Name______
Date______Per______
Chapter 20 Review Sheet—Regulars Test
1)List the general properties of acids and bases.
Acids: taste sour, form electrolytes, cause litmus paper to turn red
Bases: taste bitter, feel slippery, form electrolytes
2)When you combine an acid and a base, what are the products? What is this called?
ACID + BASE → SALT + WATERThis is called a neutralization reaction.
3)Describe the system for naming acids, including how the endings change based on the ions.
Negative Ion:Acid Name:
_____ idehydro ____ic acid
_____ ite______ous acid
_____ ate______ic acid
4)What is an electrolyte?
An electrolyte is a compound that conducts electricity because it separates into ions in solution.
5)Give the definition for an acid and a base for the Lewis, Bronsted-Lowry and Arrhenius theories.
Arrhenius: acid – gives off Hydrogen ions in solution
base – gives off Hydroxide ions in solution
Bronstead-Lowry: acid – donates a hydrogen ion (proton donor)
base – accepts a hydrogen ion (proton acceptor)
6)What are the definitions of a conjugate acid and a conjugate base?
conjugate acid – the particle formed when a base gains a hydrogen ion
conjugate base – the particle formed when an acid donates a hydrogen ion
7)What does amphoteric mean?
An amphoteric substance can act as either an acid or a base. Ex) water
8)Describe the pH and pOH scales.
The pH scale goes from 0 – 14. Strong acids are close to 0 and strong bases are close to 14. Both weak acids and weak bases are near 7. Neutral substances have a pH of 7.0. pOH = 14 – pH
9)What is the difference between strong acids/bases and weak acids/bases?
Strong acids and strong bases completely dissociate (break apart) in solution, whereas weak acids and weak bases only partially dissociate in solution.
10)What is the difference between the words weak/strong and concentrated/dilute when referring to acids and bases?
Weak/Strong depends on the amount of dissociation (see #10).
Concentrated/Dilute depends on the molarity. Molarities of greater than 6 M are concentrated and less than 1 M is dilute.
11)Tell whether the following would be acidic or basic:
Apple juice acid
Bleach base
Milk acid
Detergent base
Tomatoes acid
Dr. Pepper acid
TUMS base
Vinegar acid
Something bitter base
Ammonia base
Comet® base
Something sour acid
12)Name the following acids and bases:
- HNO2 nitrous acid
- HBrO4 perbromic acid
- HF hydrofluoric acid
- Ca(OH)2 calcium hydroxide
- HClOhypochlorous acid
- H2C2O4 oxalic acid
- KOH potassium hydroxide
- H3PO3 phosphorous acid
- H2SO4 sulfuric acid
- HIO2 iodous acid
13)Write the formula for the following acids or bases:
- Hydrobromic acidHBr
- Sulfurous acidH2SO3
- Hydrocyanic acidOMIT
- Tartric acidOMIT
- Aluminum hydroxideAl(OH)3
- Carbonic acidH2CO3
14)Tell whether the following acids are Monoprotic, Diprotic or Triprotic:
- HNO3monoprotic
- H2CO3diprotic
- HC2H3O2 monoprotic
- H3PO4triprotic
- H2SO4diprotic
- HBrO3 monoprotic
15)For the reactions, label the acid, base, conjugate acid and conjugate base:
HCl + H2O H3O+ + Cl-
Initial acid: HCl
Initial base: H2O
Conjugate acid: H3O+
Conjugate base: Cl-
NH3 + H2O NH4+ + OH-
Initial acid: H2O
Initial base: NH3
Conjugate acid: NH4+
Conjugate base: OH-
H2SO3 + NaHCO3 H2CO3 + NaHSO3 OMIT
CaCO3 + HNO3 Ca(NO3)2 + H2CO3 OMIT
16)Give the conjugate base for each of the following acids:
HNO2NO2-1
HC2H3O2 C2H3O2-1
HCl Cl-1
H3PO3 H2PO3-1
H2SO4 HSO4-1
NH4+ NH3
H3O+ H2O
HN3 N3-1
18) Give the conjugate acid for each of the following bases:
OH-H2OI-HI
NH3NH4+H2O H3O+
H2PO4- H3PO4HSO4- H2SO4
19)What is the [OH-] of a solution with a pOH of 9.7?
