8. Acids & Bases Flashcards
What is a Bronsted-Lowry base?
Proton acceptor
What is a Bronsted-Lowry acid?
A proton donor
What is an amphiprotic species?
Can act as both a base and acid.
What is a conjugate acid-base pair?
A pair of species differing by a single proton.
acid + metal -> ?
salt + hydrogen
acid + base -> ?
salt + water
acid + metal carbonate/metal hydrogen carbonate -> ?
salt + carbon dioxide + water
pH= ?
-log[H+]
[H+]= ?
10^-pH
Kw = ?
[H+][OH-] = 10^-14
ammonia + water –> ?
ammonium + water
C1V1= ?
C2V2
What is the difference between a Lewis acid and a Bronsted-Lowry acid?
A Lewis acid is a species that can accept an electron pair.
A Brønsted–Lowry acid is a species that can donate a proton (H⁺)
Give four examples of Lewis acids.
BF₃, AlCl₃, Fe³⁺, H⁺
Give three examples of Bronsted-Lowry acids.
HCl, H₂SO₄, NH₄⁺
How would you work out whether an acid is strong or weak given its pH and concentration?
Work out the pH using the concentration given.
If this pH is lower than the pH given, then the acid is weak as it has not fully dissociated.
What is the difference between a base and an alkali?
A base is a substance that can neutralise an acid.
An alkali is a soluble base that produces OH− ions in solution.
What is the ionic equation for a neutralisation reaction?
H+ + OH− → H2O
What is the difference in the type of arrow used to show the dissociation of a weak acid compared to a strong acid?
Weak acid will have a reversible arrow, whereas a strong acid will have a single arrow.
What does a small value of pKa mean?
The acid is strong
pKa= ?
-log10Ka
Ka= ?
10^-pKa
