Acids and Bases

Question 1

H+ transfer reactions are

Answer 1

reversible

Question 2

Svante Arrhenius definition of acids/bases

Answer 2

an acid as a compound that dissolves in water to yield hydrogen cations (now recognized to be hydronium ions) and a base as a compound that dissolves in water to yield hydroxide anions.

Question 3

Brønsted-Lowry acid

Answer 3

A compound that donates a proton to another compound

Question 4

Brønsted-Lowry base

Answer 4

An acid-base reaction is, thus, the transfer of a proton from a donor (acid) to an acceptor (base).

Question 5

Acid base reaction in terms of proton donor/acceptor….

Answer 5

An acid-base reaction is, thus, the transfer of a proton from a donor (acid) to an acceptor (base).

Question 6

conjugate base

bc… talk abt reverse rxn

Answer 6

When an acid donates H+, the species that remains is called the conjugate base of the acid because it reacts as a proton acceptor in the reverse reaction

Question 7

conjugate acid

Answer 7

when a base accepts H+, it is converted to its conjugate acid

Question 8

acid ionization+ex with HF

Answer 8

The reaction between a Brønsted-Lowry acid and water to form hydronium ions is called acid ionization
For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:

Question 9

Base ionization

Answer 9

occurs when it accepts protons from water molecules. In the example below, pyridine molecules, C5NH5, undergo base ionization when dissolved in water, yielding hydroxide and pyridinium ions:

Question 10

acid and conjugate base relationship

Answer 10

Weaker the acid, stronger the conjugate base.

Question 11

amphiprotic

Answer 11

Species capable of either donating or accepting protons

Question 12

diff btwn bonsted lowery and arrhenius

Answer 12

bronsted: acid is proton doner

arrhenius: hydrogen

An Arrhenius acid increases hydrogen ion concentration.

Question 13

autoionization of water

kw

Answer 13

at 25 °C, Kw has a value of 1.0 10−14.

The process is endothermic, and so the extent of ionization and the resulting concentrations of hydronium ion and hydroxide ion increase with temperature.

Question 14

Kw
The Ion Product Constant of Water

what does it not include+when temp increase

Answer 14

the concentrations of solids and liquids are not included. Therefore, our expression for kw does not include the concentration of water, which is a pure liquid.

When temp increase the ph would be lower but same amount of oh and h ions. just bigger number concentration so when u multiply them for Kw you get larger KW.

Question 15

Therefore, the sum of pH and
pOH will always be 14 at

Answer 15

25 degrees for any aqueous solutions

this relationship will not hold true at other temperatures, because kw is temperature dependent!

Question 16

At 100°C, the pH of pure water is 6.14. That is the neutral point on the pH scale at this higher temperature. A solution with a pH of 7 at this temperature is …..bc…..

Answer 16

slightly alkaline because its pH is a bit higher than the neutral value of 6.14.

Question 17

Ph formula

Answer 17

Question 18

POH formula (2)

Answer 18

14-ph

Question 19

OH- concentration formula

Answer 19

Question 20

H3O+ concentration formula

Answer 20

10^-ph

Question 21

at 25 degrees relate ph and poh

Answer 21

Question 22

Since the autoionization constant Kw is——-, these correlations between pH values and the acidic/neutral/basic adjectives will be ——- at temperatures other than —.

Answer 22

temperature dependent

different

25 °C

Question 23

If neutral solution neutral solutions exhibit pH = pOH = 6.31

then what do acidic solutions and basic solutions exhibit in terms of PH and POH? Less than 6.31?????

Answer 23

acidic solutions exhibit pH less than 6.31 and pOH greater than 6.31, whereas basic solutions exhibit pH greater than 6.31 and pOH less than 6.31.

Question 24

acid-ionization constant, Ka+formula

the equilibrium constant for the ionization of an acid

Answer 24

Question 25

The larger the Ka

Answer 25

the larger the concentration of h3O+
and A− relative to the concentration of the nonionized acid, HA, in an equilibrium mixture, and the stronger the acid.

Question 26

A strong acid is strong when…. bc….

Answer 26

An acid is classified as “strong” when it undergoes complete ionization, in which case the concentration of HA is zero and the acid ionization constant is immeasurably large (Ka ≈ ∞).

Question 27

percent ionization

+quadratic or assumption rule

Answer 27

if percent ionization is less than 5% you can use approximation but if its larger you need quadractic equation

Question 28

The percent ionization of a weak acid

Answer 28

decreasing as concentration increases.

Question 29

base-ionization constant (Kb) in aqueous solutions

Answer 29

In solutions of the same concentration, stronger bases ionize to a greater extent, and so yield higher hydroxide ion concentrations than do weaker bases. A stronger base has a larger ionization constant than does a weaker base

Question 30

Ka, Kb, Kw relationship

Answer 30

Question 31

acid/base/conjugate partner relationship

Answer 31

the stronger the acid or base, the weaker its conjugate partner

Question 32

buffer

Answer 32

A solution containing appreciable amounts of a weak conjugate acid-base pair

resist changes when strong acid/bases are added

Question 33

pka

+smaller it is….
+what it says abt the acid
+formula

Answer 33

how willing an acid is to give up a proton
smaller pka the stronger the acid

= -logKa

Question 34

pka/pkb/pkw relationship

Answer 34

pKa+pKb=pKw=14

Question 35

pka back to ka

Answer 35

ka=10^-pka

Question 36

ph, pka and log formula that relates it all

Answer 36