Acid, bases and salt & BUFFER SYSTEM

Question 1

most common and important compounds known. In the form of aqueous solutions, these compounds are key materials in both biochemical systems and the chemical industry.

Answer 1

acid, bases, salts

Question 2

Swedish chemist _____(1859–1927) proposed that acids and bases be defined in terms of the chemical species they form when they dissolve in water.

Answer 2

Svante August Arrhenius

Question 3

hydrogen-containing compound that, in water, produces hydrogen ions (H+ ions). The acidic species in Arrhenius theory is thus the hydrogen ion.

Answer 3

Arrhenius acid

Question 4

hydroxide-containing compound that, in water, produces hydroxide ions (OH- ions). The basic species in Arrhenius theory is thus the hydroxide ion. For this reason, Arrhenius bases are also called hydroxide bases

Answer 4

Arrhenius base

Question 5

examples of arrhenius acids, This ion is formed through an interaction between water and the acid when they are mixed.
-ionization

Answer 5

HNO3 (nitric acid) and HCl (hydrochloric acid)

Question 6

e process in which individual positive and negative ions are produced from a molecular compound that is dissolved in solution.

Answer 6

ionization

Question 7

examples of arrhenius base, are ionic compounds in the pure state. When these compounds dissolve in water, the ions separate to yield the OH- ions.
-dissociation

Answer 7

NaOH (sodium hydroxide) and KOH (potassium hydroxide).

Question 8

process in which individual positive and negative ions are released from an ionic compound that is dissolved in solution.

Answer 8

dissociation

Question 9

_____(1879–1947), a Danish chemist, and ______ (1874–1936), a British chemist, independently and almost simultaneously proposed broadened definitions for acids and bases — definitions that applied in both aqueous and nonaqueous solutions and that also explained how some non hydroxide-containing substances, when added to water, produce basic solutions.

Answer 9

Johannes Nicolaus Brønsted and homas Martin Lowry

Question 10

substance that can donate a proton (H+ ion) to some other substance.

Answer 10

Brønsted–Lowry acid

Question 11

substance that can accept a proton (H+ ion) from some other substance.

Answer 11

Brønsted–Lowry base

Question 12

An absolute structural requirement for a Brønsted–Lowry acid is the presence of a _____The generalized notation for a Brønsted–Lowry acid, is ___

Answer 12

hydrogen atom, HA

Question 13

An absolute structural requirement for a Brønsted–Lowry base is the ______ of electrons. This is the site where the coordinate covalent bond forms when an incoming proton (from an acid) is accepted by the base.

Answer 13

presence of lone pair

Question 14

a substance that can either lose or accept a proton and thus can function as either a Brønsted–Lowry acid or a Brønsted–Lowry base.

Answer 14

amphiprotic substance

Question 15

The absolute structural requirement for an amphiprotic substance is the _____. ___ is the most common amphiprotic substance.

Answer 15

presence of hydrogen atom and lone pair, water

Question 16

the equilibrium constant for the reaction of a weak acid with water
-It describes the likelihood of the compounds and the ions to break apart from each other.

Answer 16

acid ionization constant/ acid dissociation constant/ Ka

Question 17

ionic equation

Answer 17

HCI + KOH –> H20 + KCI

H+ +CI- +K + OH- —–> H20 + K+ + CI-

Question 18

ionic compound containing a metal or polyatomic ion as the positive ion and a nonmetal or polyatomic ion (except hydroxide) as the negative ion.

Answer 18

salt

Question 19

the chemical reaction between an acid and a hydroxide base in which a salt and water are the products.
(acid + base —> water + salt

Answer 19

acid-base neutralization

Question 20

an aqueous solution in which the concentration of H3O+ ion is higher than that of OH- ion. less than 7

Answer 20

acidic solution

Question 21

aqueous solution in which the concentration of the OH- ion is higher than that of the H3O+ ion. greater than 7

Answer 21

basic solution

Question 22

aqueous solution in which the concentrations of H3O+ ion and OH- ion are equal. equal to 7

Answer 22

neutral solution

Question 23

scale of small numbers that is used to specify molar hydronium ion concentration in an aqueous solution.

Answer 23

pH scale (power of hydrogen)

Question 24

an aqueous solution containing substances that prevent major changes in solution pH when small amounts of acid or base are added to it.

