration
conjugate acid
A _____ is produced when a base accepts a hydrogen ion from an acid.
neutral
A ________ solution has a pH of 7 and a pOH of 7 because the concentrations of hydrogen ions and hydroxide ions are equal
Bronsted-Lowry
A __________ acid is a hydrogen ion donor. A__________ base is a hydrogen ion acceptor
acid
A base that accepts a H+ ion becomes an _______ because it then has an extra H+ ion that it can donate
hydroxide
A basic solution contains more _____ ions than hydrogen ions.
weak
A strong acid has a _______ conjugate base. A strong base has a ________ conjugate acid. (so does not go into equilibrium)
strong
A weak acid has a _______ conjugate base. A weak base has a _______ conjugate acid. (leans to the left so in equilibrium)
Arrhenius
An ________ acid must contain an ionizable hydrogen atom. An ________ base must contain an ionizable hydroxide group.
monoprotic
An acid that can donate only one hydrogen ion is called a _____ acid.
base
An acid that donates an ion becomes a _______ because it has a negative charge and can readily accept a positive hydrogen ion
weak
Equilibrium arrows are used for _____ acids and bases (only partly ionized in water and in equilibrium)
strong
For all _________ monoprotic bases, the concentration of the base is the concentration of the OH- ions
strong
For all __________ monoprotic acids, the concentration of the acid is the concentration of the H+ ions
equivalence point
It is important to choose an indicator for a titration that will change color at the _________ ___________ of the titration
conjugate base
The _____ of a weak acid is strong.
weakest
The _________ acids have the smallest Ka values because their solutions have the lowest concentrations of ions and the highest concentrations of un-ionized acid molecules
concentrations
The ______________ of hydrogen ions and hydroxide ions determine whether an aqueous solution is acidic, basic, or neutral
partially
Weak acids and weak bases are only _________ ionized, so you must use Ka and Kb values to determine the concentrations of the H+ and OH- ions in solutions of weak acids and bases
hydrogen
When acids react with metals, they produce _____ gas.
titration
You can use _______ to calculate the concentration of a solution by figuring out the number of moles of acid/base, then use the balanced equation to calculate moles of acid/base present, and then use the volume of acid/base added that neutralized the reaction to calculate the concentration
Arrhenius
______ theory classifies certain compounds as acids or bases based on what kind of ions formed when the compound was added to water (H+ or OH-)
weak
________ acids produce an equilibrium mixture of molecules and ions in an aqueous solution
indicators
_________ change color depending on the concentration of hydrogen ions in a solution
Strong base
a base that dissociates entirely into metal ions and hydroxide ions
strong base
a base that dissociates entirely into metal ions and hydroxide ions in aqueous solution
Weak base
a base that ionizes only partially in dilute aqueous solution
weak base
a base that ionizes only partially in dilute aqueous solution to form the conjugate acid of the base and hydroxide ion
pH meter
a device that measures the pH of a solution (usually during titration). Measures H+ ion activity in a solution. (measures the exact pH of a solution)
Lewis model
a lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor
Titration
a method for determining the concentration of a solution by reacting a known volume of that solution with a solution of known concentration
Bronsted-Lowry model
a model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor
Arrhenius model
a model of acids and bases; states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution and a base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution
Bronsted-Lowry base
a proton (hydrogen ion) acceptor
Neutralization reaction
a reaction in which an acid and a base in an aqueous solution react to produce a salt and water
neutralization reaction
a reaction in which an acid and a base react to form water and a salt and involves the combination of H+ and OH- ions to generate water. (turns pH to =7). (when an acid and base react and completely neutralize each other).
neutral solution
a solution that has equal concentrations of hydrogen and hydroxide ions (pH=7)
Bronsted-Lowry acid
a species that is a proton (hydrogen ion) donor
amphoteric
a substance that can act as both an acid and a base
H3O+
a water molecule that gains a hydrogen ion becomes _________
OH-
a water molecule that loses a hydrogen ion becomes _______
pH
acid strength and concentration (amount the acid dissociates, concentration sometimes doesn't have an effect based on acid strength) determine...
Diprotic acids
acids that contain two ionizable hydrogen atoms per molecule
Strong acids
acids that ionize completely. (single arrow in the ionization equation because reaction goes to completion→ completely ionizes)
Triprotic acids
acids with three hydrogen ions to donate
hydrogen ions and hydroxide ions
all water solutions contain...
Bronsted-Lowry model (of acids and bases)
an acid is a hydrogen-ion donor, and a base is a hydrogen-ion acceptor
Monoprotic acid
an acid that can donate only one hydrogen ion
monoprotic acid
an acid that donates only one proton of hydrogen atom per molecule to an aqueous solution
strong acid
an acid that ionizes completely in aqueous solution
Weak acid
an acid that ionizes only partially in dilute aqueous solution
weak acid
an acid that ionizes only partially in dilute aqueous solution
triprotic acid
an acid that is capable of donating three protons or hydrogen atoms per molecule when dissociating in aqueous solutions
diprotic acid
an acid that is capable of donating two protons or hydrogen atoms per molecule when dissociating in aqueous solutions
Polyprotic acid
any acid that has more than one ionizable hydrogen atom
Acid-base indicators
chemical dyes whose colors are affected by acidic and basic solutions. Used for titration; are weak acids.
