Unit 8 – Acid-base Titration Flashcards

1
Q

It is a method of quantitative analysis for determining the concentration of an acid/base by neutralizing it with standard solution of base/acid.

A

Acid-base Titration

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2
Q

Types of acid-base titration

A

Alkalimetry
Acidimetry

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3
Q

It is the determination of BASIC CONTENT in a sample by titrating it with a standard acid solution.

A

Alkalimetry

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4
Q

It is the determination of ACID CONTENT in a sample by titrating it with a standard acid solution.

A

Acidimetry

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5
Q

T/F
In ALKALIMETRY, the BASIC CONTENT should be titrate with ACID.

A

T

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6
Q

T/F
In ACIDIMETRY, the ACID CONTENT should be titrate with a standard BASIC solution.

A

T

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7
Q

It is the course of an acid-base titration that is best followed by examining the pH as the titration progresses.

A

Titration Curve

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8
Q

It provides a visual picture of how the property of the titration reaction changes as the titrant is added to the analyte.

A

Titration Curve

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9
Q

Stages in the titration

A

Pre-equivalence point
Equivalence point – end point
Post-equivalence point

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10
Q

Equivalence points in acid-base titrations are determined most often using _____ that change color at or near equivalence point.

A

Chemical indicators

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11
Q

_____ are WEAK ORGANIC acids or bases whose conjugate forms have different colors.

A

Acid-base indicators

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12
Q

T/F
It must be WEAKER than the ANALYTE acid or base that it reacts last with the titrant.

A

T

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13
Q

An average observer visualizes color imparted by a typical indicator within concentration ratio: _____

A

[Hin] / [In-] = 10 to 0.1

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14
Q

It is the point in titration having the GREATEST SLOPE.

A

Inflection point

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15
Q

It very nearly coincides with the equivalence point.

A

Inflection point

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16
Q

T/F
To MINIMIZE titration error, an indicator’s entire transition pH range must fall WITHIN the rapid change in pH at the equivalence point.

A

T

17
Q

This is the use of strong acids or strong bases.

A

Standard solution (titrant)

18
Q

This react more completely with an analyte, yielding a sharper endpoint.

A

Standard solution (titrant)

19
Q

It is widely used for titration of bases

A

HCl

20
Q

It is a strong acid and dilute solutions are stable with little or reducing power.

A

HCl

21
Q

T/F
Chloride ions does not form precipitates with most cations.

A

T

22
Q

It is a concentrated acid and NOT a PRIMARY STANDARD.

A

Hcl

23
Q

It forms insoluble sulfates with a number of common cations.

A

Sulfuric acid

24
Q

Standard bases used for standardization of acids.

A

Primary standard bases

25
Q

It is most often used for standardization of acid solutions.

A

Primary standard bases

26
Q

Most often used for the standardization of acid solutions.

A

Sodium carbonate

27
Q

High purity solid that are commercially available, but is hygroscopic.

A

Sodium carbonate

28
Q

It is also known as borax.

A

Sodium tetraborate

29
Q

T/F
Sodium tetraborate cannot be heated to remove water.

A

T

30
Q

Sodium tetraborate is stored in dessicator over an aqueous solution saturated with _____ and _____.

A

NaCl and Sucrose

31
Q

It is used almost exclusively for titrating acids in solutions.

A

NaOH

32
Q

T/F
Dilute NaOH solutions are stable and can be stored in plastic containers.

A

T

33
Q

It slowly reacts with glass to form soluble silicates.

A

NaOH

34
Q

It has a cementing property; often glass stoppers are “freeze” tightly to the mouth of the container.

A

NaOH

35
Q

T/F
NaOH must be protected from oxygen.

A

F. It should be protected from carbon dioxide/