Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEMICAL TECHNICIAN > SQUAREDEL REVIEWER 2019 ANALCHEM > Flashcards

SQUAREDEL REVIEWER 2019 ANALCHEM Flashcards

1
Q
  1. What do you call a combination of two or more materials which retain their individual properties and can be separated by physical means.

A. solvents
B. reactions
C. mixtures
D. solutions

A

C. mixtures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q
  1. A polar solute usually dissolves In a polar solvent and a nonpolar solute usually dissolves in a nonpolar solvent. This is

A. Hund’s rule
B. Henry’s law
C. the solubility rule
D. the like dissolves like rule

A

D. the like dissolves like rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q
  1. What is the molarity of a solution containing 72.9 grams of HCI in enough water to make 500 mL of solution?

A. 2.0 m/L
B. 4.05 g/L
C. 5.0 m/L
D. 4.05 m/L

A

D. 4.05 m/L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q
  1. A solution has 3x10^(-4) copper 2+ content. How much is the copper 2+ content in ppm?

A. 3 ppm
B. 38 ppm
C. 9 ppm
D. 19 ppm

A

D. 19 ppm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q
  1. Solutions of electrolytes and metals are

A. Insulators
B. Polar
C. Negative
D. Conductors

A

D. Conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q
  1. The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measuring a very small volume of a stock solution. Instead it Is done by a series of dilutions. A sample of 0.8214 g of KMn04 (158.04) was dissolved in water and made up to the volume in a 500 ml volumetric flask. A 2.000-ml sample of this solution was transferred to a 1000-ml volumetric flask and diluted to the mark with water. Next, 10.00 ml of the diluted solution were transferred to a 250 ml flask diluted to the mark with water. What is the concentration (in molarity) of the final solution?

A. 0.1039 M
B. 2.079 × 10^(-5) M
C. 8.316 × 10^(-7) M
d. none of the choices

A

C. 8.316 × 10^(-7) M

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q
  1. How much of a 2.0M stock solution do you need to prepare 50 ml of a 1.0 M solution?

A. 75 ml
B. 30 ml
C. 25 ml
D. 50 ml

A

C. 25 ml

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q
  1. A statement that sums up what you learned from an experiment and states if the hypothesis is proven or disproven is called?

A. procedure
B. control group
C. hypothesis
D. conclusion

A

D. conclusion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q
  1. A prediction or a possible explanation to the question or problem which can be tested in an experiment is called?

A. hypothesis
B. procedure
C. graph
D. data

A

A. hypothesis

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q
  1. The number 2.34 x 10^(-7) is the scientific notation for

A. 234000
B. 23400
C. 23400000
D. 2340000

A

C. 23400000 (typo given should be raise to 7)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q
  1. Express the number 0.051065 to four significant figures

A. 0.051
B. 0.051
C. 0.05106
D. 0.0511

A

C. 0.05106

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q
  1. The volume of a liquid is 20.5 mL. Which of the following sets of measurement represents the value with good accuracy?

A. 19.2 mL, 19.3 mL, 18.8 mL, 18.6 mL
B. 18.9 mL, 19.0 mL, 19.2 mL, 18.8 mL
C. 18.6 mL, 17.8 mL, 19.6 mL, 17.2 mL
D. 20.2 mL, 20.5 mL, 20.3 mL, 20.1 mL

A

D. 20.2 mL, 20.5 mL, 20.3 mL, 20.1 mL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q
  1. What is the chemical formula of diphosphorus monobromide?

A. PBr2
B. PBr
C. P2Br2
D. P2Br

A

D. P2Br

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q
  1. Which of the following is a chemical reaction?

A. an air conditioner cooling the air
B. none of these choices
C. bleaching your clothes
D. melting of ice

A

C. bleaching your clothes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q
  1. Noble gases are inert because they have completed outer electron shells. Which of these elements isn’t a noble gas?

