Unit 13 marker board review
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Unit 13 Marker Board Review. Acids & Bases Made with love and care by. Question #1. List 4 properties of acids. Answer: 1 – Sour taste 2 – React with metals to form hydrogen gas 3 – React with metal carbonates to form CO 2 gas 4 – Turn indicators red. Question #2.

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Unit 13 Marker Board Review

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Unit 13 marker board review

Unit 13 Marker Board Review

Acids & Bases

Made with love and care by


Question 1

Question #1

List 4 properties of acids.

Answer:

1 – Sour taste

2 – React with metals to form hydrogen gas

3 – React with metal carbonates to form CO2 gas

4 – Turn indicators red


Question 2

Question #2

List 4 properties of bases.

Answer:

1 – Taste bitter

2 – Unreactive with metals and carbonates

3 – Feel slippery

4 – Turn indicator blue


Question 3

Question #3

According to Arrhenius, acids must contain _______ ions & bases must contain _______ ions.

Answer:

hydrogen

hydroxide


Question 4

Question #4

A Bronsted acid _____________ a _______________ and a base ______________ a ____________.

Answer:

- donates

- hydrogen ion

- accepts

- hydrogen ion


Question 5

Question #5

Label the Acid, Base, Conj Acid, Conj Base

  • NH3 + H2O  NH4+ + OH-

  • H2CO3 + H2O  H3O+ + HCO3-

Answer:

NH3 + H2O  NH4+ + OH-

B A CA CB

H2CO3 + H2O  H3O+ + HCO3-

A B CA CB


Question 6 acc only

Question #6 (Acc Only)

Base anhydrides contain a _________________ and oxygen.

Acid anhydrides contain a _________________ and oxygen.

Answer: Metal

Nonmetal


Question 7

Question #7

When an acid reacts with a base to neutralize it, the products are a _______________ & ___________.

Answer: Salt & Water


Question 8

Question #8

Pure water has a pH of _________ because …

Answer: 7…Because it is neutral!


Question 9

Question #9

Acids have a pH ___________ than 7; bases _____________ than 7.

Answer: Less

Greater


Question 10

Question #10

Write the name for the following formulas. Is it an acid or base?

Check your answers after you’ve written ALL of them!

  • HBr

  • NaOH

  • HNO2

  • HCN

  • NH3

  • H2SO4

  • Mg(OH)2

  • H2CO3

  • HC2H3O2

Hydrobromic Acid—acid

Sodium Hydroxide—base

Nitrous Acid—acid

Hydrocyanic Acid - acid

Ammonia—base

Sulfuric Acid—acid

Magnesium Hydroxide - base

Carbonic Acid—acid

Acetic Acid—acid


Question 11

Question #11

Write & balance the equation for the neutralization of sulfuric acid with potassium hydroxide.

Answer: H2SO4 + 2 KOH  2 H2O + K2SO4


Question 12

Question #12

Write & balance the neutralization reaction of hydrobromic acid & calcium hydroxide.

Answer:

2 HBr + Ca(OH)2 2 H2O + CaBr2


Question 13

Question #13

The formula for the hydronium ion is ____________________ & for the hydroxide ion _______________.

Answer: H30+& OH-


Question 14

Question #14

An H+ ion is really just a _______________ and cannot exist in solution.

Answer: Proton


Question 15

Question #15

Write the equation for the self-ionization of water.

Answer: H2O + H2O  OH- + H3O+


Question 16

Question #16

The formula for calculating [H3O+] from pH is ______________________. I type this into my calculator as: _________

Answer: [H3O+] = 10^(-pH)

2nd log (negative pH)


Question 17

Question #17

The formula for calculating [H3O+] from [OH-] is ______________________. I type this into my calculator as: _______

Answer: Kw = [OH-][H3O+] = 1.0 x 10-14

[H3O+] = 1.0 x 10-14

[OH-]

1.0 E -14 / [OH-]


Question 18

Question #18

  • List the formulas for pH, H+ concentration, pOH, & OH- concentration

Answer:

pH = -log [H+] OR 14 - pOH

[H+] = 10^(- pH) OR 1.0 x 10-14 / [OH-]

pOH = -log [OH-] OR 14 - pH

[OH-] = 10^(- pOH) OR 1.0 x 10-14 / [H3O+]


Question 19

Question #19

  • pH + pOH = ___________

  • Answer: 14


Question 20

Question #20

What is the pH of an HCl solution with a concentration of 0.0015 M?

  • Answer: pH = -log (0.0015) = 2.8


Question 21

Question #21

  • What is the pH of a solution with an pOH of 10.5?

Answer: pH = 14 – pOH = 14 – 10.5 = 3.5


Question 22

Question #22

  • What is the [H+] of a solution with a pH of 4.51?

Answer: [H+] = 10^(-4.51) = 3.09 x 10-5 M


Question 23

Question #23

  • What is the pOH of a solution with a [H+] of 9.99 x 10-9 M?

Answer: pOH = -log [OH-]

[OH-] = 1.0 x 10-14 / 9.99 x 10-9 = 1.0 x 10-6 M

pOH = -log(1.0 x 10-6) = 6.0


Question 24

Question #24

  • What is the pOH of a solution with an [OH-] of 7.81 x 10-3 M?

Answer: pOH = -log [OH-] = -log (7.81x10-3) = 2.1


Question 25

Question #25

  • Calculate the [OH-] if the pOH is 5.21.

Answer: [OH-] = 10^(-5.21) = 6.17 x 10-6 M.


Question 26

Question #26

What is the purpose of a titration? What is the role of an indicator in a titration?

Answer: A titration enables you to determine the concentration of a solution by reacting a known volume of the solution with a solution of known concentration.

An indicator changes color when the end point of the titration has been reached.


Question 27

Question #27

  • You add a substance to pure water and the pH rises from 7 to 9. What has happened to the concentration of H3O+? Is the substance added an acid or a base?

Answer: The concentration of H3O+ has decreased. The substance is a base.


Question 28

Question #28

  • In the titration of a strong acid with a strong base, what pH range should the indicator have?

Answer: 6-8


Question 29 provided by sam b s for your benefit

Question #29provided by Sam B.S for your benefit

  • In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluoric acid solution. What is the molarity of the hydrofluoric acid solution?

  • MHF = 0.5015M


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