G12E chemistry EOT T1

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55 Terms

1
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What is the ion-product constant of water?

Kw = 1×10-14 at 25C

2
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What is the equation relating [H+] and [OH-] in a solution at a temperature of 25C?

Kw = [H+][OH-]

3
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How do we find [H+] from the pH?

[H+] = 10-pH

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How do we find the pH from [H+] ?

-log(H+)

5
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How do we get pOH or pH?

14 - pH = pOH

14 - pOH = pH

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What’s a buffer solution?

  • A buffer solution is a solution that resists change in pH when an acid or case is added to it.

7
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What does a buffer solution consist of?

A weak conj. acid-base pair. Either:

  • A weak acid + conj. base

  • A weak base + conj. acid

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What is an oxide?

a compound which is the result of the reaction between a metal or non-metal with oxygen.

9
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Which groups of oxides are basic?

1 and 2 (except Be + O)

They react with water to make a basic solution.

Example in picture

<p>1 and 2 (except Be + O)</p><p>They react with water to make a basic solution.</p><p>Example in picture</p>
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What makes a basic oxide?

It makes a hydroxide compound (or basic solution) when it reacts with water

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What makes an acidic oxide?

Most acidic oxides are with nonmetals.

It forms an acidic solution when it reacts with water.

<p>Most acidic oxides are with nonmetals.</p><p>It forms an acidic solution when it reacts with water.</p>
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What happens when a basic oxide reacts with an acid and an acidic oxide reacts with a base?

They form an ionic compound and water.


Source:

<p>They form an ionic compound and water.</p><div data-type="horizontalRule"><hr></div><p>Source: </p><div data-youtube-video=""><iframe width="640" height="480" allowfullscreen="true" autoplay="false" disablekbcontrols="false" enableiframeapi="false" endtime="0" ivloadpolicy="0" loop="false" modestbranding="false" origin="" playlist="" src="https://www.youtube.com/embed/JZymzk6qoRU" start="0"></iframe></div><p></p>
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What does it mean when something is amphoteric?

It means it has both acidic and basic properties.

Example: Water

14
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Give an example of an amphoteric oxide.

AI2O3 (aluminum oxide)

<p>AI<sub>2</sub>O<sub>3 </sub>(aluminum oxide)</p>
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What is a hydroxide?

element + OH

<p>element + OH</p>
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How does a neutral oxide form?

A neutral oxide is formed when the cation is from a strong base and an anion is from a strong acid.

17
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Which groups make a basic hydroxide?

Group 1 and 2

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Give an example of an amphoteric hydroxide

Al(OH)3

19
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According to the periodic table, which directions does acidity increase in?

  • Acidity increases from left to right (due to electronegativity)

  • Increases from top to bottom (due to size)

20
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What is the common ion effect?

  • The common ion effect describes the effect on equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution. The common ion effect generally decreases solubility of a solute.

  • Basically, if you add another ion that already exists in the solution it makes it harder to dissolve. Like if you add too much tang to your water.

<ul><li><p>The common ion effect describes the effect on equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution. The common ion effect generally decreases solubility of a solute.</p></li><li><p>Basically, if you add another ion that already exists in the solution it makes it <strong>harder to dissolve</strong>. Like if you add too much tang to your water.</p></li></ul><p></p>
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A homogeneous equilibrium

all species are present in the same phase

<p>all species are present in the same phase</p>
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A heterogeneous equilibrium

species exist in more than one phase

<p>species exist in more than one phase</p>
23
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Le Chatelier's principle:

  • if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to re-establish an equilibrium.

  • Basically, if stress is added to the equilibrium, the equilibrium will shift in response to the stress to remain balanced

24
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According to Le Chatelier's principle:

What’ll happen if the concentration of the reactant increases?

  • Equilibrium will shift towards the decrease in the concentration of the reactants.

  • Equilibrium of the reaction shift towards the right.

25
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According to Le Chatelier's principle:

What’ll happen if the concentration of the reactant decreases?

  • Equilibrium will shift towards the increase in the concentration of the reactants.

  • •Equilibrium of the reaction shift towards the left.

