Acid Base Equilibria

Question 0

The Swedish chemist, (blank) defined (blank) as substances that produce H+ ions in water and (blank) as substances that produce OH- ions in water.

Answer 0

Svante Arrhenius, acids, bases

Question 1

(blank) comes from the Old English meaning of the word “to bring low”

Answer 1

base

Question 2

An (blank) is a substance that, when dissolved in water, increases the concentration of (blank) ions.

Answer 2

acid; H+

Question 3

A (blank) is a substance that, when dissolved in water, (blank) the concentration of (blank) ions.

Answer 3

base; increases; OH-

Question 4

A Danish chemist, (blank), and English chemist, (blank), proposed a more general concept.

Answer 4

Johannes Bronsted; Thomas Lowry

Question 5

A hydrogen ion is no more than a lone (blank).

Answer 5

proton

Question 6

What is the equation of a hydronium ion?

Answer 6

H3O+

Question 7

The notation (blank) also is interchangeable for H3O+.

Answer 7

H+(aq)

Question 8

According to Bronsted-Lowry, a (blank) is a substance that (blank) a proton.

Answer 8

base; accepts

Question 9

According to Bronsted-Lowry, an acid is a substance that (blank) a (blank).

Answer 9

donates; proton

Question 10

An acid and a base always work together to transfer a (blank).

Answer 10

proton

Question 11

Any acid or base that differ only in the presence or absence of a proton are called a (blank) pair.

Answer 11

conjugate acid-base

Question 12

A strong (blank) completely transfers its protons to water.

Answer 12

acid

Question 13

A (blank) acid partially dissociates in aqueous solution.

Answer 13

weak

Question 14

The stronger an acid is, the weaker its (blank) will be.

Answer 14

conjugate base

Question 15

We can categorize acids and bases according to their behavior in (blank).

Answer 15

water

Question 16

Substances with negligible acidity do not (blank) a (blank) to water.

Answer 16

donate; proton

Question 17

In pure water equilibrium is established and this process in termed (blank) of water.

Answer 17

autoionization

Question 18

At 25 degrees Celsius, the ion-product of water is 1.0 * (blank).

Answer 18

10^-14

Question 19

The molar concentration of H+(aq) in an aqueous solution is usually very small. Therefore we express H+ in terms of (blank), which is the negative logarithm in a base of 10.

Answer 19

pH

Question 20

In biological systems many reactions require (blank) transfers. Therefore the (blank) of fluids is critical.

Answer 20

proton; pH

Question 21

Human blood has a normal pH range of (blank) to (blank).

Answer 21

7.35; 7.45

Question 22

A Lewis acid is an electron-pair (blank).

Answer 22

acceptor

Question 23

A Lewis base is an electron-pair (blank).

Answer 23

donor

Question 24

Ka is called the (blank).

Answer 24

acid-dissociation constant

Question 25

The most common soluble strong bases are the ionic (blank) of the (blank) metals.

Answer 25

hydroxides; alkali

Question 26

Strong acids are also strong (blank).

Answer 26

electrolytes

Question 27

3 common acid-base indicators:

Answer 27

methyl red; bromthymol blue; phenolphthalein

Question 28

5 common bases

Answer 28

sodium hydroxide NaOH; potassium hydroxide KOH; calcium hydroxide Ca(OH)2; sodium bicarbonate NaHCO3; magnesium hydroxide Mg(OH)2

Question 29

5 common acids

Answer 29

nitric acid HNO3; sulfuric acid H2SO4; hydrochloric acid HCl; phosphoric acid H3PO4; acetic acid HC2H3O2