Acids and Bases

Question 1

What does an Arrhenius acid do?

Answer 1

It accepts protons/makes (H₃O⁺) in water.

Question 2

What does an Arrhenius base do?

Answer 2

It donates protons/makes OH^- in water.

Question 3

What is a hydronium ion?

Answer 3

H₃O⁺

Question 4

What is a hydroxide ion?

Answer 4

OH^-

Question 5

What is a Bronsted-Lowry acid?

Answer 5

A proton donor

Question 6

What is a Bronsted-Lowry base?

Answer 6

A proton acceptor

Question 7

What is a Lewis acid?

Answer 7

A proton acceptor

Question 8

What is a Lewis base?

Answer 8

A proton donor

Question 9

When is a solution concentrated?

Answer 9

When there are a lot of solute molecules in the system.

Question 10

When is a solution diluted?

Answer 10

When there are few solute molecules in the system.

Question 11

What is a polyprotic acid?

Answer 11

When an acid has more than one proton to donate (more than one H⁺).

Question 12

What is a conjugate acid?

Answer 12

What’s left after an acid donates it’s proton.

Question 13

What is a conjugate base?

Answer 13

What’s present after a base accepts the proton (or donated its hydroxide ion).

Question 14

What does “amphoteric” mean?

Answer 14

Species that can act as both acid and base (water is an example).

Question 15

What is the chemical reaction of autoionization of water?

Answer 15

H₂O –> H⁺ + OH^-

Question 16

What is the water dissociation constant?

Answer 16

K_w=1•E^-14. Equilibrium constant for autoionization of water.

Question 17

What is pH?

Answer 17

A logarithmic scale of acidity.

Question 18

What is a buffer?

Answer 18

Weak acid or base and its conjugate that resists changes in pH when acid or bases are added.

Question 19

What is titration?

Answer 19

When a known concentration solution reacts with an unknown concentration to determine concentration.

Question 20

What is an end point (or stoichiometric point)?

Answer 20

When all reactants have reacted in a titration—no left-over of any reactants.

Question 21

What does an indicator do?

Answer 21

Changes color at a certain pH.

Question 22

What is a titration curve?

Answer 22

Graph of pH versus volume of known solution.

Question 23

What is the pH level (range) of acids?

Answer 23

pH is less than 7.

Question 24

What is the pH level (range) of bases?

Answer 24

pH is more than 7.

Question 25

What are the strong acids (7)?

Answer 25

HCl, HBr, HI, HNO₃, HClO₃, HClO₄, H₂SO₄.

Question 26

What are two characteristics of acids?

Answer 26

Always contain H⁺ in chemical compound and turns litmus red.

Question 27

What are two characteristics of bases?

Answer 27

Always contains OH^- in chemical compound and turns litmus blue.

Question 28

When are acids weak?

Answer 28

When they aren't one of the 7 strong acids.

Question 29

What the the strong bases (8)?

Answer 29

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂.

Question 30

When are bases weak?

Answer 30

When they aren't one of the 8 strong bases.

Question 31

For polyprotic acids, each successive proton is \_\_\_?

Answer 31

Weaker than the one before.

Question 32

For strong acids, assume \_\_\_.

Answer 32

That [H⁺] = the concentration of the acid.

Question 33

For strong bases, assume \_\_\_.

Answer 33

That [OH^-] = the concentration of the base.

Question 34

What kind of salt forms from WEAK ACID + STRONG BASE?

Answer 34

BASIC salt.

Question 35

What kind of salt forms from WEAK ACID + WEAK BASE?

Answer 35

NEUTRAL salt.

Question 36

What kind of salt forms from STRONG ACID + WEAK BASE?

Answer 36

ACIDIC salt.

Question 37

What kind of salt forms from STRONG ACID + STRONG BASE?

Answer 37

NEUTRAL salt.

Question 38

For a strong acid, there must be \_\_\_.

Answer 38

A weak conjugate base.

Question 39

For a weak acid, there must be \_\_\_.

Answer 39

A strong conjugate base.

Question 40

For a strong base, there must be \_\_\_.

Answer 40

A weak conjugate acid.

Question 41

For a weak base, there must be \_\_\_.

Answer 41

A strong conjugate acid.