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ACHEM - testing > Chemistry Unit #8: Acids and Bases .............. Test on April 19, 2017 > Flashcards

Chemistry Unit #8: Acids and Bases .............. Test on April 19, 2017 Flashcards

1
Q

What is the acid name of H₃PO₄?

A

Phosphoric acid

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2
Q

Is F⁻ an acid or a base? (In terms of Brønsted-Lowry)

A

A base because it can accept a proton?

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3
Q

Define hydroxonium ion

A

When H⁺ reacts with water to create the hydrate H₃O⁺

H⁺ + H₂O ⇌ H₃O⁺

H⁺ or H₃O⁺ is a hydroxonium/hydronium ion

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4
Q

Who wrote “Experimental History of Colours”

A

Robert Doyle wrote “Experimental History of Colours”

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5
Q

Is HF a strong or weak acid/base?

A

Weak acid

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6
Q

Is HNO₂ a strong or weak acid/base?

A

Weak acid

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7
Q

Weak bases are _____ electrolytes

A

weak

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8
Q

What is the acidic name of HNO₂?

A

nitrous acid

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9
Q

What are problems associated with using indicators? 4

A

People do not always agree on colours

Most people only detect 1:10 colour ratio changes

Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red

Samples tested must be in solution

Adding too much will change the pH

Solutions must be clear and colourless

Coloured solutions affect indicator colour

Some indicators may react with sample

Change in composition will change colour

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10
Q

Strong acids are _____ electrolytes

A

strong

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11
Q

Define electrolyte

A

When an ionic substance creates an ion in a solution

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12
Q
A
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13
Q

Define Alkali

A

A base that is soluble in water

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14
Q

Metal oxides mixed with water form……?

A

bases

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15
Q

Is this chemical reaction, is the acid monoprotic or diprotic?

H₂SO₄(aq) ⇒ 2H⁺(aq) + SO₄²⁻(aq)

A

Diprotic because when it dissociated, the acid released 2 H⁺

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16
Q

For diprotic acids, the second proton released is always ____ than the first.

A

Weaker

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17
Q

When acids undergo a neutralization reaction with bases, what forms when the base is a carbonate?

A

Salt, carbon dioxide and water

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18
Q

In the chemical equation of NH₃ + H₂O ⇒ NH₄ + OH⁻, since NH₄ is the CA, that makes NH₃ the ____

A

Base. Water is then the acid.

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19
Q

A pH of 1 is ______ times stronger than a pH of 3

A

A pH of 1 is 100 times stronger than a pH of 3

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20
Q

People do not always agree on colours. Most people only detect _____ ratio colour ratio changes

A

People do not always agree on colours. Most people only detect 1:10 colour ratio changes

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21
Q

Define Strong Acids 2

A

Strong bases completely dissociate (split up) into ions in an aqueous solution

They release hydroxide ions in an aqueous solution

NaOH ⇒ Na⁺ + OH⁻

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22
Q

A pH of 1 is _____ times stronger than a pH of 2

A

A pH of 1 is 10 times stronger than a pH of 2

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23
Q

What is the points for Temperature as one of the ways we can distinguish between a strong and a weak acid?

A

Temperature

A reaction between an acid and a substance like a reactive metal is exothermic and the strong acid will release more energy.

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24
Q

Is the chemical reaction of BF₃ + NH₃ a Lewis definition or a Brønsted-Lowry definition?

A

a Lewis definition because the BF₃ acid’s valence electron and the NH₃ base’s valence electron is already full.

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25
Q

What is a pH scale? 2 - 4

A

A pH scale is a way of expressing the strengths of acids and bases.

Instead of using very small numbers, we just use the NEGATIVE power of 10 on the Molarity of the H⁺ (or OH⁻) ion.

A pH of 1 is 10 times stronger than a pH of 2

A pH of 1 is 100 times stronger than a pH of 3

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26
Q
A
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27
Q
A
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28
Q

What is the equilibrium constant of water, {H₂O(l) ⇌ H⁺(aq) + HO⁻(aq)}?

A

Kc = 1 * 10⁻¹⁴

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29
Q

All acids release _______ _____ into solution

A

Hydrogen ions

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30
Q

Brønsted-Lowry Acids and Bases contain _____-bonding pair of electrons

A

Non

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31
Q
A
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32
Q

Strong acids have _____ conductivity

A

strong

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33
Q

An acid of pH = 2 release _______ H⁺ into the solution than an acid of pH = 3

A

An acid of pH = 2 release more H⁺ into the solution than an acid of pH = 3

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34
Q

What is the Lewis definition of an Acid?

