Unit 9 - Acids & Bases

Question 1

Strong Acid

Answer 1

Completely dissociates.

Question 2

Weak Acid

Answer 2

Weak acids are not fully ionized or dissociated.

Question 3

Properties of Acids

Answer 3

Sour

Question 4

Properties of Bases

Answer 4

Bitter and slippery

Question 5

Acids

Answer 5

Electron acceptors.

Yeild H+ Ions in solution.

H+ donor.

Question 6

Bases

Answer 6

Electron donator.

Yeilds OH- in solution.

H+ Ion acceptor.

Question 7

NEUTRALIZATION REACTION

Answer 7

When an acid and base react in solution to form salt and water.

Question 8

Titration

Answer 8

The process of adding a known amount of solution of known concentration to determine the concentration of another solution.

Question 9

Products of an acid/base reaction

Answer 9

Salt + Water

Question 10

STANDARD SOLUTION

Answer 10

Solution of known concentration

Question 11

END POINT

Answer 11

When the indicator changes color.

Question 12

Titration Curve

Answer 12

Question 13

Amphoteric

Answer 13

Acid or Base

Question 14

pH, pOH, [H+], [OH-] Calculation Road Map

Answer 14

Question 15

pH Scale

Answer 15

pH = (-) log [H+]

pOH = - log [OH-]

pH + pOH = 14

[H+] = 2nd Log (-) pH

[OH-] = 2nd Log (-) pOH

[H+] [OH-] = 1E-14

Question 16

If the [H+] =1E-5 in a Coca-Cola what is the concentration of [OH-]? Is the solution acidic, basic, or neutral?

Answer 16

[H+] [OH-] = 1E-14

[OH-] = (1E-14) / ([H+])

[OH-] = (1E-14) / (1E-5)

[OH-] = 1E-9

The solution is acidic because 1E-5 is less than 1E-7.

Question 17

Determine the conjugate acid/base pairs.

NH₃ + H₂O —> NH₄⁺ + OH^-

Answer 17

Question 18

Hydronium Ion

Answer 18

[H+]

Question 19

Hydroxide Ion

Answer 19

[OH-]

Question 20

How would you calculate the pH of a solution with a hydronium concentration of 1E-5 M?

Answer 20

pH = -log 1E-5 =5

Question 21

Calculate the pH of a solution with a Hydronium ion concentration of 1.3E-9 M

Answer 21

pH= -log(1.3E-9) =8.89