Download Practice Test 4 Ch 12,13,14

Chem 10Practice , Test 4 (Ch 12, 13, 14)
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MULTIPLE CHOICE. Mark the correct answer for Qs1-30 on a Scantron only.
Each Q is worth 2 points. If you have any erase marks on the scantron right them
below with the correct answer. (60 points)
1) Evaporation is:
A) a cooling process for humans when they sweat.
B) the opposite process as condensation.
C) an endothermic process.
D) increased by increasing temperature.
E) all of the above
2) Which intermolecular force is present in all molecules and atoms?
A) dipole-dipole forces
B) X-forces
C) hydrogen bonding
D) dispersion forces
E) none of the above
3) Which state of matter has a high density and a definite volume?
A) solids
B) gases
C) liquids
D) both solids and liquids
E) none of the above
4) Which noble gas has the highest boiling point?
A) Xe
B) He
C) Ne
D) Kr
5) Which intermolecular forces are found in CCl4?
A) dipole-dipole forces
B) hydrogen bonding
C) dispersion forces
D) X-forces
E) none of the above
6) Which intermolecular force found in
A) dipole-dipole forces
B) hydrogen bonding
C) dispersion forces
D) X-forces
E) none of the above
is the strongest?
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E) Ar
7) Which molecule below has hydrogen bonding?
A) CH 3 OH
B) H 2O
C) HF
D) NH 3
E) all of the above
8) Substance A is a molecular compound that dissolves in gasoline but not in water. The
molecules of A are very likely
A) nonpolar
B) nonmetallic
C) metallic
D) polar
E) none of the above
9) The oxygen in the air we breath is classified as:
A) the solute in a heterogeneous gas-liquid mixture.
B) the solvent in a simple mixture.
C) the solvent in a homogeneous gas mixture.
D) the solute in a homogeneous gas mixture.
E) none of the above
10) Which of the following compounds is a strong electrolyte?
A) NaCl
B) HCl
C) NH 4 Cl
D) NaC 2 H3 O2
E) all of the above
11) Solubility of solids in water:
A) increases with increasing temperature.
B) is independent of the temperature.
C) decreases with increasing temperature.
D) Solids are not soluble in water.
E) none of the above
12) We dissolve 2.45 g of sugar in 200.0 g water. What is the mass percent of sugar in the
solution?
A) none of the above
B) 123%
C) 2.42%
D) 1.21%
E) 1.23%
13) Which of the following substances is not a solution?
A) homogenized milk
B) bronze
C) soda
D) sea water
E) All of the above are solutions.
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14) If you prepare a solution by adding sufficient amount of solute so that after heating and
cooling the solution there is a visible amount of solid solute left in the bottom of the
beaker, the solution would be considered:
A) saturated.
B) unsaturated.
C) supersaturated.
D) thermally saturated.
E) none of the above
15) What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
A) 257 mL
B) none of the above
C) 560. mL
D) 0.560 mL
E) 21.9 mL
16) A 0.15 M solution of BaCl2 contains
A) 0.15 M Ba2+ ions and 0.15 M Cl- ions
B) 0.30 M Ba2+ ions and 0.30 M Cl- ions
C) 0.15 M Ba2+ ions and 0.30 M Cl- ions
D) 0.30 M Ba2+ ions and 0.15 M Cl- ions
E) none of the above
17) How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33
moles of NaF?
A) 13.1
B) 239
C) 31.1
D) 55.9
E) none of the above
18) Which of the following is NOT a property of acids?
A) Acids have a slippery feel.
B) Acids turn litmus paper red.
C) Acids dissolve many metals.
D) Acids have a sour taste.
E) All of the above are properties of acids.
19) Which of the following is not an acid-base conjugate pair?
A) none of the above
B) H2CO3 and HCO3C) H2O and OHD) H2S and OHE) NH4+ and NH3
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20) Solubility of gases in water
A) increases with increasing temperature.
B) decreases with increasing temperature.
C) is independent of temperature.
D) gases are not soluble in water.
E) none of the above
21) The Arrhenius definition of an acid is:
A) produces H⁺ in solution.
B) produces OH⁻ in solution.
C) a proton acceptor.
D) a proton donor.
E) none of the above
22) What are the products of a neutralization reaction?
