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BATTERY REVIEWER - ANACHEM > ANACHEM - MIDTERM > Flashcards

ANACHEM - MIDTERM Flashcards

1
Q

Which of the following is the confirmatory
test for the presence copper ions?

A

Which of the following is the confirmatory
test for the presence copper ions?

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2
Q

In titration, the solution of known
concentration is the

A

-standard solution or
-titrant

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3
Q

The phosphorus in a sample of phosphorus
rock weighing 0.5428g is precipitated as
MgNH4PO4.6H2O and ignited to Mg2P2O7
If the ignited precipitate weighs 0.2234g.

A

Calculate the % of P2O5 in the sample
-26.25
The weight of MgNH4PO4.6H2O
-0.4927

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4
Q

A substance that dissolves in water and
conducts electricity when present in an
aqueous solution is

A

Ionic

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5
Q

Process that allows coagulated particles to
revert to disperse state is known as

A

Peptization

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6
Q

Which of the following cations is considered
most toxic heavy metal that could affect the
nervous system?

A

Mercury ion

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7
Q

A weak acid, HF, is in solution with
dissolved sodium fluoride, NaF to make
buffer solution. If HCl is added, which ion
will react with the extra hydrogen ions from
the HCl to keep the pH from changing?

A

OH-

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8
Q

A solution was known to contain both Ag+
ions and Bi3+ ions. Which of the following
could be added to separate them in such a
way that one ion would end up in a
precipitate, while the other remained in
solution?

A

HNO3

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9
Q

If 8.19g KIO3 is dissolved in enough water
to make 500.0mL of solution, what is the
molarity of the potassium iodate solution?
The molar mass of KIO3 is 214g/mol.

A

7.65 x 10^-2 M

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10
Q

A process in which equations are arranged
so that unwanted units cancel and only the
desired units will remain.

A

Dimensional analysis

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11
Q

The equation below shows the
decomposition of lead nitrate. How many
grams of oxygen gas are produced when
11.5 g NO is formed? (N -14 g/mol; O-16
g/mol)
2Pb(NO3)2(s) –> 2PbO(s) + 4NO2(g)+
O2(g

A

1.00g

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12
Q

Dispersed particles in liquid phase, that settles spontaneously.

A

Colloidal suspension

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13
Q

The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below.
P4S3(s) + O2(g) → P4O10(s) + SO2(g)
What mass of SO2 is produced from the combustion of 0.331 g P4S3?

A

0.289 g

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14
Q

An electrolyte that partially dissociates in water

A

Weak Electrolyte

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15
Q

In titrimetric analyses, secondary standards are usually standardized against a primary standard.

A

False

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16
Q

All of the following are colligative properties EXCEPT

A

gas solubility as a function of partial pressure above a solution (Henry’s law).

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17
Q

Which of the following compounds is the deep blue color complex of copper ion?

A

Cu(NH3)(^2+)4

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18
Q

Le Châtelier’s Principle states that if a chemical system at equilibrium is stressed,

A

the system will adjust to reduce the stress.

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19
Q

Sodium Hydroxide a common titrant in titration of bases is also considered as a primary standard.

A

False

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20
Q

A solution is prepared by dissolving 4.40g of KSCN in enough water to make 340mL of solution. What is the concentration of the solution?

A

0.133 M

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21
Q

A Bronsted-Lowry base is defined as:

A

a proton acceptor

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22
Q

Which of these compounds is most likely to be covalent?

A

CS2

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23
Q

A 1.45 g sample of chromium contains () atoms.

A

1.68 x 10^22

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24
Q

If 16.4 g of oxygen gas react with excess hydrogen, what mass of water is produced? 2H2(g) + O2(g) →2H2O(g)

A

18.5 g

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25
Q

Which of these compounds is most likely to be ionic?

A

ICl

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26
Q

Which of the following is the correct Kb expression for HPO4(^2-) if added to water?

A

Kb = [H2PO4-][OH-]/[HPO4(^2-)]

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27
Q

What is the mass percent of each element in sulfuric acid, H2SO4?

A

2.055% H, 32.69% S, 65.25% O

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28
Q

Which of the following statements concerning osmosis is/are CORRECT?

A

-Osmosis involves the movement of a solvent through a semipermeable membrane. OR
-Osmotic pressure is a colligative property.

