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Chemistry Final Review

Total questions: 134

Worksheet time: 6hrs 0mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.

This orbital diagram represents

a)

Calcium

b)

Scandium

c)

Potassium

d)

Yttrium

3.

Which of the following is the correct Lewis Dot structure of Carbon?

a)

I

b)

II

c)

III

d)

IV

e)

V

4.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

5.

Look at this picture of Argon off the periodic table. Which of the following is true for this element?

a)

18 protons

b)

40 protons

c)

22 protons

d)

21.9 protons

6.

Where are electrons located in the atom?

a)

Nucleus

b)

Outside the nucleus in a cloud

c)

Outside the nucleus in fixed rings

d)

With the protons

7.

What electron configuration matches an Neon atom?

a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
8.

What is the shorthand electron configuration of Iodine?

a)

[Kr]5s24d105p6

b)

[Kr]5s24d106p6

c)

[Kr]5s25d106p6

d)

None of the above

9.

How is Lithium (Li) Classified based on its location on the periodic table?

a)

nonmetal

b)

an alkaline earth metal

c)

a transition metal

d)

an alkali metal

10.

The following shows 3 different types of electron configurations:

Element 1 = 1s22s22p63s23p64s1

Element 2= 1s22s22p63s23p64s2

Element 3= 1s22s22p63s1

Which would be the correct electron configuration for Ca?

a)

Element 1

b)

Element 2

c)

Element 3

11.

Which atom has the largest atomic radius?

a)

Be

b)

Mg

c)

Ca

d)

Sr

12.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

13.

What is the name of the group that contains Ar and Kr?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

14.

What is the name of the group of elements that includes Mg and Ca

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

15.

Which halogen is found in period 5?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

16.

Which Lewis Dot Diagram would represent Phosphorous ?

a)
b)
c)
d)
17.

What color of light does a hydrogen atom emit when an electron transitions from n=3 energy level to n=2 energy level?

a)

Yellow

b)

Orange

c)

Green

d)

Blue

18.

Which of the following has the lowest metallic character?

a)

Na

b)

Ca

c)

Ag

d)

As

19.

Which lists an alkaline earth metal, alkali metal, transition metal, and halogen in that order?

a)

Calcium, Lithium, Iron, Chlorine

b)

Magnesium, Titanium, Vanadium, Bromine

c)

Sodium, Nickel, Fluorine, Gallium

d)

Potassium, Calcium, Iron, Chlorine

20.
Which process involves the joining of small nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
21.
Arrange in order of increasing ability to penetrate matter.
a)
Beta, gamma, alpha
b)
Alpha, gamma, beta
c)
Gamma, beta, alpha
d)
Alpha, beta, gamma
22.

Which type of radiation can be stopped by clothing or paper?

a)

alpha

b)

beta

c)

gamma

d)

positron

23.

Which type of radiation has the shortest wavelength and can penetrate through our bodies?

a)

alpha

b)

beta

c)

gamma

d)

positron

24.

An element has two naturally occurring isotopes. One is 12 amu and is 19.9% abundant. The other is 13 amu and is 80.1% abundant. What is the average atomic mass?

a)

12.79 amu

b)

12.011 amu

c)

6.941 amu

d)

10.812 amu

25.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
26.
Solve this equation for alpha decay.
20985At = ___ + 42He
a)
20583Bi
b)
20986Rn
c)
20781Tl
d)
20885At
27.

 Balance the following nuclear equation:

           2658Fe + 201n ⟶    27   60Co +   ?\ \ \ \ \ \ \ \ \ \ \ _{26}^{58}Fe\ +\ 2_0^1n\ \longrightarrow\ _{\ \ \ 27}^{\ \ \ 60}Co\ +\ \ \ ?  


a)

   −1   0B\ \ \ _{-1}^{\ \ \ 0}B  

b)

   01n\ \ \ _0^1n  

c)

   11H\ \ \ _1^1H  

d)

   94238Am\ \ \ _{94}^{238}Am  

28.

