Acid & Bases

Question 1

Sorenson PH scale.

Answer 1

Question 2

Ka for acids and bases

Answer 2

Question 3

Pka for acids and bases

Answer 3

Question 4

PH of weak acids

Answer 4

Question 5

titrations

Question 6

Arrhenius definition of acid

Answer 6

acids are proton (H+) acceptors
bases hydroxyl ion (OH-) donors

HCL is acid in water but not in benzene (as it is not an aqeous environment)
ammonia (NH3) is a base with no hydroxyl group

Question 7

Bronsted lowry definition

Answer 7

acid proton donor
base proton acceptor

HCL not ionised in benzene as does not accept proton

definition works with some non aqueous solutions like ethanol but is less good in aprotic solvents.

Question 8

lewis definition

Answer 8

more general
lewis acid - electron pair acceptor
lewis base - electron pair donor

all bronsted lowry acids are lewis acids but not vice versa.

lewis definition metal cations are acids
group three elements are acids accordng to lewis.

Question 9

how to determine strong/weak acid

Answer 9

strong acids: ↑ka value as [HA] is low and [A-] ↑
pKa most common way to measure strength
pKa = -log[Ka]
strong acids have a low Ka

Question 10

how to determine strong/weak base

Answer 10

strong bases = ↑kb as [B] is low and [BH+]↑
pKa used to measure strength of base but by measuring the strength of its conjugate acid.
stronger base: weaker conjugate acid
low Ka
↑pKa