Answer 24

buffer

Question 25

Most human body fluids are highly buffered. For example, a buffer system maintains blood’s pH at a value close to___, an optimum pH for oxygen transport.

Answer 25

7.4

Question 26

Buffers contain two active chemical species:

Answer 26

(1) a substance to react with and remove added base and (2) a substance to react with and remove added acid.

Question 27

, a buffer system is composed of a weak acid and its conjugate base

Answer 27

a conjugate acid–base pair

Question 28

contain either a weak acid and a salt of that weak acid or a weak base and a salt of that weak base. weak acid = salt of weak acid weak base = salt of weak base

Answer 28

buffer solutions

Question 29

HCl and NaCl

Answer 29

No. An acid and the salt of that acid are present. However, the acid is a strong acid rather than a weak acid.

Question 30

HCN and KCN

Answer 30

Yes. HCN is a weak acid, and KCN is a salt of that weak acid.

Question 31

HCl and HCN

Answer 31

No. Both HCl and HCN are acids. No salt is present.

Question 32

NaCN and KCN

Answer 32

No. Both NaCN and KCN are salts. No weak acid is present.

Question 33

results from lower than normal levels of HCO3- ion in the blood. Causes include severe diabetes and severe diarrhea.

Answer 33

metabolic acidosis

Question 34

results from higher than normal levels of HCO3- in the blood. This condition, less common than metabolic acidosis, can be caused by prolonged vomiting and is also a side effect of certain drugs that, like vomiting

Answer 34

metabolic alkalosis

Question 35

results from higher than normal level of CO2 in the blood. Hypoventilation (a lowered breathing rate), caused by lung diseases such as emphysema and asthma or obstructed air passages, produces respiratory acidosis.

Answer 35

respiratory acidosis

Question 36

results from lower than normal levels of CO2 in the blood. Causes include hysteria and anxiety (brought on, for example, by chemistry exams) and a high fever.

Answer 36

Respiratory alkalosis

Question 37

substance whose aqueous solution conducts electricity. The presence of ions (charged particles) explains the electrical conductivity.

Answer 37

electrolytes

Question 38

is a substance whose aqueous solution does not conduct electricity. eg: table sugar (sucrose), glucose, and isopropyl alcohol, do not produce ions in solution.

Answer 38

nonelectrolyte

Question 39

strong electrolytes

Answer 39

sodium hydroxide, sodium chloride, hydrochloric acid

Question 40

weak electrolytes

Answer 40

acetic acid, water, ammonia

Question 41

non-electrolytes

Answer 41

sugar, alcohol, oil

Question 42

substance that completely (or almost completely) ionizes/dissociates into ions in aqueous solution. All strong acids and strong bases and all soluble salts are strong electrolytes.

Answer 42

strong electrolytes

Question 43

a substance that incompletely ionizes/dissociates into ions in aqueous solution. produce solutions that are intermediate between those containing strong electrolytes and those containing nonelectrolytes in their ability to conduct an electric current.

Answer 43

weak electrolytes

Question 44

For every kilogram of its mass, the body contains about ____mL of intracellular fluid, ____mL of interstitial fluid, and ___0 mL of blood plasma.

Answer 44

400, 160, 40

Question 45

main component of any type of body fluid.

Answer 45

water

Question 46

a major factor in controlling water movement, is directly related to electrolyte concentration gradients.

Answer 46

osmotic pressure

Question 47

The electrolytes present in body fluids

Answer 47

(1) govern the movement of water between body fluid compartments and (2) maintain acid–base balance within the body fluids.

Question 48

essential for basic life functioning, such as maintaining electrical neutrality in cells and generating and conducting action potentials in the nerves and muscles.

Answer 48

electrolytes

Question 49

5 signs of chemical reaction

Answer 49

change in color change in odor production of new gases input or release of energy difficult to reverse

Question 50

number in front of reactants and products

Answer 50

stoichiometric coefficients

Question 51

substances exist before a chemical change takes place

Answer 51

reactants

Question 52

the new substances that are formed in chemical change

Answer 52

products

Question 53

one in which number of atoms of each element as reactant is equal to product

Answer 53

balanced equation

Question 54

mass relationships between substances in chemical reaction, based on mole ratio

Answer 54

stoichiometry

Question 55

indicated by coefficients in balanced equation

Answer 55

mole ratio