A. Chlorine
B. Krypton
C. Helium
D. Argon

A

A. Chlorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q
  1. What is the most common isotope of hydrogen?

A. Hydrogen only has one isotope
B. Deuterium
C. Tritum
D. Protium

A

D. Protium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q
  1. As you move from top to bottom down the periodic table

A. change in atomic radius cannot be predicted
B. ionization energy Increases
C. electronegativity decreases
D. atomic radius decreases

A

C. electronegativity decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q
  1. What do you call an atom that has more protons than electrons?

A. an anion
B. none of the choices
C. a molecule
D. an isotope

A

B. none of the choices (cation)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q
  1. Which one of the following is a chemical equation?

A. CO2
B. C + O2 -> CO2
C. Ice + heat -> water
D. iron + oxygen -> rust

A

B. C + O2 -> CO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q
  1. As you move from left to right across the periodic table

A. atomic radius increases
B. ionization energy decreases
C. electronegativity decreases
d. atomic radius decreases

A

d. atomic radius decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q
  1. Balance the following equation: Ag + O2 → Ag2O

A. Put a 2 in front of Ag
B. Add a 4 in front of Ag and a 2 in front of Ag2O
C. Add a subscript 2 to the end of Ag2O
D. Add a 2 in front of Ag and a 1 in front of Ag2O

A

B. Add a 4 in front of Ag and a 2 in front of Ag2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q
  1. Which is NOT an acceptable name for Hg2Cl2?

A. mercury (II) chloride
B. mercury (1) chloride
C. mercurous chloride
D. dimercury dichloride

A

A. mercury (II) chloride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q
  1. Under the Lewis concept of acids and bases, an acid is

A. An electron pair donor
B. a proton acceptor
C. a proton donor
D. an electron pair acceptor

A

D. an electron pair acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q
  1. Which of the following is NOT an acid?

A. milk of magnesia
B. apple juice
C. milk
D. gastric juice

A

A. milk of magnesia

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q
  1. Which of the following is NOT an acid-base conjugate pair?

A. NH, and NH^+
B. H2S and OH^-
C. H2O and OH^-
D. HCN and CN^-

A

B. H2S and OH^-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q
  1. When NH4CI hydrolyzes, the resulting solution is

A. acidic
B. basic
C. neutral
D. none of the choices

A

A. acidic (Cl will become HCl strong acid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q
  1. Aqua regia, the reagent that can be used to dissolve gold, is a 3:1 mixture of which acids?

A. hydrochloric and nitric acids
B. hydrofluoric and nitric acids
C. hydrochloric and sulfuric acids
D. perchloric and sulfuric acids

A

A. hydrochloric and nitric acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q
  1. Which of the following conjugate acid/base pairs should be used to prepare a buffer with pH near
    7.15?

A. Formic acid / sodium formate (pKa - 3.74)
B. Sodium dihydrogen phosphate/ sodium hydrogen phosphate (pKa2 = 7.20)
C. Succinic acid/sodium succinate (pKa = 5.64)
D. Glycylglycine / sodium glycylglycate (pKa = 8.35)

A

B. Sodium dihydrogen phosphate/ sodium hydrogen phosphate (pKa2 = 7.20)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q
  1. Predict the products of the following acid-base reaction: NHs(aq) + HNO3(aq)

A. no reaction takes place
B. NH4OH(aq)
C. NH2OH(aq) + HNO2(aq)
D. NH4NO3(aq)

A

D. NH4NO3(aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q
  1. What is the gas which behaves the most like an ideal gas?

A. oxygen
B. nitrogen
C. helium
D. hydrogen

A

C. helium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q
  1. What happens to the volume of a fully inflated balloon when it is taken outside on a cold day?

A. its volume decreases
B. its volume increases
C. it remains the same
D. its volume becomes equal to zero

A

A. its volume decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q
  1. The standard pressure of the atmosphere at sea level is?

A. 760 mm Hg
B. all of the choices
C. 760 torr
D. 1 atm

A

B. all of the choices

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q
  1. Each of these flasks contains the same number of molecules. In which container is the pressure highest?
    (images show flasks in increasing size from Flask 1 - 4)

A. Flask 2
B. Flask 1
C. Flask 3
D. Flask 4

A

B. Flask 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q
  1. What is the molar mass of an unknown gas if 1.60 grams of that gas occupies a volume of 2.24 L
    at STP?

