Analytical Chemistry Chapter 2 Flashcards

1
Q

A standardized system of units that the scientist adopt

A

International System of Units (SI)

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2
Q

SI is the acronym of the:

A

“Système international d’Unités”

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3
Q

a non-SI unit of length that is widely used to express the wavelength of very short radiation such as x-rays.

A

Angstrom Unit (Å)

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4
Q

How to determine the amount of chemical species?

A

Mass Measurement

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5
Q

Name the Unit and Abbreviation

Mass
Length
Time
Temperature
Amount of substance
Electric current
Luminous density

A

kilogram - kg
Meter - m
Seconds - s
Kelvin - K
Mole - m
Ampere - A
Candela - cd

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6
Q

The _________ is the SI unit for the amount of a chemical substance.

It is always associated with specific microscopic entities such as atoms, molecules,
ions, electrons, other particles, or specified groups of such particles as represented by a
chemical formula.

One mole contains exactly _______elementary entities
(atoms, molecules, ions, electrons, and so on)

6.02214076×10²³ is known as _________

When expressed in the unit mol⁻¹, this number is
called _______, which is often rounded to __________

A

mole (mol)

6.02214076×10²³

Avogadro’s constant

Avogadro’s number

6.022×10²³ mol⁻¹

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7
Q

How do we calculate molar masses?

A

Summing the atomic masses of all the atoms appearing in a chemical formula

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8
Q

The ________ of a substance is the mass in grams of 1 mole of that substance.

A

Molar Mass (M)

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9
Q

______ is an
unchanging measure of the quantity of matter in an object.

_______ invariant measure of the amount of matter.

_______ is the force
of attraction between an object and its surroundings, principally Earth.

the force of gravitational attraction between that matter and earth.

Weight and mass are related by the familiar expression _________
where w is the _____,
m is its ______, and
g is the _________.

A

Mass

Weight

w=mg

weight of an object

mass

acceleration due to
gravity

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9
Q

The distinction between mass and weight is often lost in common usage, and the process of comparing masses is usually called ______.

The objects of known mass as well as the results of weighing are frequently called______.

Always bear in mind, however, that analytical data are based on _____ rather than _______.

Usage of _____ is for the act of determining the mass of an object. Also, we often say ________
to mean the standard masses used in weighing.

A

weighing

weights

mass, weight

weights

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10
Q

The masses for the elements listed in the table 2-1 (SI Base Units) are relative masses in terms of ______.

The ______ is defined as 1/12 the mass of a neutral 12C atom

A

unified atomic mass units (u) or daltons (Da)

dalton

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11
Q

The ________ is 1/1000 of a mole, and the mass in grams of a millimole,
the millimolar mass (mM), is likewise 1/1000 of the molar mass.

1 mmol = 10^-3 mol
10^3 mmol = 1 mol

A

millimole

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12
Q

There are four fundamental ways of expressing solution concentration

A

molar concentration percent concentration solution-diluent volume ratio
p-functions.

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13
Q

The ________ of a solution of a solute species X is the number of moles of that species that is contained in 1 L of the solution (not 1 L of the solvent).

A

molar concentration of solution of a chemical species X

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14
Q

symbolized by M, which has the dimensions of mol/L, or mol^-1.

Is also equal to the number of millimoles of solute per milliliter of solution.

A

Molar concentration or molarity

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15
Q

If the number moles of solute is nx, and the volume of solution is V, the molar concentration is cx, what is the equation?

Equation when finding a number of moles.

A

cx=nx/V

Molarity =

M= no. mol solute/no L. solution

=no. mmol solute/no mL. solution

NA = CA x VA

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16
Q

is the total number of moles of a solute,
regardless of its chemical state, in 1 L of solution. It describes how a
solution of a given concentration can
be prepared.

A

Molar analytical concentration

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17
Q

Gives the total number of moles of a solute in 1 L of the solution or the total number of millimoles in 1 ml.

Specifies a recipe by which the solution can be prepared.

Total number of moles of a solute, regardless of its chemical state, in one liter of solution. It describes how a solution can be prepared.

A

Analytical Molarity

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18
Q

Express the molar concentration of a particular species in a solution at equilibrium.

To determine the species molarity, it is necessary to know _________.

Molar concentration of a particular species in a solution at equilibrium.