A) water and salt
B) carbon dioxide and water
C) oil and water
D) salt and carbon dioxide
E) none of the above
23) Which of the following acids is a monoprotic, strong acid?
A) hydrobromic acid
B) carbonic acid
C) sulfuric acid
D) phosphoric acid
E) none of the above
24) What is the pH of a solution that has a H⁺ concentration equal to
A) 10.20
B) 5.20
C) 0.22
D) 4.77
E) none of the above
?
25) The pH of a solution is 5.00. Which of the following is TRUE about the solution?
A) Its [H3O+] is 1.0 x 105 M
B) Its [H3O+] is 1.0 x 10-5 M
C) Its [H3O+] is 1.0 x 10-9 M
D) It is more acidic than a solution whose pH is 4.00.
E) none of the above
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26) What is the concentration of the hydronium ions in a neutral solution
A) 0.0 M
B) < 1.0
M
C) 1.0
D) > 1.0
E) 1.0
M
M
M
27) Which of the following is a weak base?
A) potassium hydroxide
B) sodium fluoride
C) ammonia
D) calcium hydroxide
E) none of the above
28) What is the conjugate acid of OH⁻?
A) OH⁻
B) NaOH
C) H 2 O
D)
E) none of the above
29) Which of the following acids is diprotic?
A) HNO3
B) HI
C)
D) HClO4
E) none of the above
30) When an acid reacts with a metal, what is one of the usual products?
A) salt
B) hydrogen gas
C) water
D) carbon dioxide
E) none of the above
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1. What is the pH, pOH , [OH-] and nature (acidic/basic/neutral) of a solution that has a [H+ ] = 0.0039 M?
Formulas: pH + pOH =14.00, pH = - log [H+ ], pOH =-log [OH- ]
(7 pts)
PH= - log [H+] = 2.41-acididc
pOH=14-pH=11.54
[OH-]= 2.6 x 10 -12 M
2. Complete and balance the following equation:- (5 pts)
phosphoric acid (aq) + magnesium carbonate (s) → ? + ? + ?
2H3PO4 (aq)+ 3 MgCO3(s) →Mg3(PO4)2 (aq) + 3 H2O (l) + 3CO2(g)
3. Classify the following as acids ( strong/weak), bases(strong/weak) or salts: ( 5 pts)
1) HClO2 weak acid
2) KNO3 salt
3) CH3 NH2 weak base
4) HF weak acid
5) MgO strong base
4. Write the balanced total ionic and net ionic equation for the following reaction:
Remember to cancel the spectator ions.
MgCl2(aq) + 2AgNO3(aq) → Mg(NO3)2 (aq)+ AgCl(s) ( 6 points)
NOT ON THIS TEST.
Ag+ + Cl- → AgCl (s)
5. How many grams of BaCrO4 can be produced from the reaction of 1.05 L of 0.470 M BaCl2 solution with
K2CrO4 solution according to the following equation : Show all formulas and work to get full credit.(6 points)
BaCl2 (aq) + K2CrO4 (aq) → Ba CrO4 (s) + 2 KCl(aq)
0.470 moles BaCl2 x 1.05 L BacL2= 0.494 moles baCl2
0.494 moles BaCl2 x 1mol BaCrO4/1 mol BaCL2= 0.494 mol BaCrO4 x 253.33 g= 125 g BaCrO4
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6. How will you make 500.0 mL of 0.200 M KOH solution using dry chemical? Show all formulas and work to
get full credit ( 5 pts)
M=g/MM x L.
G= M x MM x L=5.61 g
Weigh 5.61 g KOH and H2Oin volumetric flask and dilute to mark with DI water.
7. Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would
be associated with each of the following compounds. ( 6 points)
A) BeF2
____London_______________________
B) OF2
____London______________________
C) HCl
____Dipole-Dipole______________________
D) HF
______H bonding
_______________________
E) IBr
______Dipole-Dipole_____________________
F) Br2
______London_____________________
Answers to multiple choices:
1) E
2) D
3) D
4) A
5) C
6) A
7) E
8) A
9) D
10) E
11) A
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12) D
13) E
14) A
15) E
16) C
17) B
18) A
19) D
20) B
21) A
22) A
23) A
24) D
25) B
26) E
27) C
28) C
29) C
30) B
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