A. 35.8 g/mol
B. 160 g/mol
C. 16.0 g/mol
D. 81.0 g/mol

A

C. 16.0 g/mol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q
  1. When chromium changes from an oxidation state of +3 to that of +6, the Cr^3+ must:

A. gain 6 electrons
B. lose 6 electrons
C. lose 3 electrons
D. gain 3 electrons

A

C. lose 3 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q
  1. During the electroplating of silver, silver ions in solution.

A. are oxidized at the anode
B. are oxidized at the cathode
C. are reduced at the cathode
D. remain in solution unchanged

A

C. are reduced at the cathode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q
  1. The equation that represents a reaction that is NOT a redox reaction is:
    Reaction 1: 2H2 + O2 -> 2H2O
    Reaction 2: Zn + CuSO4 -> ZnSO4 + Cu
    Reaction 3: 2H2O2 -> 2H2O + O2
    Reaction 4: H2O + CO2 -> H2CO3

A. Reaction 3
B. Reaction 1
C. Reaction 4
D. Reaction 2

A

C. Reaction 4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q
  1. In an electrolytic cell oxidation occurs

A. at the anode
B. between the cathode and the anode
C. at either the cathode or the anode
D. at the cathode

A

A. at the anode ( RED CAT AN OX) PANIC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q
  1. For this reaction Mg+ H2O -> MgO + H2 which is FALSE?

A. H is the oxidizing agent
B. Mg lost electrons
C.Mg is the oxidizing agent
D. H gained electrons

A

C. Mg is the oxidizing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q
  1. Which procedure is recommended for reading the level of an aqueous solution in a buret or graduated cylinder?

A. Keep the eye level with the top of the meniscus and record that reading
B. Read both the bottom and top of the meniscus and average those readings
C. Keep the eye level with the bottom of the meniscus and record that reading
D. Look down at the meniscus at an angle to obtain the average reading directly

A

C. Keep the eye level with the bottom of the meniscus and record that reading

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q
  1. What is the main ISO standard used by testing and calibration laboratories to gain accreditation and formal recognition of their competence to carry out tests and/or calibrations, including sampling?

A. ISO/IEC 17025
B. EURACHEM
C. AOAC
D. ISO 9000:2000

A

A. ISO/IEC 17025

42
Q
  1. This detects contamination from reagents, sample handling, and the entire measurement process.

A. matched-matrix blank
B. method blank
C. solvent blank
D. calibration blank

A

B. method blank

43
Q
  1. There is a definite correlation between orderliness and level of safety in the laboratory. In addition, a disorderly laboratory can hinder or endanger emergency response personnel. Which of the following housekeeping rules should NOT be adhered to?

A. never obstruct access to exits and emergency equipment
B. properly label and store all chemicals
C. store chemical containers on the floor
D. clean work areas, including floors, regularly

A

C. store chemical containers on the floor

44
Q
  1. In order to ensure an accurate weighing when using the balances, one should _____________

A. leave the object on the balance for several minutes to ensure a stable reading
B. not lean on the balance bench, close the draft doors on the balance and zero the balance prior to weighing
C. turn the balance off to clear any previous weighings from its memory
D. weigh the object several times on different balances and take the average of these weighings

A

B. not lean on the balance bench, close the draft doors on the balance and zero the balance prior to weighing

45
Q
  1. Which of the following is NOT part of the technique for pouring in a laboratory?

A. Connect the pouring spout and receiving container using a stirring rod
B. Pour fast enough to avoid spills
C. Pour and allow the liquid to run along the stirring rod
D. Hold containers at arms length, with elbows slightly bent

A

B. Pour fast enough to avoid spills

46
Q
  1. The method that is widely used for the determination of the protein content of meat and animal food is the?

A. Kjeldahl method
B. Mohr method
C. McBride method
D. Liebig method

A

A. Kjeldahl method

47
Q
  1. The water content of an 875.4-mg sample of cheese was determined with a moisture analyzer. What is the %w/w H2O in the cheese if the final mass was found to be 545.8 mg?

