Acids

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

Give the definition of an acid

Back (Answer)

Acid – A compound that dissolves in water to produce hydrogen ions (H+)

Front (Question)

Give the definition of a base

Back (Answer)

Base – A substance that reacts with acid producing a salt and water.

Front (Question)

Give the definition of an alkali

Back (Answer)

Alkali – Soluble bases which dissolve in water to produce hydroxide ions OH-

Front (Question)

Give the definition of neutralisation

Back (Answer)

Neutralisation - H+ (aq) + OH-(aq) -> H2O(l)

Front (Question)

Give the definition of monoprotic

Back (Answer)

Monoprotic – 1 mole of acid produces 1 mole of H+ ions.

Front (Question)

Give the definition of diprotic

Back (Answer)

Diprotic – 1 mole of acid produces 2 moles of H+ ions.

Front (Question)

Give the definition of a Hydonium ion or hydroxonium ion or oxonium ion.

Back (Answer)

Hydonium ion or hydroxonium ion or oxonium ion – H3O+. It is the ion formed when acids react with water.

Front (Question)

Give the definition of a buffer

Back (Answer)

Buffer – solutions that can resist changes in pH when small quantities of acid or base are added.

Front (Question)

Give the definition of a Bronsted-Lowry acid

Back (Answer)

A Bronsted-Lowry acid is a proton donor.

#10

Front (Question)

Give the definition of a Bronsted-Lowry base

Back (Answer)

A Bronsted-Lowry base is a proton acceptor.

#11

Front (Question)

What happens to strong bases in aqueous solution?

Back (Answer)

Strong acids (HCl, H2SO4, HNO3) and bases (NaOH, KOH) completely dissociate in aqueous solution.

#12

Front (Question)

What happens to weak bases in aqueous solution?

Back (Answer)

Weak acids and bases are slightly dissociated in aqueous solution.

#13

Front (Question)

How do you calculate the new concentration of a solution?

Back (Answer)

New concentration of a solution = amount in moles of

#14

Front (Question)

What is the equation for pH?

Back (Answer)

pH = -log10[H+]

#15

Front (Question)

What is the equation for [H+]?

Back (Answer)

[H+] = 10(-pH)

#16

Front (Question)

What is the equation for Kw?

Back (Answer)

Kw=[H+] [OH-] units mol2dm-6

#17

Front (Question)

At 25oC what does Kw equal?

Back (Answer)

At 25oC Kw = 1.00 x 10-14

#18

Front (Question)

In pure water how would you calculate [H+]?

Back (Answer)

In pure water [H+] = √Kw

#19

Front (Question)

What is the equation for pKw?

Back (Answer)

pKw = -log10Kw (14 at 25oC)

#20

Front (Question)

What is the equation for pOH?

Back (Answer)

pOH = log10 [OH-]

#21

Front (Question)

What is the link between pOH and pH?

Back (Answer)

pOH + pH = pKw

#22

Front (Question)

Give the equilibrium equation for the dissociation of HA.

Back (Answer)

HA H+ + A-

#23

Front (Question)

What is the equation for Ka?

Back (Answer)

Ka = [A-] [H+] /[HA]

#24

Front (Question)

What is the equation for pKa?

Back (Answer)

pKa = -log10[Ka]