Using the Bohr model of hydrogen in the reference packet, what color of light is given off by a hydrogen atom as its electron falls from n=5 to n=2 ?

a)

Yellow

b)

Red

c)

Green

d)

Blue

29.

When an electron falls from n=6 to n=2, what region of the electromagnetic spectrum does that wavelength occupy?

a)

radio

b)

gamma

c)

infrared

d)

visible

30.

How many valence electrons does Silicon (Si) have?

a)

3

b)

4

c)

5

d)

6

31.

The shorthand electron configuration  [Ne] 3s23p4 belongs to which element?

a)

Gallium

b)

Boron

c)

Aluminum

d)

Sulfur

32.

If 25 g of iodine 131 is given to a patient, how much is left after 40 days? The half-life of iodine-131 is 8 days.

a)

0.78g

b)
1.25g
c)

25g

d)

12.5g

33.

The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 75 years if the initial amount is 8.0 g?

a)
3.0g
b)

2 g

c)

4 g

d)

1 g

34.

The half life of radium 226 is 1602 years. If you have 200 grams of radium today how many grams would have been present 3204 years ago?

a)

2

b)

800

c)

400

d)

50

35.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper (I) bromide

d)

copper (II) bromide

36.

What is the name of the following compound: K2SO4

a)

potassium sulfur

b)

potassium sulfate

c)

potassium (I) sulfate

d)

potassium (II) sulfide

37.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
38.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
39.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

40.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
41.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

42.

Classify the following molecule.

a)

polar

b)

nonpolar

43.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

44.

Which of the following is polar?

a)

H2O

b)

CBr4

c)

H2

d)

O2

45.

Which of the following has a Bent shape?

a)

CF4

b)

HBr

c)

NH3

d)

H2S

46.

Which of the following is NONpolar?

a)

H2O

b)

CBr4

c)

HBr

d)

NH3

47.

What are phases (solubility) of the products for the following reaction:

CuCl2(aq) + NaOH(aq) → Cu(OH)2(??) + NaCl(??)  

a)

Cu(OH)2(aq) + NaCl(aq)  

b)

Cu(OH)2(aq) + NaCl(s)  

c)

Cu(OH)2(s) + NaCl(aq)  

d)

Cu(OH)2(g) + NaCl(s)  

48.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
49.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
50.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
51.
Which set of coefficients properly balances the reaction below?
_Cu + _H2O →_ CuO3 + _H2
a)
1,3,1,5
b)
2,6,2,6
c)
1,3,1,3
d)
1,2,3,4
52.
What are the correct coefficients for the reaction below?
_C4H10 + _O2 → _CO2 + _H2O
a)
4, 26, 16, 20
b)
2, 13, 8, 10
c)
1, 6.5, 4, 5
d)
2, 8, 13, 10
53.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
54.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

55.

Predict the products for the this Single Replacement reaction: (Copper has a charge of 1+)

Mg + CuCl →

a)

MgCl2 + Cu

b)

Mg + Cu

c)

MgCu + Cl2

d)

MgCl + Cu2

56.

What are the products of this reaction:

C2H4 + O2 →

a)

C2O2 + H4

b)

CO2 + H2 + O2

c)

CO + H

d)

CO2 + H2O

57.

Convert 87L to mL (1L=1000mL)

a)

87,000mL

b)

0.087mL

c)

0.000087mL

d)

87,000,000mL

58.

How many atoms are in 7.89 mol of magnesium? (1 mol = 6.022x1023 atoms)

a)

1.31 x 1023 atoms

b)

4.75 x 1023 atoms

c)

4.75 atoms

d)

1.31 atoms

59.

How many grams of sodium are in 8.93mol? (1 mol = 22.99g)

a)

205 g

b)

0.388 g

c)

31.92 g

d)

14.06 g

60.

A bicycle has a speed of 6.00 m/s. What is its speed in km/h? (1km=1000m) (1h= 3600s)

a)

21.6 km/h

b)

16.67 km/h

c)

2.16 km/h

d)

1.67 km/h

61.

Unit 9:Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.

a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
62.

Unit 9:Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 

a)
0 K 
b)
107 K 
c)
207 K 
d)

310 K 

63.

