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ANACHEM MIDTERM > THE CHEMICAL COMPOSITION AND AQUEOUS SOLUTIONS > Flashcards

THE CHEMICAL COMPOSITION AND AQUEOUS SOLUTIONS Flashcards

1
Q

produced in the reaction of an
acid with a base

A

Salt

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2
Q

form ions when dissolved in
water and thus produce solutions that
conduct electricity

A

Electolytes

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3
Q

ionize essentially
completely

A

Strong electrolytes

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4
Q

ionize only partially

A

Weak Electrolytes

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5
Q

proposed independently a
theory of acid/base behavior that is
particularly useful in analytical chemistry.

A

J. N. Brønsted (Denmark) & J. M. Lowry
(England)

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6
Q

Proton theory of acid and base

A

Brønsted-Lowry Theory

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7
Q

a substance that donates
protons

A

Acid

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8
Q

a substance that accepts
protons

A

Base

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9
Q

The species forms
when an acid loses a proton

A

Conjugate Base

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10
Q

The species formed
when a base accepts a proton.

A

Conjugate Acid

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11
Q

completely
dissociated into HSO4
– and H3O+ ions and
for this reason is classified as a strong
analyte

A

Sulfuric Acid (H₂SO₄)

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12
Q

conjugate base of the acid
HNO2

A

Nitrite ion

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13
Q

conjugated acid of
water is hydrated proton written as H3O+

A

Hydronium ion

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14
Q

Strong Classification of Electrolytes

A
  1. Most Salts
  2. Alkali and alkalineearth hydroxide
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15
Q

Weak Classification of Electrolytes

A
  1. Most organic acids
  2. most organic gases and ammonia
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16
Q

when an acid and a
base react to form water and a salt and
involves the combination of H+ ions and
OH- ions to generate water.

A

Neutralization reaction: ( acid1 + base2 ⇌
base1 + acid2 )

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17
Q

an ion that bears both a
positive and a negative charge.

A

Zwitterion

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18
Q

can act as either an acid or as a
base

A

Water

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19
Q

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

A

Amphiprotic solvents

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20
Q

– involves
the spontaneous reaction of molecules of
a substance to give a pair of ions

A

Autoprotolysis (autoionization)

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21
Q

are those who reacts with
water completel

A

Strong acids

22
Q

those who do not
completely react with water.

A

Weak acids

23
Q

the ratio
of concentrations of reactants and
products is constant

A

Chemical Equilibrium

24
Q

a system at equilibrium that represents a dynamic state in which two opposing processes are taking
place at the same time and at the same rate

A

Chemical Equilibrium

25
Q

Chemical Equilib Formula

A

K= products / reactant

26
Q

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

A

Equilibrium-constant expressions (K)

27
Q

reactions that
proceeds forward (→) and backward
(←).

A

Reversible Reactions (⇌)

28
Q

independent of the route by which
equilibrium is reached

A

Position of a chemical equilibrium

29
Q

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

A

Mass-action effect

30
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 principle

31
Q

a branch of
chemical science that deals with the flow
of heat and energy in chemical reactions

A

Thermodynamics

32
Q

FACTORS AFFECTING CHEMICAL
EQUILIBRIUM

A
  1. Nature of reactants
  2. Frequency & efficiency of collisions
  3. Surface Area Exposed
  4. Concentration
  5. Pressure
  6. Temperature
  7. Catalyst
33
Q

This principle states that if a
system is disturbed, the
equilibrium condition is upset
and a reaction tends to proceed
in the direction just to eliminate
or minimize the change

A

LE CHATELIER’S PRINCIPLE

34
Q

describes the
elements whether active or inactive

A

Nature of reactants

35
Q

The speed of a chemical reaction also depends on how often the molecules or ions of the reactants collide with one another

A

Frequency & efficiency of collisions

36
Q

This is carried out by the large space occupied by the material

A

Surface Area Exposed

37
Q

one or more of the reactants is increased, the forward reaction will speed up momentarily until a new position at equilibrium is reached

A

Concentration

38
Q

significantly affect the reaction rate only when one or more of the reactants or products is a gas.

A

Pressure

39
Q

are more energetic and have more kinetic energy, thus their collisions are more likely to result in a reaction

A

Temperature

40
Q

a substance that influences the speed of a reaction

A

Catalyst

41
Q

Heat can be considered as one of the reactants. An increase in temperature would cause a shift to the right.

A

ENDOTHERMIC

42
Q

Heat can be considered as one of the products, the equilibrium will shift to the left in order to relieve the stress on the system

A

EXOTHERMIC

43
Q

Equilibrium Constant (Keq)

A

equal to
the product of the concentration of the
products of the substance formed at
equilibrium divided by the product of the
concentration of the reactants, each
concentration raised to a power which is
the same as the coefficient of the
substance in the chemical equation

44
Q

Law of Mass Actions

A

states that the rate
of a chemical reaction is proportional to
the concentration of the reacting species

45
Q

has
the value of 1.008 x 10-14 but we shall use
the approximation that at room temperature
Kw ≈ 1.00 x 10^-14

A

Ion-Product Constant for Water (Kw)

46
Q

water that contains
one or more dissolved substance

A

Aqueous Solution

47
Q

are
essentially completely dissolved in saturated
aqueous solution

A

Solubility-Product constant (Ksp)

48
Q

Common-ion Effect

A

a mass-action effect
predicted from the Le Châtelier principle

49
Q

Constant Ka

A

the acid dissociation
constant

50
Q

Constant Kb

A

the base dissociation
constant

ANACHEM MIDTERM (1 decks)

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