acid base chemistry

Question 1

What does Bronsted-Lowry theory describes?

Answer 1

acid-base interaction in terms of proton transfer between chemical species.

Question 2

What is a Bronsted-Lowry acid?

Answer 2

A proton donor

Question 3

What is a Bronsted-Lowry base?

Answer 3

A proton receiver

Question 4

What is an acid base reaction?

Answer 4

Any reaction involves a proton transfer from an acid to a base.

Question 5

What is an amphoteric substance?

Answer 5

A substance that can act as Bronsted-Lowry acid or base

Question 6

What are strong acids and bases?

Answer 6

Any species that dissociates completely into its constituent ions in aqueous solution.

Question 7

What are the common strong acids?

Answer 7

HCl, HBr, HI, H2SO4, HNO3, HClO4

Question 8

What are the common strong bases?

Answer 8

Group 1 and 2 metal hydroxide (LiOH, NaOH, KOH, Ca(OH)2, RbOH, Sr(OH)2, CsOH, Ba(OH)2 ) Little Nannies Kill Rabbits Causing Carnivorous Screaming Babies

Question 9

What are conjugate acids or base?

Answer 9

An acid after donating a proton becomes a conjugate base; a base after receiving a proton becomes a conjugate acid.

Question 10

What is autoionization, or self-ionization of water?

Answer 10

Water molecules exchange protons with one another to a very small extent

Question 11

What is pure water?

Answer 11

Pure water means water with no other compounds dissolved in the water.

Question 12

What is Kw?

Answer 12

Autoionization constant, which is equal to 10^-14 at 25 degree Celsius

Question 13

How can an aqueous solution be acidic?

Answer 13

[H3O] > [OH]

Question 14

How can an aqueous solution be basic?

Answer 14

[OH] > [H3O]

Question 15

How can an aqueous solution be neutral

Answer 15

[H3O] = [OH]

Question 16

What does Le Chatelier’s principle tell us?

Answer 16

The reaction will shift to counteract the change in concentration and establish a new equilibrium.

Question 17

What are always true for any aqueous solutions at 25 degree Celsius?

Answer 17

Kw= [H3O].[OH] = 10^-14

pH + pOH = 14

Question 18

What is an Arrhenius acid?

Answer 18

​An Arrhenius acid is any species that increases the concentration of H+ in aqueous solution.

Question 19

What is an Arrhenius base?

Answer 19

​An Arrhenius base is any species that increases the concentration of OH- in aqueous solution.

Question 20

What does pH stand for?

Answer 20

The abbreviation pH stands for potential hydrogen.

Question 21

What is the alkalinity of any species?

Answer 21

It is the capability to resist changes in [H+] that would make the water more acidic.

Question 22

What are acidic and alkaline molecules?

Answer 22

​An acidic molecule would have a low ability to attract hydrogen ions, while an alkaline molecule would have a high ability to attract hydrogen ions.

Question 23

What does “p” in pH and pOH stand for?

Answer 23

​The lowercase p indicates “-log”.

Question 24

What is molarity?

Answer 24

The number moles of solute per liter of solution, can be written as “M”

Question 25

What is molality?

Answer 25

The number moles of solute per kilogram of solvent, can be written as “m”.

Question 26

What is the special thing about Bronsted-Lowry acid?

Answer 26

​Any Brønsted-Lowry acid must contain a hydrogen that can dissociate as H+.

Question 27

​What is the special thing about Bronsted-Lowry base?

Answer 27

​

Brønsted-Lowry base must have at least one lone pair of electrons to form a new bond with a proton.

Question 28

What is pKa

Answer 28

pKa is the negative base-10 logarithm of the acid dissociation constant (Ka) of a solution

Question 29

What is pKa?

Answer 29

pKa is the negative base-10 logarithm of the acid dissociation constant (Ka) of a solution.