Unit 9:What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K? PV=nRT

a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
64.

Unit 9:You have a gas that has a pressure of 2 atm and a volume of 10L.  What would be the new volume if the pressure was changed to 1 atm? (temperature is constant)

a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
65.

Unit 9:A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?

a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
66.

Unit 9:A sample of oxygen at 28.0°C has 340.0 kPa. What will its temperature be at 150.0 kPa?

a)
132.8 K
b)
132.8 °C
c)
682.2 K
d)
12.35 K
67.

Unit 9:A mixture of H, Ne, & O has a pressure of 12.4 atm. If Hydrogen measures 5.6 atm and Oxygen measures 2.0 atm, what is the pressure of Neon?

a)

7.6 L

b)

4.8 L

c)

5.4 L

d)

12.0 L

68.

Unit 7:

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
69.

Unit 7:

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)
SO
b)
SO2
c)
SO3
d)
SO4
70.

Unit 7:

What is the percent by mass of magnesium in MgO?

a)
20%
b)
40%
c)
50%
d)
60%
71.

Unit 7:

What is the mass of 0.75 moles of (NH4)3PO4?

a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
72.

Unit 7:

What is the formula based off the following name:

Magnesium Carbonate pentahydrate 

a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
73.

Unit 7:

Name the following hydrate:  NaCl * 5H2O

a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
74.

Unit 7:

Find the percent composition of Cu2S?

a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
75.

Unit 8:

2 KClO3 → 2 KCl + 3 O2 How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?

a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
76.

Unit 8:

CH4 + 2 O2 → CO2 + 2 H2O How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?

a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
77.

Unit 8:

2Al + 3H2SO4 -> Al2(SO4)3 + 3H2

How many liters of aluminum sulfate would be formed if 25g H2SO4 completely reacted with aluminum?

a)

1.9L

b)

5. 00 L

c)

5.7 L

d)

10L

78.

Unit 8:

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the experimental yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

15.5

79.

Unit 8:

P4 + 6Cl2 --> 4PCl3  The reaction of 75.0g P4 reacts with chlorine gas. This reaction produces an experimental yield of 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 

a)
78%
b)
64%
c)
27%
d)
33%
80.

Unit 7

What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.

a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
81.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
82.
What phase change(s) may occur at pressures below 4.58 mmHg?
a)
sublimation/deposition
b)
melting/freezing
c)
all phase changes are possible at these pressures
d)
vaporization/condensation
83.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
84.

What is point B?

a)

Triple point

b)

Liquid point

c)

Critical Point

d)

Solid point

85.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

86.
The temperature of an unknown piece of metal with a mass of 30.00 g changes from 25.0 °C to 35.0 °C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?
a)
1.17 J/g°C
b)
-1.17 J/g°C
c)
0.857 J/g°C
d)
-0.857 J/g°C
87.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
88.

Where would you use the equation q = mcΔTq\ =\ mc\Delta T  ?

a)

Between C and D

b)

Between D and E

c)

At C, D, or E

d)

None of these

89.

Where would you use the equation q = ΔHfmq\ =\ \Delta H_fm  ?

a)

Between C and D

b)

Between D and E

c)

At C, D, or E

d)

None of these

90.

What phase change occurs when you start at C and end at D?

a)

Freezing

b)

Melting

c)

Condensing

d)

Vaporization

91.

Calculate the energy needed to completely boil away 30 g of water at 100 ⁰C .

a)

67,800 J

b)

2260 J

c)

226,000 J

d)

100 J

92.

How many joules are required to boil 75 grams of water?

a)

25050J

b)

169500J

c)

31350J

d)

10000J

93.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

94.

What phase of matter exists in part C of the graph?

a)

Gas

b)

Liquid

c)

Solid

d)

Plasma

95.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
96.