[OH-] = antilog –pOH[OH-] = antilog -9.7[OH-] = 2.0 x 10-10 M
20)What is the pOH of a solution with [H+]=3.1x10-9?
This is a two step problem. First, calculate the pH and then calculate pOH.
pH = - log [H+]pH = - log (3.1 x 10-9)pH = 8.5
pOH = 14 – pHpOH = 14 – 8.5pOH = 5.5
21)What is the [H+] of a solution with a pH of 5.12?
[H+] = antilog – pH[H+] = antilog –5.12[H+] = 7.6 x 10-6 M
22)What is the [H+] of a solution with a pOH of 10.3?
This is a two step problem. First, calculate the pH and then calculate [H+].
pH = 14 – pOHpH = 14 – 10.3pH = 3.7
[H+] = antilog – pH[H+] = antilog –3.7[H+] = 2.0 x 10-4 M
23)What is the pH of a solution with [H+]=3.2x10-13?
pH = - log [H+]pH = - log (3.2 x 10-13)pH = 12.5
24)What is the [OH-] of a solution with a pH of 4.7?
This is a two step problem. First, calculate the pOH and then calculate [OH+].
pOH = 14 – pHpOH = 14 – 4.7pOH = 9.3
[OH-] = antilog –pOH[OH-] = antilog -9.3[OH-] = 5.0 x 10-10 M
25)What is the pH of a solution with [OH-]=3.3x10-4?
This is a two step problem. First, calculate the pOH and then calculate pH.
pOH = - log [OH+]pOH = - log (3.3 x 10-4)pOH = 3.5
pH = 14 – pOHpH = 14 – 3.5pH = 10.5
26)What is the pOH of a solution with [H+]=8.1x10-14?
This is a two step problem. First, calculate the pH and then calculate pOH.
pH = - log [H+]pH = - log (8.1 x 10-14)pH = 13.1
pOH = 14 – pHpOH = 14 – 13.1pOH = 0.9
27)What is the pH of a solution with [OH-]=9.2x10-10?
This is a two step problem. First, calculate the pOH and then calculate pH.
pOH = - log [OH+]pOH = - log (9.2 x 10-10)pOH = 9.0
pH = 14 – pOHpH = 14 – 9.0pH = 5.0
28)What is the [H+] and [OH-] of a solution with a pH of 6.17?
[H+] = antilog – pH[H+] = antilog –6.17[H+] = 6.8 x 10-7 M
pOH = 14 – pHpOH = 14 – 6.17pOH = 7.83
[OH-] = antilog –pOH[OH-] = antilog -7.83[OH-] = 1.5 x 10-8 M
29)What is the pH and pOH of a solution with [OH-]=2.6x10-5?
pOH = - log [OH+]pOH = - log (2.6 x 10-5)pOH = 4.6
pH = 14 – pOHpH = 14 – 4.6pH = 9.4
30)What is the pH and pOH of a solution with [H+]=1.6x10-11?
pH = - log [H+]pH = - log (1.6 x 10-11)pH = 10.8
pOH = 14 – pHpOH = 14 – 10.8pOH = 3.2
31)What is the [H+] and [OH-] of a solution with a pOH of 11.07?
[OH-] = antilog –pOH[OH-] = antilog -11.07[OH-] = 8.5 x 10-12 M
pH = 14 – pOHpH = 14 – 11.07pH = 2.93
[H+] = antilog – pH[H+] = antilog –2.93[H+] = 1.2 x 10-3 M
32)Tell whether the following would be strong or weak acid or base:
NaOH strong baseH2SO4 strong acid
HClstrong acidHMnO4 weak acid
H2CO3weak acidNH4OH weak base
CuOHweak baseCa(OH)2 strong base
Fe(OH)3 weak baseHNO3 strong acid