Conjugate acid-base pair
consists of two substances related to each other by the donating and accepting of a single hydrogen ion
conjugate acid-base pair
consists of two substances related to each other by the donating and accepting of a single hydrogen ion
neutral solution
contains equal concentrations of hydrogen ions and hydroxide ions
acidic solution
contains more hydrogen ions than hydroxide ions
basic solution
contains more hydroxide ions than hydrogen ions
amphoteric
describes water and other substances that can act as both acids and bases
increase
for every factor of 10 ______ of [H+], pH will decrease by 1 unit, and vice versa
decrease
if the concentration of H+ ions increases, the concentration of OH- ions must __________, and vice versa
self-ionization
in this process, water molecules react to form a hydronium ion and a hydroxide ion
pOH
negative logarithm of the hydroxide ion concentration
water molecules, hydronium ions, and hydroxide ions.
pure water contains...
strong
single arrows are used for ____ acids (completely ionized)
Arrhenius model
states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution, and states that a base is a substance that contains a hydroxide group and dissociates to produce hydroxide in aqueous solution (useful for explaining many acidic and basic solutions, but not all bases are included )
completely
strong acids and bases ionize ______ in aqueous solution, while weak acids and bases ionize only partially
acid-base indicator
substance which changes color with pH. Use to determine if a substance is an acid or a base, and to perform titrations
neutral
substance with equal values of [H+] and [OH-]
acidic
substance with high [H+] and low [OH-]
basic
substance with low [H+] and high [OH-]
characteristics of bases
taste bitter and feel slippery, ability to conduct electricity, turn litmus paper blue
characteristics of acids
taste sour, ability to conduct electricity, react with metals and metal carbonates, turn litmus paper red, reactions with metals produce Hydrogen gas, reactions with metal carbonates and hydrogen carbonates produce carbon dioxide gas
lower
the _____ the pH value, the more acidic the solution, and the higher the concentration of H+
higher
the _____ the pH value, the more basic the solution, and the lower the concentration of H+
10^-7 M
the concentration of OH- ions in pure water
pH
the negative logarithm of the hydrogen ion concentration (how chemists express the concentration of hydrogen ions)
pH
the negative logarithm of the hydrogen ion concentration of a solution; acidic solutions have pH values between 0 and 7, basic solutions have values between 7 and 14, and a solution with a pH of 7 is neutral
pOH
the negative logarithm of the hydroxide ion concentration of a solution; a solution with a pOH above 7 is acidic, a solution with a pOH below 7 is basic, and a solution with a pOH of 7 is neutral
End point (of the titration)
the point at which the indicator used in a titration changes color
water and salt
the products of an acid base reaction (two)
negative inverse (by a factor of 10)
the relationship between [H+] and pH is...
hydrogen ions and hydroxide ions
the relative amounts of ______________ ______ ___________ determines whether a solution is acidic, basic, or neutral
conjugate acid
the species formed after a base accepts a proton
conjugate base
the species formed after an acid donates a proton
Conjugate acid
the species produced when a base accepts a hydrogen ion
conjugate acid
the species produced when a base accepts a hydrogen ion from an acid
conjugate base
the species produced when an acid donates a hydrogen ion to a base
Conjugate base
the species that results when an acid donates a hydrogen ion
base ionization constant
the value of the equilibrium constant expression for the ionization of a base
acid ionization constant
the value of the equilibrium constant expression for the ionization of a weak acid
Acid ionization constant
the value of the equilibrium constant expression for the ionization of a weak acid.
Ion product constant for water
the value of the equilibrium constant expression for the self-ionization of water
ion product constant for water
the value of the equilibrium constant expression for the self-ionization of water
Arrhenius acid
this acid is defined as any species that increases the concentration of H+ ions in an aqueous solution
Arrhenius base
this base is defined as any species that increases the concentration of OH- ions in an aqueous solution
(characteristics of an) acid
this substance increases the concentration of H+ ions in an aqueous solution, are proton (H+ ion) donors, sour, react with metals, turns litmus paper red, and have a pH less than 7
(characteristics of a) base
this substance increases the concentration of OH- in an aqueous solution, are proton (H+ ion) acceptors, bitter, slippery, turns litmus paper blue, and has a pH greater than 7.
conjugate acid-base pair
two species in a conjugate acid-base pair that have the same molecular formula except the acid has an extra H+ compared to the conjugate base
Amphoteric
water and other substances that can act as both acids and bases
to add an indicator
what you must never forget when doing a titration
base
you know that a substance is a _______ when the compound contains OH-, CO3-2, or HCO3- ions
acid
you know that a substance is an _________ when it has an hydrogen atom in the compound (or has basic form of HX, or HXO)