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29
Q

The molar mass of boron is 10.81 g/mole. What is the mass of a single boron atom?

A

6.510 x 10^24g

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30
Q

What concentration unit is necessary for the calculation of vapor pressure lowering?

A

mole fraction

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31
Q

Which of the following is the strongest acid?

A

Oxalic Acid Ka = 5.9 × 10^-2

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32
Q

If a solution is prepared by dissolving 7.7g of lithium iodide, LiI, in enough water to make 400mL of solution, what is the %(w/v) of LiI?

A

1.9%

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33
Q

What volume of 6.0M HNO3 is required to prepare 250mL of 0.40M HNO3?

A

17ml

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34
Q

A 0.6025g sample of a chloride salt was dissolved in H2O and the chloride precipitated by adding excess silver nitrate. The precipitate of silver chloride was filtered, washed, dried and found to weigh 0.7134g. Calculate the % Cl in the sample.

A

29.29%

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35
Q

How many liters of 0.2805 M C4H12O6(aq) contain 1.000g of C6H12O6 ?

A

0.01979 L

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36
Q

Name the basic parts of a titration set-up

Name of basic part 1 -
Name of basic part 2 -
Name of basic part 3 -
Name of basic part 4 -
Name of basic part 5 -

A

Name of basic part 1- Burette clamp
Name of basic part 2- Burette
Name of basic part 3- Iron ring
Name of basic part 4- Erlenmeyer flask
Name of basic part 5- Analyte

37
Q

The curve upper surface of liquid in a burette or graduated cylinder is the

A

meniscus

38
Q

Given the following equilibrium, which of the following statements is TRUE if additional F is added to the solution? HF(aq)+ H2O (l) –> H3O+(aq) + F-(aq)

A

[H3O+] will decrease and the pH value will increase

39
Q

A temperature dependent concentration that is often used to measure the colligative properties of substances

A

m

40
Q

Which of the following is FALSE about a system at equilibrium?

A

It’s a “dynamic equilibrium”: reactants and products are constantly changing

41
Q

What is the mass percent of each element in sulfuric acid, H2SO4?

A

2.055% H, 32.69% S, 65.25% O

42
Q

A 0.1298g sample of pure acid was titrated with 42.11ml of 0.1234 N NaOH. What is the equivalent weight of the acid?

A

24.98

43
Q

Given the reaction at equilibrium: N2(g)+ 3H2(g) <–> 2NH3(g) . If the pressure is increased at constant temperature, there will be an increase in the number of moles of

A

NH3 only

44
Q

Which of the following liquids will be miscible with water in any proportions: ethanol (CH3CH2OH), carbon tetrachloride (CCl4), hexane (C6H14), and/or formic acid (HCO2H)?

A

ethanol and formic acid

45
Q

Which of the following is a substance that ionizes completely in a solution?

A

a strong electrolyte

46
Q

Which of the following is NOT part of Group II cations?

A

Cobalt

47
Q

When computing for the equivalent weight, what are the values that you will consider?

A
  • the weight in grams, OR
  • molar mass
48
Q

How many hydrogen atoms are present in 1.0g of NH3?

A

3.5 x 10^22 atoms

49
Q

Which of the following is the confirmatory reagent for bismuth ion?

A

Na2SnO2

50
Q

Crystalline NaF is added to a dilute solution of hydrofluoric acid (HF). What happens to the hydrogen ion concentration as a result of this addition?

A

unchanged

51
Q

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:
4NH3 + 5O2 → 4NO + 6H2O
When 20.0g NH and 50.0g O are allowed to react, which is the limiting reagent?

A

NH3

52
Q

What is the [H+] concentration of a solution with pH = 3.48?

A

3.31 x 10^-4M

53
Q

What is the weight of NaCl in a 0.500L bottle of 2.00M NaCl?

A

58.4g

54
Q

Which of the following is used to increase the rate of sedimentation for cation analysis?

A

Centrifuge

55
Q

What concentration unit is necessary for the calculation of boiling point elevation?

A

molality

56
Q

The moles of solute per liter of solution is expressed by

A

M

57
Q

Unknown X was treated with six drops of HCl. A precipitate was observed. Which of the following ions could be present?

A

Tin ion

58
Q

How many moles of HCl are present in
0.098 grams of HCl?

