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1

abscissa

The x-axis of a graph.

2

anhydrous

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

3

atomic mass

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

4

back titration

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.

5

blank titration

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.

6

concentration

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).

7

density

Mass per unit volume.

8

direct titration

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

9

electrolyte

A substance that produces ions when dissolved.

10

end point

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.

11

equivalence point

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

12

formal concentration

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

13

formula mass

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

14

gravimetric analysis

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

15

gravimetric titration

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.

16

indicator

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

17

liter

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

18

molality

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

19

molarity

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

20

mole

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

molecular mass

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

22

ordinate

The y-axis of a graph.

23

parts per billion

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

24

parts per million

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

25

primary standard

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

product

The species created in a chemical reaction.

27

reactant

The species consumed in a chemical reaction.

28

reagent grade chemical

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

29

SI units

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

30

solute

A minor component of a solution.