Chapter 1 Flashcards

1
Q

abscissa

A

The x-axis of a graph.

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2
Q

anhydrous

A

Adjective describing a substance from which all water has been removed.

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3
Q

atomic mass

A

Number of grams of an element containing Avogadro’s number of atoms.

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4
Q

back titration

A

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.

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5
Q

blank titration

A

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

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6
Q

concentration

A

An expression of the quantity per unit volume or unit mass of a substance. Common measures of concentration are molarity (mol/L) and molality (mol/kg of solvent).

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7
Q

density

A

Mass per unit volume.

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8
Q

direct titration

A

One in which the analyte is treated with titrant and the volume of titrant required fro complete reaction is measured.

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9
Q

electrolyte

A

A substance that produces ions when dissolved.

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10
Q

end point

A

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.

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11
Q

equivalence point

A

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

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12
Q

formal concentration

A

F, the molarity of a substance if it did not change its chemical form on being dissolved. It

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13
Q

formula mass

A

FM, The mass containing one mole of the indicated chemical formula of a substance.

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14
Q

gravimetric analysis

A

Any analytical method that relies on measuring the mass of a substance (such as a precipitate) to complete the analysis.

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15
Q

gravimetric titration

A

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. Gravimetric titrations can be more accurate and precise than volumetric titrations.

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16
Q

indicator

A

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

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17
Q

liter

A

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

18
Q

molality

A

m, A measure of concentration equal to the number of oles of solute per kg of solvent.

19
Q

molarity

A

M, A measure of concentration equal to the number of moles of solute per liter of solution.

20
Q

mole

A

mol, SI unit for the amount of substance that contains as many molecules as there are atoms in 12 g of (12)^C. There are approximately 6.022 x 10^(23) molecules per mole.

21
Q

molecular mass

A

The number of grams of a substance that contains Avogadro’s number of molecules.

22
Q

ordinate

A

The y-axis of a graph.

23
Q

parts per billion

A

ppb, An expression of concentration denoting nanograms of solute per gram of solution

24
Q

parts per million

A

An expression of concentration denoting micrograms of solute per gram of solution.

25
Q

primary standard

A

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

26
Q

product

A

The species created in a chemical reaction.

27
Q

reactant

A

The species consumed in a chemical reaction.

28
Q

reagent grade chemical

A

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

29
Q

SI units

A

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

30
Q

solute

A

A minor component of a solution.

31
Q

solvent

A

Major constituent of a mixture.

32
Q

standardization

A

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

33
Q

standard solution

A

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 of a standard reagent.

34
Q

stoichiometry

A

Ratios of substances participating in a chemical reaction.

35
Q

titrant

A

Substance added to the analyte in titration.

36
Q

titration

A

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

titration error

A

Difference between the observed endpoint and the true equivalence point.

38
Q

trace analysis

A

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

39
Q

volume percent

A

Defined as (volume of solute/volume of solution) x 100.

40
Q

volumetric analysis

A

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

41
Q

weight percent

A

(Mass of solute/mass of solution) x 100