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Chemistry 1/2 > chap 11 key terms > Flashcards

chap 11 key terms Flashcards

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1
Q

accuracy

A

Accuracy- The value of a measurement is considered to be accurate if its judged to be close to the true value of the quantity being measured.

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2
Q

acid

A

Acid- a substance capable of donating a hydrogen ion (proton).

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3
Q

acid-base reaction

A

Acid-base reaction- A reaction in which one substance, an acid, donates a hydrogen ion (proton) to another substance, a base.

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4
Q

acidic proton

A

Acidic proton- A proton bonded to an electronegative element (oxygen, nitrogen or fluorine) that’s donated to a base during an acid-base reaction.

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5
Q

acidic solution

A

Acidic solution- An aqueous solution in which the concentration of hydronium ions (H3O+) is greater than the concentration of hydroxide ions (OH-). At 25OC, pH < 7.

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6
Q

acidity

A

Acidity- The concentration of H3O+ ions in an aqueous solution. Acidity is measured using the pH scale.

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7
Q

alkali

A

Alkali- A soluble base or solution of a soluble base.

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8
Q

amphiprotic

A

Amphiprotic- The ability to act as an acid (proton donor) and also as a base (proton acceptor).

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9
Q

antacids

A

Antacids- Substances that neutralise stomach acidity. They are often soluble metal hydroxides or carbonates or a mixture of both.

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10
Q

base

A

Base- A substance capable of accepting a hydrogen ion (proton).

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11
Q

basic solution

A

Basic solution- An aqueous solution in which [H3O+] < [OH-]. For a basic solution at 25OC, pH > 7.

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12
Q

bronsted-lowry theory

A

Bronsted-Lowry theory- A theory that defines an acid as a proton (hydrogen ion) donor and a base as a proton acceptor. In the reaction HCl(g) + H2O(l)  H3O+(aq) + Cl-(aq), HCl is the proton donor and is classified as an acid. H2O is a proton acceptor and is classified as a base.

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13
Q

calcification

A

Calcification- The building of a deposit of insoluble calcium salts, mainly calcium carbonate. It occurs in the formation of bone and in the development of shells in marine organisms.

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14
Q

concentrated solution

A

Concentrated solution- A solution that has a relatively high ratio of solute to solvent.

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15
Q

concentration

A

Concentration- A measure of how much solute is dissolved in a specified volume of solution.

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16
Q

conjugate acid

A

Conjugate acid- The conjugate acid of a base contains one more hydrogen ion (proton) than the base, e.g. HCl is the conjugate acid of Cl-.

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17
Q

conjugate acid-base pair

A

Conjugate acid-base pair- An acid and its conjugate base. The conjugate base contains one less hydrogen ion (proton) than the acid.

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18
Q

conjugate base

A

Conjugate base- The conjugate base of an acid contains one less hydrogen ion (proton) than the acid, e.g. Cl- is the conjugate base of HCl.

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19
Q

decalcification

A

Decalcification- The removal or loss of calcium or calcium compounds.

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20
Q

diprotic acid

A

Diprotic acid- An acid that can ionise in water to form two H3O+ ions.

21
Q

dissociate

A

to break up

22
Q

greenhouse effect

A

Greenhouse effect- The warming of the earths atmosphere due to the absorption of infrared radiation by gases such as carbon dioxide, water and methane.

23
Q

hydronium ion

A

Hydronium ion- The H3O+(aq) ion.

24
Q

hydroxide ion

A

Hydroxide ion- The OH-(aq) ion.

25
Q

indicator

A

Indicator- A substance that is different colours in its acid and base forms.

26
Q

ionic equation

A

Ionic equation- An equation for a reaction that only includes the ions that are involves in the reaction.

27
Q

ionisation

A

Ionisation- (i) the removal of one or more electrons from an atom or ion; (ii) the reaction of a molecular substance with a solvent to form ions in solution.

28
Q

ionisation constant of water

A

Ionisation constant of water- The equilibrium constant KW, where KW = [H3O+][OH-]. At 25OC, KW = 1.00 x 10-14 M2.

29
Q

ionisation reaction

A

Ionisation reaction- The reaction of an acid or base with water.

30
Q

ionise

A

Ionise- The reaction of a molecular substance with a solvent to form ions in solution. When some polar molecules dissolve in water they ionise to form a hydronium ion, e.g. HCl(g) + H2O(l)  H3O+(aq) + Cl-(aq).

31
Q

limewater test

A

Limewater test- A test for carbon dioxide gas. The presence of carbon dioxide is detected by bubbling the gas through a calcium hydroxide solution (Ca(OH)2(aq)). The limewater reacts with the carbon dioxide and turns milky.

32
Q

monoprotic acid

A

Monoprotic acid- An acid molecule that generates only one hydronium ion when ionised in water.

33
Q

natural indicator

A

Natural indicator- An indicator that can be found in plants, such as red cabbage, turmeric, cherries, beetroot and grape juice. Like commercial indicators, natural indicators can be used to determine whether a substance is acidic or basic.

34
Q

natural solution

A

Neutral solution- A solution in which the concentrations of H3O+ ions equals the concentration of OH- ions; is neither acidic nor basic. At 25OC, a neutral solution has a pH of 7.

35
Q

neutralization reaction

A

Neutralization reaction- An acid reacts with a base in stoichiometric proportions to form a salt plus water.

36
Q

ocean acidity

A

Ocean acidity- The reduction in the pH of the ocean caused mainly by absorption of atmospheric carbon dioxide.

37
Q

pH

A

pH- A measure of acidity and the concentration of hydronium ions, in solution. Acidic solutions have a pH value less than 7 at 25OC, and bases have a pH value greater than 7 (at 25OC). Mathematically, pH is defined as pH = -log10[H3O+).

38
Q

polyprotic acid

A

polyprotic acid- An acid molecule that generates more than one hydronium ion when ionised in water.

39
Q

precision

A

precision- A measure of the repeatability or reproducibility of scientific measurements and refers to how close two or more measurements are to each other.

40
Q

salt

A

salt- A substance formed from a metal or ammonium cation and an anion. Salts are the products of reactions between acids and bases, metal oxides, carbonates and reactive metals.

41
Q

saturated solution

A

saturated solution- A solution that cant dissolve any more solute at the given temp.

42
Q

self-ionisation

A

self-ionisation- An ionisation reaction of pure water I which water behaves as both an acid and a base.

43
Q

spectator ion

A

spectator ion- An ion that remains in solution and is unchanged in the course of a reaction. Spectator ions aren’t included in ionic equations.

44
Q

strong acid

A

strong acid- An acid that readily donates a hydrogen ion (proton) to a base.

45
Q

strong base

A

strong base- A base that readily accepts a hydrogen ion (proton) from an acid.

46
Q

triprotic acid

A

triprotic acid- An acid molecule that generates 3 hydronium ions when ionised in water.

47
Q

weak-acid

A

weak acid- an acid that is partly ionised in water.

48
Q

weak base

A

weak base- A base that accepts hydrogen ions (protons) from acids to a limited extent.

Chemistry 1/2 (31 decks)

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