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According to Le Chatelier's principle:

What’ll happen if If the product decreases?

Equilibrium of the reaction shift towards the right.

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According to Le Chatelier's principle:

What’ll happen if If the product increases?

Equilibrium of the reaction shift towards the left.

28
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As per Le Chatelier's principle, an increase in pressure or decrease in volume will ____?

  • At constant pressure, the addition of inert gas increases the volume, so it decreases the product formation.

  • At constant volume, the equilibrium remains undisturbed. It is because adding an inert gas at constant volume does not change the partial pressures.

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What is a lewis base?

a substance that can donate a pair of electrons.

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What is a lewis acid?

a substance that can accept a pair of electrons.

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Shortcut for lewis acids and bases

Acid = Accepts

Base = Brings

32
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Is CO2 classified as a Lewis acid/base?

Acidic, because of resonance

33
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Is H2O a Lewis acid or base?

The oxygen in water has 2 lone pairs meaning that it’s a lewis base

34
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Is I- a Lewis base or acid?

It’s a lewis base because it has excess electrons to donate.

Shortcut: if it’s a negative sign, it’s a lewis base. If it’s a plus, it’s a lewis acid.

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Is NH3 a Lewis base or acid?

NH3 has a lone pair of electrons and is a Lewis base.

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Is BCl3 a Lewis base or acid?

Acid. It’s electron deficient because it has a central atom

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In the above reaction, 𝑨𝒍𝑪𝒍𝟑 is a Lewis acid and 𝑪𝒍−is a Lewis base.

Clue: If one has a sign, the other has the opposite label. E.g: if Cl- is a lewis base then AlCl3 is a lewis acid.

<p>In the above reaction, 𝑨𝒍𝑪𝒍𝟑 is a Lewis acid and 𝑪𝒍−is a Lewis base.</p><p>Clue: If one has a sign, the other has the opposite label. E.g: if Cl<sup>-</sup> is a lewis base then AlCl<sub>3</sub> is a lewis acid.</p>
38
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How does Ka determine the strength of an acid?

knowt flashcard image
39
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Ka formula (ice table)

Ka = [product]/[reactant]

40
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What’s the formula for ionization % ?

(X (ice table) / [reactant initial concentration) x 100

<p>(X (ice table) / [reactant initial concentration) x 100</p>
41
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What is the quadratic formula?

knowt flashcard image
42
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<p>How do we find the ionization percentage from the total and the ionized from an illustration:</p>

How do we find the ionization percentage from the total and the ionized from an illustration:

example:

<p>example:</p>
43
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<p>Explain why B is the correct answer here</p>

Explain why B is the correct answer here

B has an equal number of red and green indication total ionization (100%) which is a property of a strong acid

44
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Shortcut for writing conjugate base

thanks chat gpt

<p>thanks chat gpt</p>
45
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Explain how an acid-base indicator works in a titration.

A noticeable pH change occurs near the equivalence point of acid-base titrations and an indicator can be used to signal the end of a titration.

<p>A noticeable pH change occurs near the equivalence point of acid-base titrations and an indicator can be used to signal the end of a titration.</p>
46
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What are the criteria for choosing an indicator for a particular acid-base titration?

When selecting an indicator for acid-base titrations, choose an indicator whose pH range falls within the pH change of the reaction.

<p>When selecting an indicator for acid-base titrations, choose an indicator whose pH range falls within the pH change of the reaction.</p>
47
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Examples of diprotic acids

Examples of such acids are carbonic acid 𝑯𝟐𝑪𝑶𝟑, sulfuric acid 𝑯𝟐𝑺𝑶𝟒 and chromic acid 𝑯𝟐𝑪𝒓𝑶𝟒.

48
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What’s a diprotic acid?

An acid that is capable of donating two protons to other atoms are called diprotic acids.

49
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50
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52
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Brønsted-Lowry acid

A Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion.

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Brønsted-Lowry base

A Brønsted-Lowry base is any species that can accept a hydrogen ion (𝑯+)

54
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Brønsted shorcut

Brønsted acids give away protons, while bases grab them.

55
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