What is the Keq expression for this reaction?    2 NO(g)  +  O2(g) ⇌  2 NO2(g)

a)

Keq = [NO2]2 / [NO]2 [O2]

b)

Keq  =  [NO]2 [O2] / [NO2]2

c)

Keq  = [NO]2 [O2] [NO2]2

d)

Keq  = [NO2]2 / [NO]2 +  [O2]

97.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
98.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
a)
[Fe]3 [H2O]4  / [Fe3O4] [H2]4
b)
[Fe3O4] [H2]4 /  [Fe]3 [H2O]4
c)
[H2O]4 / [H2]4
d)
[Fe] [H2O] / [Fe3O4] [H2]
99.
If the equilibrium constant is much greater than one (K >> 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
100.
If the equilibrium constant is much less than one (K << 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
101.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)

Keq  = [NO2]2/[N2O4]

b)

Keq  = [N2O4]/[NO2]2

c)

Keq = [N2O4]2/[NO2]

d)

Keq = [NO2]/[N2O4]2

102.

What is the value of the Keq/Kc of the reaction "CO(g)+2H2(g)<---> CH3OH(g)" if the equilibrium concentrations of the reactants and product are: CO=0.17M, H2=0.34M, and CH3OH= 0.17M?

a)

0.085

b)

8.7

c)

0.12

d)

2.9

103.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
a)
increase
b)
decrease
c)
remain the same
104.
For the reaction...
energy +  N2(g)  +  O2(g)  <−>  2NO(g)
If  O2(g) is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
105.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased, the reaction will __________________.
a)
 shift to the left
b)
shift to the right
c)
not shift
106.

If the Keq = 2.3 which statement is true?

a)

The products are favored

b)

The reactants are favored

c)

Neither products or reactants are favored

107.

If the Keq = 5.46 x 10-4 which statement is true?

a)

The products are favored

b)

The reactants are favored

c)

Neither products or reactants are favored

108.
Which has a bitter taste?
a)
Base
b)
Acid
c)
flagella
d)
cila
109.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

110.

Which is the correct set of acid properties:

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

111.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

112.

Vinegar, fruit juice, and cola are examples of:

a)

salts

b)

neutral substances

c)

bases

d)

acids

113.

NaOH may be found in drain cleaners and as a component of soaps. Is NaOH an acid or a base?

a)

Acid

b)

Base

c)

Neither (Neutral)

114.

Is pure water acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

115.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

116.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

117.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

118.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

119.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

120.

What is the pOH of a solution with [H+] = 1.24 x 10 -2?

a)

1.91

b)

1.61

c)

12.09

d)

12.39

121.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

122.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

123.

What is the [OH-] if the pH is 4.9?

a)

4.9 x 10-10 M

b)

1.0 x 10-4 M

c)

1.25 x 10-5 M

d)

7.94 x 10-10 M

124.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

125.
The reaction of perchloric acid (HClO4) with lithium hydroxide (KOH) is described by the equation
HClO4 + KOH → KClO4 + H2O
Suppose 100 mL of perchloric acid is neutralized by exactly 50,0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?
a)
0.5M
b)
50M
c)
2.0M
d)
1.0M
126.
The reaction of hydrochloric acid (HCl) with ammonia (NH3) is described by the equation:
HCl + NH3 → NH4Cl
A student is titrating 100.0 mL of 0.10 M NH3 with 0.5 M HCl. How much hydrochloric acid must be added to react completely with the ammonia?
a)
20.0mL
b)
500.0mL
c)
100.0mL
d)
5.0mL
127.
How many milliliters of 0.360 M H2SO4 are required to neutralize 25 mL of 0.1 M Ba(OH)2?
a)
6.944 mL
b)
0.144 mL
c)
0.069 mL
128.

In the titration equation, M1V1 = M2V2, what is M?

a)

Molarity

b)

Concentration

c)

Amount of solution

d)

Mass of mixture

129.

What is the purpose of indicator solutions?

a)

To signal the end of a reaction

b)

To colour the solution

c)

To complete the reaction

d)

To equivalent the reaction

130.

In titration what is the long graduated piece of equipment called?

a)
Pipette
b)
Tube
c)
Burette
d)
Measuring Cylinder
131.
Acid + Base ₋--> 
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
132.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
133.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
134.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13

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