A

0.0027 mol

59
Q

A pipette that can measure and transfer various amounts of liquid is

A

serological

60
Q

A molecule is found to contain 47.35% by mass C, 10.60% by mass H, and 42.05% by mass O. What is the empirical formula for this molecule?

A

C3H8O2

61
Q

A solution is prepared by 100mL of 10M HCl to 1L volumetric flask and filling it to the mark with water. What is the pH of the solution?

A

1

62
Q

Which of the following is the product of the reaction between a solution containing soluble ion of silver and nitric acid?

A

[Ag(NH3)2]Cl

63
Q

Which is a correct method for calculating the moles of calcium carbonate present in 132 grams of calcium carbonate?

A

132gCaCO3 (1mol/100.1g)

64
Q

An aqueous solution containing a concentration of 2.5 X 10 OH ions will have a pH of which of the following?

A

6.40

65
Q

A solution of anything in water is known as

A

aqueous

66
Q

Which laboratory equipment is needed to prepare solutions of known %(w/w)?

A

a volumetric flask

67
Q

In a solution of a solid in a liquid, the solid is called which of the following?

A

Dissolve

68
Q

Given the Ka values shown, which one of the anions shown is the weakest base?
CH COOH (Ka = 1.8 x 10^-5) HCOOH (Ka = 1.0 x 10^-4) HClO (Ka = 3.0 x 10^-8)
HF (Ka = 6.8 x 10^-4)

A

F-

69
Q

When alcohol is dissolved in water which would normally be the solute?

A

the compound present in smaller amount

70
Q

The pH of a 1.25 x 10-3 M NaOH solution is:

A

3.10

71
Q

What is the mass of 0.71 mol Na?

A

16 g

72
Q

In a solution of a solid in a liquid, the liquid is called which of the following?

A

dissolver

73
Q

A 0.001 M aqueous solution of HCl has a pH of

A

3.0

74
Q

A substance that changes in color at equivalence point.

A

indicator

75
Q

An iron ore was analyzed by dissolving a 1.1324g sample in concentrated HCl. The resulting solution was diluted with water and the iron (III) was precipitated as hydrous oxide Fe2O3.xH2O by the addition of NH3 After filtration and washing, the residue was ignited at a high temperature to give 0.5394g of pure Fe2O3 (FW= 159.69).

A

Calculate the % Fe O (FW= 231.54) in the sample?
-46.04
Calculate the % Fe (55.847)
-33.32

76
Q

How many grams are in 1.946 moles of NaCl? (Na - 23 g/mol; Cl - 35 g/mol)

A

112.9g

77
Q

The TARE button in the analytical balance cancels the weight of the container

A

True

78
Q

Method of analysis that involves measurement of the mass of the product to calculate the quantity of the original analyte.

A

Gravimetric Analysis

79
Q

A 0.45 M solution of a newly discovered weak acid HZ has a pH of 2.60. What is the value of Ka for HZ?
HZ + H2O <—> H3O+ + Z-

A

1.4 x 10-5 M

80
Q

Which of the following is the supernatant liquid from precipitating insoluble chlorides?

A

HCl

81
Q

For the following system at equilibrium, what will cause the shift toward left side of the reaction?
UO2(s) + 4 HF(g) <-> UF4(g) + 2 H2O(g)

A

adding UF4(g)

82
Q

If 25.00mL of 2.00M NaCl is transferred by pipet into a volumetric flask and diluted to 5.00L, what is the molarity of the diluted NaCl?

A

0.190mol Ag(107.9g/mol)

83
Q

What is the solubility product expression for Fe2(CO3)3?

A

Ksp = [Fe2+]^2[CO3^2-]^3

84
Q

A 0.25 M solution of carbonic acid has a pH of 3.48. What is the Ka of the solution?
H2CO3 + H2O <-> HCO3- + H3O+

A

4.4 x 10^-7

85
Q

In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased?

A

CaCO3(s) <-> CaO(s) + CO2(g)

86
Q

Which of the following compounds shows an orange precipitate for a confirmatory test?

A

Sb2S3

87
Q

To prepare 0.250L of 0.100M aqueous NaCl (58.4 g/mol), one may

A

dissolve 1.46g of NaCl in enough water to make 0.250L of solution

88
Q

Particles that are invisible to the naked eye.

A

colloidal suspension

BATTERY REVIEWER - ANACHEM (3 decks)

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