A

Equilibrium Molarity

how the solute behaves when it is dissolved in a solvent

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19
Q

In percent concentration what are the three common method:

the denominator in each of these expressions is the ____________ rather than mass or volume of solvent

Only __________ has the advantage of being temperature independent

A

mass or volume of solution

weight percent

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20
Q

______is often used to express the concentration of commercial aqueous
reagents. For example, nitric acid is sold as a 70% (w/w) solution, meaning that the reagent contains 70 g of HNO3 per 100 g of solution.

Weight percent should more properly be called ______ and abbreviated m/m

_______ is commonly used to specify the concentration of a solution prepared by diluting a pure liquid compound with another liquid. For example, a 5% (v/v) aqueous solution of methanol usually describes a solution prepared by
diluting 5.0 mL of pure methanol with enough water to give 100 mL.

_______is often used to indicate the composition of dilute aqueous solutions of solid reagents. For example, 5% (w/v) aqueous silver nitrate often refers to a solution prepared by dissolving 5 g of silver nitrate in sufficient water
to give 100 mL of solution.

True or False: Do not always specify the type of percent when reporting
concentrations in this way

A

Weight percent

mass percent (weight percent is widely used in book)

Volume percent

Weight or volume percent

False

21
Q

For very dilute solutions, ________ is a convenient way to express concentration:

where cppm is the ______.

For even more dilute solutions,
_______ rather than 10^6 ppm is used in the previous equation to give the results in parts per billion (ppb).

The term ______ is also used, especially in oceanography

A

parts per million (ppm)

(formula)

concentration in parts per million

10^9 ppb

parts per thousand (ppt)

22
Q

The composition of a dilute solution is sometimes specified in terms of the volume
of a more concentrated solution and the volume of solvent used in diluting it

The volume of the former is separated from that of the latter by a _____.
Ex: 1:4 HCl
solution contains four volumes of water for each volume of concentrated hydrochloric acid.

dilution equation:

A

Solution-Diluent Volume Ratios

colon

Vconcd X cconcd + Vdil X cdil

23
Q

Scientists frequently express the concentration of a species in terms of its _____________.

The _____ is the negative logarithm (to the base 10) of the molar concentration of that species.

___ offer the advantage of allowing concentrations that vary over 10 or more orders of magnitude to be expressed in terms of
small positive numbers.

The best-known
p-function
is _____, which is the negative
logarithm of [H3O+]

A

p-function, or p-value

p-value

pX = -log [X]

p-values

pH

24
Q

The density of a substance is its mass per unit volume.

Expresses the mass of a
substance per unit volume. In SI units, density is expressed in units of ____________.

______Ratio of its mass to the mass of an equal volume of water at 4°C.

______Ratio of the
mass of a substance to the mass of an
equal volume of water.

Specific gravity is
_______ and so is not tied to any particular system of units. Widely used in describing items of commerce

A

Density

kg/L or g/mL

specific gravity

dimensionless

25
Q

_________ is the quantitative relationship among the amounts of reacting chemical species.

is the relationship among the number of moles of reactants and products as represented by a
balanced chemical equation.

A

Stoichiometry

Stoichiometry of a reaction

26
Q

An ______ gives the simplest whole number ratio of atoms in a chemical compound.

In contrast, a ________ specifies the number of atoms in a molecule.

State figure 2-2

A _______ provides additional information. Their structural formulas, C2H5OH and CH3OCH3, reveal structural differences between these compounds that are not shown in their common molecular formula.

A

empirical formula

molecular formula

structural formula

27
Q

A ______ is a statement of the combining ratios or stoichiometry (in units of moles) among the reacting substances and their products.

Often the physical state of
substances appearing in
equations is indicated by the letters:

(g), (l), (s), and (aq)

A

balanced chemical equation

Refer to gaseous, liquid, solid, and aqueous solution states

28
Q

______ is the most plentiful solvent on Earth, is easily purified, and is not toxic. It is, therefore, widely used as a medium for chemical analyses.

A

Water

28
Q

form ions when dissolved in water (or certain other solvents) and thus produce solutions that conduct electricity

_____ ionize essentially completely in a solvent.

Among the strong electrolytes listed are _____,______,______.

ionize only partially

A

electrolytes

Strong electrolytes

weak electrolytes

acids, bases, and salts

29
Q

An important feature of the Brønsted-Lowry concept is the idea that the product
formed when an acid gives up a proton is a potential proton acceptor and is called
the __________.

