Back to marketplace

Acid & Base: .5 + .6

No description yet. This curated deck is ready for daily study.

Total cards: 15•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (15)

#1
Front (Question)

Purpose of acid - base titrations

Back (Answer)

Determine the exact concentration of an acid or base

#2
Front (Question)

pH curve graph x and y axis

Back (Answer)

y = pH x = volume of titrant

#3
Front (Question)

What is an equivalence point?

Back (Answer)

The amount of acid exactly reacts with the base - no acid or base remain, only a salt and water. Moles H+ = moles OH-

#4
Front (Question)

The two types of the indicator and their pH range + colour change

Back (Answer)

Methyl Orange = acidic, red to yellow Phenolphthalein = alkaline, colourless to pink

#5
Front (Question)

Describe the the pH curve for a strong acid + strong base and indicator used

Back (Answer)

Initial pH: Very low (~1, strong acid). Rapid rise around pH 7 (equivalence point). Final pH: Very high (~13, strong base). Suitable indicators: Phenolphthalein or Methyl Orange

#6
Front (Question)

Describe the the pH curve for a strong acid + weak base and indicator used

Back (Answer)

Initial pH: Very low (~1, strong acid). Equivalence point: Below pH 7 (~5). Final pH: Moderate (~9 to 10, weak base). Suitable indicator: Methyl Orange.

#7
Front (Question)

Describe the the pH curve for a weak acid + strong base and indicator used

Back (Answer)

Initial pH: Moderate (~4, weak acid). Equivalence point: Above pH 7 (~9). Final pH: Very high (~13, strong base). Suitable indicator: Phenolphthalein.

#8
Front (Question)

Describe the the pH curve for a weak acid + weak base and indicator used

Back (Answer)

Initial pH: Moderate (~4, weak acid). No sharp pH change → No clear equivalence point. pH meter required (no suitable indicator).

#9
Front (Question)

What is a buffer solution

Back (Answer)

Maintains a relatively constant pH despite the addition of small amounts of acid or base.

#10
Front (Question)

What do acidic buffer solutions contain?

Back (Answer)

A weak acid and it’s respective salt

#11
Front (Question)

What do basic buffer solutions contain?

Back (Answer)

A weak base and it’s respective salt

#12
Front (Question)

Equilbrium in buffer solutions

Back (Answer)

HA (aq) ⇌ H+ (aq) + A- (aq)

#13
Front (Question)

Describe you would obtain the pH curve for the titration? [5]

Back (Answer)

Measure pH (of the acid) Add alkali in known small portions Stir mixture Measure pH (after each addition) Repeat until alkali in excess Add in smaller increments near endpoint

#14
Front (Question)

Concentraion of ions in a buffer solution and why

Back (Answer)

The concentration of HA and A− in the mixture must be much greater than the concentration of H+. This helps buffer changes.

#15
Front (Question)

How to work out the identity of an acid using the half equivalence point

Back (Answer)

[HA] = [A-] Ka = [H+] log(Ka) = -log[H+] pKa = pH Each acid has a specific pKa value