A

A substance that can accept an electron pair

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35
Q

How do you calculate pH? 1 - 3

A

pH = -log [H⁺(aq)]

Or When working backwards;

[H⁺(aq)] = antilog (-pH)

Or

[H⁺(aq)] = 10⁻ᵖᴴ

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36
Q

What are the indicators inside the Universal indicator? 4

A

Methyl orange

Methyl red

Bromothymol blue

Phenolphthalein

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37
Q

Define Arrhenius Acid

A

Substance that increases the concentration of H⁺ in aqueous solution.

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38
Q

Adding yellow to red will not be detectable until you have 1 part yellow to __ parts red

A

Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red

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39
Q

Is this chemical reaction, is the acid monoprotic or diprotic?

HCI(aq) ⇒ H⁺(aq) + CI⁻(aq)

A

Monoprotic because when it dissociated, the acid could only release 1 H⁺

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40
Q

What is the Brønsted-Lowry definition of an Acid?

A

A proton (H⁺) donor

The proton is really just a hydrogen atom that has lost it’s electron!

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41
Q

What are the 5 common examples of strong monoprotic acid?

A

HNO₃,

HBr,

HI,

HCIO₄

and H₂SO₄

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42
Q

Weak bases can react with water to form ______ ions in solution

A

Hydroxide

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43
Q

What is the Brønsted-Lowry definition of an Base?

A

A proton (H⁺) acceptor

The proton is really just a hydrogen atom that has gained it’s electron!

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44
Q

Most acids consist of hydrogen and an ______

A

anion

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45
Q

Is a Lewis acid an electrophile or nucleophile?

A

a Lewis acid is an electrophile because the H⁺ is positive and it is attracted to the negative compound like CI⁻

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46
Q

Strong acids ________ dissociate

A

Completely (Note the yield arrow: We use ⇒)

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47
Q

Most bases consist of a ______ with a hydroxide

A

Most bases consist of a cation (metal positively charged ion) with a hydroxide

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48
Q

Define Equimolar

A

Refers to when two solutions containe the same number of moles

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49
Q

Is a Lewis base an electrophile or nucleophile?

A

a Lewis base is a nucleophile because the OH⁻ is negative and it is attracted to the positive compound like Na⁺

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50
Q

Is H₂SO₄ a strong or weak acid/base?

A

Strong acid

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51
Q

Name two natural acid-base indicators

A

Red cabbage juice

Various teas

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52
Q

[H⁺] = [HO⁻] = ______ M for pure water

A

Kc = 1 * 10⁻⁷

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53
Q

When acids react with precious metals, what forms?

A

Nothing because precious metals do not react with the acid

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54
Q

Strong bases have _____ conductivity

A

strong

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55
Q

What is the Lewis definition of a Base?

A

A substance that can donate an electron pair

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56
Q

Is HBr, a strong or weak acid/base?

A

Strong acid

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57
Q

When acids undergo a neutralization reaction with bases, what forms when the base is a hydroxide?

A

Salt and water

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58
Q

Is ammonia a strong or weak acid/base?

A

Weak base

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59
Q

When acids and bases were identified by taste, what do bases taste like?

A

bitter

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60
Q
A
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61
Q

[H⁺] = [____] = Kc = 1 * 10⁻⁷ M for pure water

62
Q

Define Weak Bases

A

Weak bases slightly dissociate (split up) into ions in an aqueous solution

64
Q

Identify the acid, base, conjugate acid and conjugate base. H₂PO₄⁻ + HCO₃⁻ ⇌ HPO₄⁻² + H₂CO₃

A

H₂PO₄⁻ —– A

HCO₃⁻ —– B

HPO₄⁻² —– CB

H₂CO₃ —– CA

65
Q

Are group 1 hydroxides, metal hydroxides with one valence electron, like NaOH a strong or weak acid/base?

A

Strong base

66
Q

Is NaH an ionic acid?

A

No because it will release H⁻

68
Q

Most acids consist of ________ and an anion

69
Q

In equimolar solutions, which has a higher pH? A weak or strong acid?

A

A weak acid has a higher pH than a strong acid of equal concentration because not all of the hydrogen ions have dissociated

71
Q

Strong bases are _____ electrolytes

72
Q

Define Arrhenius base 2

A

Substance that increases the concentration of OH⁻ in aqueous solution.

Substance that neutralizes an acid by removing H⁺ in aqueous solution.

73
Q

What metals do not react with acids?

A

Cu(s), Ag(s), Au(s) They are called ‘noble metals’

74
Q

What is the points for Conductivity as one of the ways we can distinguish between a strong and a weak acid?