We refer to acid1 and base1 as a ______, or just a ________.

Similarly, every base accepts a proton to produce a ________.

When these two processes are combined, the result is an _____ or _____

A

conjugate base of the parent acid

conjugate acid-base pair

conjugate pair

conjugate acid

acid-base, or neutralization

30
Q

An acid ______.

A base _______.

A

donates protons

accepts protons

31
Q

An acid donates protons only in the presence of a
________.

Likewise, a base accepts
protons only in the presence of a
________.

A _______ is formed when
an acid loses a proton. For example,
acetate ion is the conjugate base of
acetic acid. Similarly, ammonium
ion is the conjugate acid of the base
ammonia.

A ______ is formed when a
base accepts a proton.

A _______ acts as an acid only in the presence of a base and vice versa.

A

proton acceptor
(a base)

proton donor (an acid)

conjugate base

conjugate acid

substance

32
Q

Species that have both acidic and basic properties

A

amphiprotic

33
Q

When dissolved in water,
an amino acid, such as glycine, undergoes a kind of internal acid-base reaction to
produce a ______

—a species or an ion that has both a positive and a negative charge.

A

zwitterion

34
Q

_____ is the classic example of an amphiprotic solvent

a solvent that can
act either as an acid or as a base, depending on the
solute.

Other common amphiprotic solvents are:

A

Water

methanol
ethanol
anhydrous acetic acid.

35
Q

behave as acids in the presence of basic solutes
and bases in the presence of acidic solutes.

A

Amphiprotic Solvents

36
Q

Amphiprotic solvents can undergo self-ionization, or ______, to form a pair of ionic species.

______ (also called
______) is the spontaneous
reaction of molecules of a substance to give a pair of ions.

A

Autoprotolysis or autoionization

37
Q

In figure 2-3. The first two are _____ because reaction with the solvent is sufficiently complete that no undissociated solute molecules are left in aqueous solution.

The rest are weak acids, which react incompletely with water to give solutions containing significant quantities of both the parent acid and its conjugate base.

A

strong acids

weak acids

38
Q

Swedish chemist, formulated many of the early ideas regarding the ionic dissociation in solution.

Suggest the relationship between the amount of carbon dioxide in atmosphere and global temperature, also called as greenhouse effect.

A

Svante Arrhenius

39
Q

In a ______, various
acids dissociate to different degrees and have different strengths.
Ex: _______

In a _______, several acids are completely dissociated and show the same strength. Ex: ______

A

differentiating solvent, Acetic Acid

leveling solvent, Water

40
Q

Many reactions used in analytical chemistry never result in complete conversion of reactants to products.

Instead, they proceed to a __________ in which the ratio of concentrations of reactants and products is constant.

_______ are algebraic equations that describe the concentration
relationships among reactants and products at equilibrium.

True or False. The position of a chemical equilibrium is dependent of the route by which equilibrium is reached.

A

State of Chemical Equilibrium

Equilibrium Constant Expressions

False. Dependent - “independent”

41
Q

________states that the position of an equilibrium always shifts in such a direction as to relieve a stress that is applied to the system.

A

Le Châtelier’s principle

42
Q

The _______ is a shift in
the position of an equilibrium caused by adding one of the reactants or products to a system.

A

mass-action effect

42
Q

Are the amount of reactants and products constant?

Why?

A

Equilibrium is a dynamic process.

Although chemical reactions appear to stop at equilibrium, in fact,

the amounts of reactants and products are constant because the “rates of the forward and reverse
processes are identical”.

43
Q

__________is a branch of chemistry that concerns
the flow of heat and energy in chemical reactions. The position of
a chemical equilibrium is related to these energy changes.

A

Thermodynamics

44
Q

The influence of concentration or pressure (if the participants are gases) on the
position of a chemical equilibrium is conveniently described in quantitative terms
by means of an_______.

A

equilibrium-constant expression

45
Q

In other words, the
number of moles of Ba(IO3)2 divided by the volume of the solid Ba(IO3)2 is constant
no matter how much excess solid is present. Therefore, the previous equation can be
rewritten;

where the new constant is called the….

A

Solubility-product constant or the solubility
product.

45
Q

Two chemist in field of thermodynamics. First to propose the law of mass action.

A

Cato Guldberg and Peter Waage

46
Q

The _______ is a mass-action effect predicted from Le Châtelier’s principle

A

common-ion effect