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1. Q: Name this compound: 2. Q: Write the formula for 3. Q: What is the formula for
H3PO3 permanganic acid. ammonia?
4. Q: What is the name of 5. Q: What is the formula for 6. Q: What is the formula for
H2C2O4? chromic acid? phosphoric acid?
8. Q: What is the formula of
7. Q: What is the name of H2S? 9. Q: What is the name of HF?
hydroiodic acid?
11. Q: A volume of 20.00 mL of a
solution of HNO3 having an
10. Q: What volume of a 1.366M
unknown concentration is titrated
solution of NaOH would be 12. Q: What is the pH of a 0.0825
with 34.37 mL of a 0.8220M
required to titrate 47.22 mL of a M solution of HBr?
solution of NaOH. What is the
2.075M solution of H2SO4?
concentration of the HNO3
solution?
13. Q: Determine the H3O+
14. Q: What is the concentration 15. Q: What does "diprotic"
concentration in a solution of pH
of OH- ions in a neutral solution? mean?
8.83.
17. Q: Is the following molecule
16. Q: Give an example of a 18. Q: Bases accept H+ and
monoprotic, diprotic, or triprotic?
triprotic acid. become ___________ acids.
CH3COOH
20. Q: In the following reaction,
19. Q: In the following reaction, identify the acid and the base, 21. Q: What is the term for a
identify the conjugate acid and using the Bronsted-Lowry substance that is considered both
base: definition. an acid and a base according to
NH3 + H2O <--> NH4+ + OH- H3PO4 + NO2- <--> HNO2 + the Bronsted-Lowry definition?
H2PO4-
23. Q: Write the chemical
22. Q: Name one amphoteric 24. Q: Write the equilibrium
equation showing the self-
substance. expression for Kw.
ionization of water.
27. Q: If [OH-] = 6.0 x 10 -3 M,
25. Q: What is the pOH of a 26. Q: What formula do you use
what is the concentration of
solution with a pH of 4? to find pOH?
[H3O+]?
29. Q: Write the Ka expression for
28. Q: What is the abbreviation the following reaction: 30. Q: What is the pOH of a
for the acid ionization constant? H2O (l) + CH3COOH (aq) <--> solution of 3.00 x 10 -5 M HCl?
H3O+(aq) + CH3COO- (aq)
31. Q: In a neutralization reaction,
33. Q: Titration is used to find
an acid and a base react to 32. Q: H2SO4 + Ba(OH)2 --> ?
what?
produce __________?
34. What is the point in a titration 35. Q: If you reach the
when the amount of added base equivalence point using 36. Q: If the pH of your solution is
exactly equals the amount of acid phenolphthalein indicator, what 5.2, what is the [H3O+]?
or base originally in the solution? color will your solution be?
37. Q: In a titration, what do you 39. Q: If a solution has a
38. Q: If a solution has a pH of 2,
call the solution with the known concentration of 7.4, is it an acid, a
is it an acid, a base, or neutral?
concentration? base, or neutral?
40. Q: If a solution has a 41. Q: A solution with equal
42. Q: What is the name of
concentration of 7, is it an acid, a concentrations of of OH-, and
H3O+?
base, or neutral? H3O+ is called __________?
43. Write the Kb (base ionization
constant) expression for the
following reaction:
NH3(g) + H2O(l) <--> NH4+(aq) +
OH-(aq)
3. A: NH3 2. A: HMnO4 1. A: Phosphorous acid
6. A: H3PO4 5. A: H2CrO4 4. A: Oxalic acid
9. A: hydroflouric acid 8. A: HI 7. A: Hydrosulfuric Acid
12. A: 1.08 11. 1.413M HNO3 10. A: 143.5 mL
15. A: Refers to an acid that will
donate two H+ ions per molecule 14. A: [OH-] = 1x10 -7 13. A: 1.48 x 10 -9 M
when dissolved in water.
17. A: monoprotic, it splits into
18. A: conjugate CH3COO- and H+ (only one 16. A: H3PO4, H3PO3
hydrogen splits off)
20. A: acid - H3PO4 19. A: Conj. Acid - NH4+
21. A: amphoteric
base - NO2- Conj. Base - OH-
24. A: Kw = [H+][OH-]
or 23. A: 2H2O <--> H3O+ + OH- 22. A: water, ammonia
Kw = [H3O+][OH-]
25. A: 10
27. A: 1.7 x 10 -12 M 26. A: pOH = -log[OH-]
(pH + pOH = 14)
29. A: Ka =
30. A: 9.48 [H3O+][CH3COO-] 28. A: Ka
[CH3COOH]
33. A: The concentration of an
32. A: H2O + BaSO4 31. A: water and a salt
acid or a base.
36. A: 6.3 x 10 -6 M 35. A: Light pink 34. A: equivalence point
39. A: base 38. A: acid 37. A: standard solution
42. A: hydronium ion 41. A: neutral 40. Neutral
43. A: Kb =
[NH4+][OH-]
[NH3]
