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Chemistry 12 > Unit 4: Acids, Bases, And Salts (3) > Flashcards

Unit 4: Acids, Bases, And Salts (3) Flashcards

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1
Q

A solution with an accurately know concentration is called a____ or a _____

A

Standard solution

Standardized solution

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2
Q

A primary standard is…

A

A substance which can be obtained in a pure stable form (Doesnt absorb water or carbon dioxide). It must also have a known molar mass which can be used to prepare a solution of known concentration

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3
Q

How can you create a standard solution that is not a primary standard?

A

Titrate a base with a primary standard (or other solution of known concentration) to find the exact concentration of the base.

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4
Q

What are the two acidic primary standards most commonly used?

A

Potassium hydrogen phthalate (KHC8H4O4)

Oxalis acid dihydrate (H2C2O4•2H2O)

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5
Q

Potassium hydrogen phthalate (KHC8H4O4), is ____ in its reaction with NaOH and the best indicators to use with it are ______ or ______.

A

Monoprotic
Phenolphthalein
Thymol blue

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6
Q

Oxalis acid dihydrate (H2C2O4•2H2O) is _____ in its reaction with NaOH and the best indicator to use with it is _____.

A

Diprotic

Phenolphthalein

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7
Q

The most common basic primary standard is _____.

A

Sodium carbonate (Na2CO3)

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8
Q

Sodium carbonate (Na2CO3) is _____ in its reaction with HCl and the best indicator to use for it is_____.

A

Diprotic

Methyl orange

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9
Q

In order to carry out a titration, you must have a solution with an accurately known ______.

A

Concentration

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10
Q

When ever an acid is added to a base the H+ available in the ____ react with the _____ in the base. When no excess ___ or ____ remain in solution, the solution is ____.

A 
Acid
OH-
H+ 
OH-
Neutral
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11
Q

The process of arriving at a neutral solution is called ___.

A

Neutralization

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12
Q

What is titration?

A

Titration is the process of adding a solution of known concentration and known volume (often a base) to a solution with a known volume and unknown concentration (often an acid) to find the unknown concentration

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13
Q

At equivalence point the moles of H+ equals to…?

A

The moles of OH-

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14
Q

What is the purpose of a buffer?

A

To maintain a relatively constant pH when either a small amount of acid or base is added

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15
Q

Buffers have an equilibrium between…

A

a weak acid (or weak base) and its conjugate weak base (or conjugate weak acid).

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16
Q

Buffers only work when a ____ amount of acid or base is added

A

Small

17
Q

You need a minimum of ____ weak acid/base and its conjugate base/acid to create a buffer

A

1 M [ ]

18
Q

%purity=…?

A

((Mass of active ingredient) / (mass of sample)) X 100

19
Q

What kind of titrations are never done?

A

Weak acid weak base titrations

20
Q

What are the 4 main regions of pH vs volume graphs

A

A. Initial pH (before titration)
B. pH before equivalence point
C. pH at equivalence point
D. pH after equivalence point

21
Q

A primary solution is made from scratch and the [calculated] is equal to…?

A

[actual]

22
Q

Acid rain has a pH of 5-6. What is the pH of acid rain?

A

4-5

23
Q

What is the main cause of acid rain?

What natural phenomenon can also cause acid rain?

A

The burning of fossil fuels

And lighting

24
Q

What are 4 side effects of acid rain

A

1-leach out nutrients from soil (killing plants)
2- damage lakes (kills all stuff in the lake - Quebec)
3- affects human health (asthma and respiratory diseases)
4- breaks down buildings (destroys concrete over time)

25
Q

Name 4 ways to prevent acid rain?

A

1-higher smoke stacks/scrubbers
2- toughen up on pollution laws
3-alternative fuels and energy sources
4- better made cars (pollute less)

26
Q

Only ionic metal oxides form ___ solutions

A

Basic

27
Q

Covalent oxides form ____ solutions

A

Acidic

28
Q

A ____ is a weak ____ acid or base with different colours for its conjugate acid and conjugate base forms

A

Indicator

Organic

29
Q

An indicator is in its ____________ form when in highly acidic solutions

A

Conjugate acid

30
Q

An indicator is in is ________ form when in highly basic solutions

A

Conjugate base

31
Q

In acidic solutions [HIn] is _____ (,=) [In-]

A

Greater than (>)

32
Q

In basic solutions [HIn] is _____ (,=) [In-]

A

Less than (

33
Q

The [H3O+] at which an indicator changes colour equals to..?

A

The Ka for the indicator

34
Q

An indicator is at the midpoint of of its colour change when the pH of the solution equals…?

A

The pKa of the indicator

Chemistry 12 (7 decks)

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