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Quantitative Analysis > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

The x-axis of the graph

A

Abscissa

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2
Q

Adjective describing a substance from which all water has been removed

A

Anhydrous

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3
Q

The number of grams containing Avogadro’s number of atoms

A

Atomic mass

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4
Q

One in which an excess of standard reagent is added to react with analyte. Then the excess reagent is titrated with a second reagent or with a standard solution of analyte

A

Back titration

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5
Q

One in which a solution containing all reagents except analyte is titrated. The volume of titrant needed should be subtracted from the volume needed to titrate unknown

A

Blank titration

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6
Q

States how much solute do a container in a given volume or mass of solution or solvent

A

Concentration

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7
Q

The mass per unit volume

A

Density

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8
Q

One in which the analyte is treated with titrated and the volume of titrated required for complete reaction is measured

A

Direct titration

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9
Q

A substance that dissolves into ions in solution

A

Electrolyte

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10
Q

Point in a titration at which there is a sudden change in a physical property, such as indicator color, pH, conductivity, or absorbance. Used as a measure of the equivalence point

A

End point

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11
Q

Point in a titration at which the quantity of titrant is exactly sufficient for stoichiometric reaction with the analyte

A

Equivalence point

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12
Q

A description of how the solution was made by dissolving F moles per liter

A

Formal concentration

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13
Q

The sum of atomic masses of atoms in the formula

A

Formula mass

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14
Q

Chemical analysis based on weighing a final project

A

Gravimetric analysis

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15
Q

A titration in which the mass of titrant is measured, instead of the volume. Titrant concentration is conveniently expressed as mol reagent/kg titrant solution; can be more accurate and precise than volumetric titrations

A

Gravimetric titration

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16
Q

A compound having a physical property (usually color) that changes abruptly near the equivalence point of a chemical reaction

A

Indicator

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17
Q

The volume of a cube that is 10 cm on each edge

18
Q

Concentration expressed as moles of substance per kilogram of solvent

A

Molality (m)

19
Q

The number of moles of a substance per liter or solution

A

Molarity (M)

20
Q

Avogadro’s number of particles (atoms, molecules, ions, etc)

21
Q

The sum of atomic masses of the atoms in the atoms in the molecule

A

Molecular mass

22
Q

The y-axis of the graph

23
Q

Mass of substance over mass of sample times 10^6

A

Parts per million (ppm)

24
Q

Mass of substance over mass of sample times 10^9

A

Parts per billion (ppb)

25
Q

A reagent that is pure enough and stable enough to be used directly after weighing. The entire mass is considered to be pure reagent

A

Primary standard

26
Q

The species created in a chemical reaction; appears on the right side of the chemical equation

27
Q

The species consumed in a chemical reaction; appears on the left side of the chemical equation

28
Q

A high-purity chemical generally suitable for use in quantitative analysis and meeting purity requirements set by organizations such as the American Chemical Society

A

Reagent grade chemical

29
Q

International system of units based on the meter, kilogram, second, ampere, kelvin, candela, mole, radian, and steradian

30
Q

A minor species in a solution

31
Q

A major species in a solution

32
Q

Process of determining the concentration of a reagent by reaction with a known quantity of a second reagent

A

Standardization

33
Q

A solution whose composition is known by virtue of the way that it was made from a reagent of known purity or by virtue of its reaction with a known quantity or a standard reagent

A

Standard solution

34
Q

The calculation of quantities of substances involved in a chemical reaction

A

Stiochiometry

35
Q

Substance added to the analyte in a titration

36
Q

A procedure in which one substance (titrant) is carefully added to another (analyte) until complete reaction has occurred. The quantity of titrant required for complete reaction tells how much analyte is present

37
Q

Difference between the observed end point and the true equivalence point in a titration

A

Titration error

38
Q

Chemical analysis of very low levels of analyte, typically ppm and lower

A

Trace analysis

39
Q

(Volume of solute/volume of solution) x 100

A

Volume percent

40
Q

A technique in which the volume of material needed to react with the analyte is measured

A

Volumetric analysis

41
Q

(Mass of solute/mass of solution) x 100

A

Weight percent

Quantitative Analysis (12 decks)

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