A

Conductivity

A weak acid does not conduct electricity as well as a strong acid.

A dimly lit bulb will mean it is a weak acid because a strong acid will a have brightly dim bulb because it has more ions.

75
Q

What are the ways we can distinguish between a strong and a weak acid? 4

A

Temperature

A reaction between an acid and a substance like a reactive metal is exothermic and the strong acid will release more energy.

Bubbling

A reaction between an acid and a substance like metal will bubble, releasing hydrogen and the strong acid will bubble more and release hydrogen.

Reaction time

A weak acid reacts more slowly than a strong acid.

A strong reacts more faster than a weak acid.

Conductivity

A weak acid does not conduct electricity as well as a strong acid.

A dimly lit bulb will mean it is a weak acid because a strong acid will a have brightly dim bulb because it has more ions.

76
Q

Since acids are ionic substances, they _______ in water.

A

Since acids are ionic substances, they dissociate in water.

77
Q

Strong acids have conjugate bases that will….. 2

A

Strong acids have conjugate bases that will not reform the acid

The conjugate bases will act neutral

78
Q

What yield arrow do we use when there is a weak acid/base reacting?

79
Q

When acids undergo a neutralization reaction with bases, what forms when the base is an ammonia?

82
Q

Are amines a strong or weak acid/base?

83
Q

Identify the acid, base, conjugate acid and conjugate base. KHCO₃ + KH₂PO₄ ⇌ H₂CO₃ + K₂HPO₄

A

KHCO₃ —– B

KH₂PO₄ —– A

H₂CO₃ —– CA

K₂HPO₄ —– CB

84
Q

Is C₁₂H₂₂O₁₁ an ionic base?

85
Q

[_____] = [HO⁻] = Kc = 1 * 10⁻⁷ M for pure water

–>

86
Q

Most bases consist of a cation (metal positively charged ion) with a _______

A

Most bases consist of a cation (metal positively charged ion) with a hydroxide

87
Q

Is CH₃OH an ionic base?

88
Q

When acids undergo a neutralization reaction with bases, what forms when the base is a metal oxide?

A

Salt and water

90
Q

What is the products of CO₃(aq) + H₂O(l) ⇌

A

CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + OH⁻(aq)

91
Q

What was lichen Rocella could be used as? 3

A

A purple dye

Add fermented urine (base) to produce an orchid blue dye

Acidified to produce a red dye

92
Q

What is chemical formula of phosphoric acid?

93
Q

Weak bases have _____ conductivity

94
Q

Pure water _____ dissociates

95
Q

If H₂CO₃ is a weak acid, that makes HCO₃⁻¹ a strong or weak acid?

A

Weaker acid

96
Q

What is the points for Reaction time as one of the ways we can distinguish between a strong and a weak acid? 2

A

Reaction time

A weak acid reacts more slowly than a strong acid.

A strong reacts more faster than a weak acid.

97
Q

Define Nucleophile 2-3

A

Substance that donates the e- pair in an organic chemical reaction.

A nucleophile is also a Lewis base.

Typical nucleophiles are CN-, OH- and NH3.

98
Q

When acids react with reactive metals, what forms?

A

Salt and hydrogen gas

100
Q

Identify the acid, base, conjugate acid and conjugate base. NH₃ + C₆H₅COOH ⇌ NH₄⁺ + C₆H₅COO⁻

A

NH₃ —– B

C₆H₅COOH —– A

NH₄⁺ —– CA

C₆H₅COO⁻ —– CB

101
Q

What did Robert Doyle write?

A

Robert Doyle wrote “Experimental History of Colours”

103
Q

Define Amphoteric? 1 - 3

A

A substance that can act both as an acid or a base

e.g. Al₂O₃ and H₂O

Al₂O₃ as a base: Al₂O₃ + 6HCI ⇒ 2AlCI₃ + 3H₂O

Al₂O₃ as an acid: Al₂O₃ + 2NaOH + 3H₂O ⇒ NaAl(OH)₄

104
Q

What is the products of NH₃(aq) + H₂O(l) ⇌

A

NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)

105
Q

Weak acids ________ dissociate

A

Partially (Note the yield arrow: We use ⇌)

106
Q

Define Monoprotic

A

Where one mole of the acid produces one mole of hydrogen ions, e.g. HCl.

107
Q

Define Strong Acids

A

Strong acids completely dissociate (split up) into ions in an aqueous solution

108
Q

What is the signification of Pka?

A

Pka is the pH at which the indicator is in the middle of its colour transition

109
Q

All acids release _______ ions into solution

110
Q

What does pH stand for?

