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Chemistry Grade 11 > Acids And Bases > Flashcards

Acids And Bases Flashcards

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1
Q

Arrhenius’ theory

A

Acids form H³O+ (ionise in water to form H+. Ions can not exist on their own, so they form H³O+)
Bases form OH‐ (dissociate in water to form OH‐)

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2
Q

Lowry-Bronsted’s theory

A

Acids are proton donors (H+)
Bases are proton acceptors (H+)

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3
Q

Definition of an ampholyte

A

Any substance that can act as either an acid or base

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4
Q

Definition of a conjugate acid-base pair

A

Compounds that differ from each other by the presence of H+

(A substance will always be paired with the product it forms)

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5
Q

Describe acids

A
  • sour to the taste
  • cause specific colour changes in indicators and plant dyes (litmus = blue to red)
  • aqueous acid solutions conduct electricity
  • neutralize bases
  • have at least 1 H atom that can ionise to form an ion (H+) in an aqueous solution
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6
Q

Describe bases

A
  • alkali = base that is soluble in water
  • bitter to taste, soapy to touch (alkali reacts with oils on skin to form soap)
  • cause colour changes in indicators and plant dyes (litmus = red to blue)
  • alkaline solutions conduct electricity
  • neutralize acids
  • produce hydroxide ions (OH‐) in aqueous solution
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7
Q

Reaction of acid and metal

A

Produce a salt and H² gas

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8
Q

Reaction of acid and oxide

A

Produce a salt and H²O

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9
Q

Reaction of acid and hydroxide

A

Produce a salt and H²O

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10
Q

Reaction of acid and metal carbonate

A

Produce a salt, H²O and CO²

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11
Q

Definition of an indicator

A

A weak organic dye that changes colours at definite pH values

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12
Q

What does a salt contain?

A
  • a cation from the base
  • an anion from the acid
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13
Q

How do you find the base in an acid-base reaction?

A

Combine the cation with O‐², OH‐ , CO³-²

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14
Q

How do you find an acid in an acid-base reaction?

A

Combine the anion with H+

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15
Q

List 5 examples of indicators

A
  • methyl orange
  • methyl red
  • bromthymol blue
  • neutral red
  • phenolphthalein
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16
Q

Formula to determine the pH of an acid

A

pH = -log [H³O+]

17
Q

Steps to determine the pH

A
  1. Balance reaction of acid with water
  2. Use molar ratio to determine the concentration of H³O+ molecules
  3. Plug in and solve
18
Q

What does Kc mean?

A

Equilibrium constant

19
Q

Formula of the equilibrium constant

A

Kc = [product concentration] ÷ [reactant concentration]

20
Q

What is the concentration of solids and pure liquids?

A

One

21
Q

Equilibrium constant of water

A

Kw = 1×10‐¹⁴ (at room temperature)

22
Q

Equilibrium constant of a neutral solution

A

[H³O+] = [OH‐] = 1×10‐7

23
Q

Ka value of a strong acid

A

A strong acid will ionise fully and have a higher concentration of product, therefore, there will be a high Ka value (very little acid left, but a lot of product)

24
Q

Ka value of weak acids

A

Weak acids partially ionise and have a lower concentration of product, therefore, they will have a low Ka value (a lot of reactant left, but very little product)

25
Q

Kb value of a strong base

A

A strong base dissociates fully and has a higher concentration and, therefore, has a higher Kb value (very little base left, but a lot of product)

26
Q

Kb value of a weak base

A

A weak base partially dissociates and has a lower concentration and, therefore, has a low Kb value (a lot of reactant left, but very little product)

27
Q

Explain the strength of an acid or base

A

How much of the acid will ionise, or the base dissociates

(Strong or weak)

28
Q

Explain the concentration of an acid or base

A

Amount of acid or base present in a given volume

(Diluted or concentrated)

29
Q

List the strong acids

A
  • HCl
  • H²SO⁴
  • HNO³
  • H²CO³
  • HBr
  • HI
  • HClO⁴
30
Q

List the strong bases

A

Group 1 metals

  • LiOH
  • NaOH
  • KOH
  • RbOH
  • CsOH

Chemistry Grade 11 (6 decks)

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