Acid%20and%20Base%20Review%20Game

1
Acid and Base Review Game

• Chemistry

2
Name the Acid

• HNO2
• Nitrous Acid
• H2SO4
• Sulfuric Acid
• HCl
• Hydrochloric Acid
• HBr
• Hydrobromic Acid
• HClO
• Hypochlorous Acid

3
Name the Base

• NaOH
• Sodium Hydroxide
• Ca(OH)2
• Calcium Hydroxide
• Mg(OH)2
• Magnesium Hydroxide
• KOH
• Potassium Hydroxide

4
Write the Formula

• Nitric Acid
• HNO3
• Hydroiodidic Acid
• HI
• Phosphoric Acid
• H3PO4
• Acetic Acid
• HC2H3O2

5
Write the Formula

• Sodium carbonate
• Na2CO3
• Barium hydroxide
• Ba(OH)2
• Lithium hydroxide
• LiOH

6
Arrhenius

• What is the definition of an acid?
• A substance which produces H when put in water
• What is the definition of a base?
• A substance which produces OH- when put in water

7

• If a soap has a hydrogen ion concentration of
  2.0 x 10-6 M, what is the pH of the solution?
  The pOH? Is it an acid or a base?
• H 2 x 10-6M pH -log(2 x 10-6) 5.7
• pOH 14 5.7 8.3
• Acid because pH lt 7

8

• What is the hydrogen ion concentration and
  hydroxide ion concentration of a solution with a
  pH of 2.3? Is the substance an acid or base?
• H 10-2.3 0.005 M
• pOH 14 2.3 11.7
• OH- 10-11.7 2 x 10-12 M
• Acid because pH lt 7

9

• What is the hydrogen ion concentration of a
  sample of phosphoric acid that has a pH of 4.9?
  What is the concentration of phosphoric acid?
• H 10-4.9 1.3 x 10-5M
• Since there are 3 Hs in each H3PO4 the
  concentration of phosphoric acid would be a third
  of the concentration of H
• 1.3 x 10-5/3 4.2 x 10-6 M

10
Neutralization Reaction

• What is the neutralization reaction for nitrous
  acid reacting with potassium hydroxide?
• HNO2 KOH ? KNO2 H2O

11
Neutralization Reaction

• Write the complete balanced equation for the
  neutralization of phosphoric acid with calcium
  hydroxide
• 2H3PO4 3Ca(OH)2 ? Ca3(PO4)2 6H2O

12

• How many grams of copper (II) sulfate
  pentahydrate will be needed to make 75 mL of a
  0.250 M solution?
• CM n/V
• .25 n/0.075
• n 0.01875 mol x 249.5 4.7 g

13

• How many kilograms of sucrose C12H22O11 will be
  needed to make 3.50 L of a 1.15 M solution?
• CM n/v
• 1.15 n/3.5
• n 4.025 mol x 342 1376.55 g / 1000 1.38 kg

14

• What is the pH of a solution made with 0.15 grams
  of barium hydroxide in 4500 mL of water?

15

• What is the molar concentration of a solution
  that contains 0.0750 moles of NaHCO3 in a volume
  of 115 mL
• CM n/v
• CM 0.075/.115 0.65 M

16

• A solution has 3.00 moles of solute in 2.00 L of
  solution, what is its molar concentration? How
  many moles would there be in 350 mL of solution?
• CM n/V
• CM 3/2 1.5M
• 1.5 n/0.35
• n 0.53 mol

17

• Describe in your own words how you would prepare
  1.00L of a 0.85 M solution of formic acid HCO2H?
• CM n/v
• 0.85 n/1
• n 0.85 mol x 46 39.1 g
• Take 39.1 grams of formic acid and dissolve in a
  little bit of water. Put into a 1.00 L
  volumetric flask and fill to the line with water

18

• What is the molarity of a sulfuric acid solution
  which contains 5.4 grams of sulfuric acid in 250
  mL of water? What is the normality?
• 5.4g/98 0.055 mol
• CM 0.055/0.25 0.22 M
• N (eq)M 2 x 0.22 0.44 N

19

• What is the molarity of a potassium hydroxide
  solution which contains 0.94 moles of potassium
  hydroxide in 450 mL of water? What is the
  normality?
• CM 0.94/0.45 2.1 M
• N (eq)M 1 x 2.1 2.1 N

20

• In the titration of 35 mL of liquid drain cleaner
  containing NaOH, 50 mL of 0.4M HCl must be added
  to reach the equivalence point. What is the
  molarity of the base in the cleaner?
• NaVa NbVb
• (0.4)(50) Nb(35)
• Nb 0.57 N / 1 0.57 M

21

• Calculate how many milliliters of 0.25 M Ba(OH)2
  must be added to titrate 46 mL of 0.40 M HClO4
• NaVa NbVb
• 0.4(46) 0.5Vb
• Vb 36.8 mL

22

• A 15.5 mL sample of 0.215 M KOH was titrated with
  an acetic acid solution, It took 21.2 mL of the
  acid to reach the equivalence point. What is the
  molarity of the acetic acid?
• (0.215)(15.5) Na(21.2)
• Na 0.157 N / 1 0.157 M

23

• What is the molarity of a solution of phosphoric
  acid with a pH of 2.65?
• 10-2.65 0.0022M / 3 7.62 x 10-4 M

24

• A 20 mL sample of an HCl solution was titrated
  with 27.4 mL of a standard solution of Ba(OH)2.
  The concentration of the standard is 0.0154 M.
  What is the molarity of the HCl?
• (0.0308)(27.4) Na(20)
• Na 0.042N / 1 0.042M

25
Buffer

• What is a buffer?
• A solution that resists changes in pH

26
Buffer

• What are buffers made of? Where can you find
  them?
• Weak acid and its conjugate base
• Weak base and its conjugate acid
• You can find them in your BLOOD

27

• I want to dilute 20 mL of a 6M solution of acetic
  acid to a 3.8M solution of acetic acid. How much
  water should I add to the 6M acetic acid to
  achieve this?
• 6(20) 3.8V
• V 31.6 mL
• ADD 11.6 mL of water

28

• I mix 20 mL of 4.5M NaCl with 40 mL of water.
  What is the new concentration of the NaCl?
• 4.5(20) M(60)
• M 1.5 M

29

• A 450 mL solution of 1.5 M HCl is sat out over
  night. 150 mL of the water evaporated. What is
  the new concentration of the HCl?
• 1.5 (450) M (300)
• 2.25 M

30

• What does the term strong acid mean?
• Strong acid means that the acid dissociates
  completely in water

31

• I used 50 grams of potassium chromate to make a
  1.4M solution. What is the volume of the
  solution?
• 50 g K2CrO4 / 194 0.26 mol
• 1.4 .26/v
• V 0.184 L

32

• What is the pH of a solution made by putting 6.0
  grams of phosphoric acid in 250 L of water?
• 6 g H3PO4 / 98 0.0612 mol
• H3PO4 0.0612 / 250 2.45 x 10-4
• H 3(2.45 x 10-4) 7.35 x 10-4
• pH -log(7.35 x 10-4) 3.13

33

• What is the pH of a solution made by putting 3.25
  grams of strontium hydroxide in 5000 L of water?
• 3.25 g Sr(OH)2 / 121.6 0.0267 mol
• Sr(OH)2 0.0267/ 5000 5.34 x 10-6M
• OH- 2(5.34 x 10-6) 1.07 x 10-5 M
• pOH -log(1.07 x 10-5) 4.97
• pH 14 4.97 9.03