A

“Power of Hydrogen”

111
Q

Weak acids have _____ conductivity

112
Q

[H⁺] = [HO⁻] = Kc = 1 * 10⁻⁷ M for _______

A

pure water

113
Q

What type of bond do Lewis Acids and Bases make?

A

A coordinated dative bond

114
Q

How do you calculate [H⁺(aq)]? 2

A

[H⁺(aq)] = antilog (-pH)

Or

[H⁺(aq)] = 10⁻ᵖᴴ

Or When working backwards;

pH = -log [H⁺(aq)]

116
Q

How do you accurately determine the pH of a solution?

A

Using a pH meter

117
Q

What is the compound name of HNO₂?

A

hydrogen nitrite

118
Q

Since acids are ionic substances, they; 2 (3)

A

They dissociate in water. And They also conduct electricity in water Called electrolyte

119
Q

Weak acids have weak conjugate bases that will….

A

Weak acids have weak conjugate bases that will reform back to the original weak acid

120
Q

What two factors affect the [H₃O⁺] for an acid. 2

A

The labelled concentration of the acid

The strength of the acid

121
Q

When water acts as proton acceptor with HF but as a proton donator, an acid, with ammonia, what is this property called?

A

Amphoteric

122
Q

Define dissociate

A

When molecules separate or split into smaller particles such as ions

123
Q

Define Weak Acids

A

Weak acids slightly dissociate (split up) into ions in an aqueous solution

124
Q

Is H₂O a strong or weak acid/base?

125
Q

Define Amphiprotic 2

A

A type of amphoteric substance that specifically can act as neither an acid or base by accepting or donating hydrogen ions.

E.g. water and diprotic acids.

126
Q

Is HCN a strong or weak acid/base?

127
Q

Non-metal oxides mixed with water form……?

128
Q

What is special about the Lewis definition of acids?

A

There is no requirement for Lewis acids to contain hydrogen

129
Q

What is the points for Bubbling as one of the ways we can distinguish between a strong and a weak acid?

A

Bubbling

A reaction between an acid and a substance like metal will bubble, releasing hydrogen and the strong acid will bubble more and release hydrogen.

130
Q

Is the chemical reaction of H⁺ + H₂O ⇒ H₃O a Lewis definition or a Brønsted-Lowry definition?

A

It a Lewis definition and a Brønsted-Lowry definition because H⁺ acid is an electrophile and the H₂O base is a nucleophile making it a Lewis definition. The H⁺ acid is also a proton donor and the H₂O base is a prton acceptor making it a Brønsted-Lowry definition.

131
Q

Is HNO₃, a strong or weak acid/base?

A

Strong acid

132
Q

Identify the acid, base, conjugate acid and conjugate base. CH₃COOH + OH⁻ ⇌ H₂O + CH₃COO⁻

A

CH₃COOH —– acid

OH⁻ —— base

H₂O —— CA

CH₃COO⁻ —— CB

133
Q

[H₃O⁺] = ____________ M for neutral solution

A

[H₃O⁺] = 1 * 10⁻⁷ M for neutral solution

134
Q

Identify the acid, base, conjugate acid and conjugate base. NaHSO₄ + NaOH ⇌ Na₂SO₄ + H₂O

A

NaHSO₄ —– A

NaOH —– B

Na₂SO₄ —– CB

H₂O —– CA

135
Q

[H₃O⁺] = ____________ M for acidic solution

A

[H₃O⁺] = 1 * 10⁻⁷ M for acidic solution

137
Q

Weak acids are _____ electrolytes

138
Q

What yield arrow do we use when there is a weak acid/base reacting?

140
Q

What is the fancy name of bubbling?

A

effervescence

141
Q

Names 3 bases that is a base that doesn’t consist of a cation (metal positively charged ion) with a hydroxide

A

Ammonia, NH₃ and organic amines, R-NH₂

142
Q

When acids and bases were identified by taste, what do acids taste like?

A

Sour (like most fruits)

143
Q

Is HI, a strong or weak acid/base?

A

Strong acid

145
Q

Is HCIO₄ a strong or weak acid/base?

A

Strong acid

147
Q

Adding yellow to red will not be detectable until you have __ part yellow to 9 parts red

A

Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red

148
Q

[H₃O⁺] = ____________ M for alkaline solution

A

[H₃O⁺] = 1 * 10⁻⁷ M for alkaline solution

149
Q

What is a hydronium ion?

150
Q

After the lichen Rocella, what came as a way to test acids and bases

A

The litmus test

ACHEM - testing (5 decks)

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