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Chemistry > Acids And Bases > Flashcards

Acids And Bases Flashcards

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1
Q

Define acid (Arrhenius theory)

A

A neutral molecule which dissociates in water to form a hydrogen ion and an anion

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2
Q

Define base (Arrhenius theory)

A

Dissociates in water to form a hydroxide ion and a cation

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3
Q

Strong acids and bases(Arrhenius)

A

Dissociates fully in aqueous solutions

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4
Q

Weak acids and bases (Arrhenius)

A

Only dissociates slightly in aqueous solution

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5
Q

Conductivity of weak acids(Arrhenius)

A

Weak acids conduct poorly because few ions

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6
Q

Conductivity of strong acids

A

Strong acids conduct well because there are numerous ions

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7
Q

Limitations of Arrhenius theory

A

Limited due to dilute aqueous solutions and has been superseded/ amphoteric substance not explained (water not amphoteric)

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8
Q

Acid (Bronsted-Lowry theory)

A

Acid is a proton donor

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9
Q

Base ( Bronsted-Lowry theory)

A

Base is a proton acceptor

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10
Q

Strength of acids(Bronsted-Lowry)

A

Stronger acids more readily donates a proton

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11
Q

Conjugate acid-base pairs

A

Species that differ from each other by H+

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12
Q

The strength of an acid if it’s conjugate base is weak

A

The stronger the acid the weaker the conjugate base

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13
Q

Indicator

A

Substances that changes colour with pH or at the end-point of a titration

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14
Q

Define Conjugate acid

A

Produced by a gain of one h+

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15
Q

Amphoteric

A

It can act as both a Brønsted-Lowry acid and a Bronsted-Lowry based.

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16
Q

Neutralisation

A

the reaction betweem acid and a base to form salt and water.

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17
Q

Alkali

A

a base that is soluble in water.

18
Q

Mono basic acids

A

Produces one H+ ion in solution

19
Q

Dibasic acids

A

Produces two H+ ions in solution

20
Q

Tribasic acids

A

Produces three H+ ions in solution

21
Q

Dissociation

A

When acids are places in solutions they split up into their ions, hydrogens ions and anions

22
Q

Salts

A

Formed when the H+ of the acid is replaces by a metal ion

23
Q

Limitation of ph scale

A

Accurate only for dilute solutions

24
Q

pH

A

-log10[H+]

25
Q

How to test sample of mineral water for presence of the sulfate ion

A

Add barium chloride( BaCI2) / white insoluble in HCI remains after addition of HCI when sulfer present

26
Q

Explain the term standardised

A

Concentration found by another titration

27
Q

State a precaution when end point in sight

A

Add drop by drop, swirl conical flask and wash down sides of conical flask.

28
Q

Describe how the liquid level in burette was adjusted to zero mark.

A

Fill above mark and adjust slowly with tap

29
Q

Name a primary standard reagent to standardise the HI solution?

A

Anhydrous sodium carbonate (Na2COs)

30
Q

Why is sodium carbonate a primary standard yet sodium carbonate crystals are not?

A

Sodium carbonate is anhydrous where as sodium carbonate crystals are hydrated. Primary
standards are anhydrous

31
Q

Why is it necessary to dilute vinegar?

A

To prevent excess amount of sodium hydroxide being used

32
Q

Purpose of white tile?

A

To see colour change more clearly.

33
Q

Purpose of swirling conical flask?

A

To ensure mixing of chemicals

34
Q

What are the two purposes of Sulfuric acid

A
  1. To prevent oxidation of Fe2+ to Fe3+

2. To ensure an acidic medium to reduce Mn0+-

35
Q

Why is there never an indicator when potassium permanganate is used?

A

Potassium permanganate is its own indicator

36
Q

How is iodine brought into aqueous solution?

A

By reacting iodine with potassium iodide we form potassium triiodide which when dissolved in water simply forms triiodide (soluble).

37
Q

Why is excess potassium iodide used?

A

Anything “excess” is to ensure all of reactant has reacted/ also to keep iodine in solution.

38
Q

What indicator is used for sodium thiosulfate?

A

Starch. It is added when pale yellow colour formed. Goes blue-black to colourless

39
Q

Why is distilled water better than deionised water for experiments?

A

Distilled water contains no chlorine oxidising agents. It is purer than deionised water.

40
Q

Name a primary standard reagent used to standardise potassium permanganate?

A

Ammonium iron (Il) sulphate.

Chemistry (19 decks)

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