A. 35.23%
B. 30.6%
C. 31.45%
D. 37.66%

A

D. 37.66%

48
Q
  1. An analytical chemist needs to transfer his/her precipitants from the beaker to the filter paper. Which of the following would be the best procedure to adopt in order to ensure a quantitative transfer of the precipitate?

A. none of the choices.
B. Most of the liquid above the ppt is decanted first, then bulk of ppt is transferred to filter paper through a stirring rod, the beaker is washed with big volumes of wash solution.
C. Most of the liquid above the ppt is decanted first, bulk of the ppt is transferred through a stirring rod, wash the beaker several times with small volumes of wash solution.
D. Solution is shaken, then immediately filtered; beaker is washed with relatively big volumes of ash solution.

A

C. Most of the liquid above the ppt is decanted first, bulk of the ppt is transferred through a stirring rod, wash the beaker several times with small volumes of wash solution.

49
Q
  1. A water sample is collected for analysis of oil and grease. The analysis will not be done immediately. The sample should NOT be

A. collected in plastic bottle
B. preserved with sulfuric acid
C. refrigerated til analyzed
D. collected in all glass bottle

A

D. collected in all glass bottle

50
Q
  1. When two materials that have different densities, like oil and water, encounter one another, they will

A. separate according to their densities
B. exchange densities
C. mix uniformly
D. repel one another

A

A. separate according to their densities

51
Q
  1. Conductivity is defined as

A. The ability of a substance to conduct electric current, which is the same as resistivity
B. The ability of a substance to repel electric current
C. The ability of a substance to conduct variable resistance
D. The ability of a substance to conduct electric current, which is the reciprocal of resistivity

A

D. The ability of a substance to conduct electric current, which is the reciprocal of resistivity

52
Q
  1. Even though all solid states of other materials are denser than the liquid states of materials, what unique property of water?

A. It is clear
B. It is tasteless
C. Solid water (ice) is less dense than liquid water (ice floats in water)
D. It can freeze

A

C. Solid water (ice) is less dense than liquid water (ice floats in water)

53
Q
  1. The following statements are true about electrical conductivity EXCEPT ______________

A. a measure of a solution’s capacity to conduct electricity
B. a measure of the total dissolved solids in a solution
C. increasing temperature has no effect on its value
D. is directly affected by temperature

A

C. increasing temperature has no effect on its value

54
Q
  1. The following statements are true about pH EXCEPT
    _____________

A. the negative logarithm of hydrogen ions content in a solution
B. a measure of the acidity or alkalinity of a solution
C. a measure of the amount of hydrogen ions in solution
D. does not change when there are changes in temperature

A

D. does not change when there are changes in temperature

55
Q
  1. In maintenance and storage of pH meters, which of the following procedure shall NOT be done?

A. Mild soap solution may be used in general cleaning of the electrodes
B. To keep the electrode bulb moist during storage, store the electrode in distilled water.
C. Blot the electrode dry after rinsing the pH electrodes.
D. Rinse pH electrodes in between measurements.

A

B. To keep the electrode bulb moist during storage, store the electrode in distilled water.

56
Q
  1. The apparatus shown below would be used to
    (image shows circular bottom)

A. distill a liquid.
B. chromatograph a mixture.
C. filter a precipitate.
D. reflux a solution.

A

D. reflux a solution.

57
Q
  1. In operating a UV-Vis spectrophotometer, the following shall be done, EXCEPT for

A. Before turning on the power, check if the sample holder does not contain anything.
B. After turning on, allow the spectrophotometer to Initialize and stabilize according to its user
manual.
C. If there are any spillage that gets onto the instrument, immediately wipe it away.
D. Keep the sample compartment open during measurement.

A

D. Keep the sample compartment open during measurement.

58
Q
  1. In using fume hoods, the following shall be done, EXCEPT for

A. Items contaminated with odorous or hazardous materials should be removed from the hood only after decontamination or if placed in a closed outer container to avoid releasing contaminants into
the laboratory air.
B. The hood shall be kept closed, except during apparatus set-up or when working within the hood.
C. The hood may be used as a permanent storage area for volatile chemicals when an
appropriate storage cabinet is not available.
D. Ensure the exhaust is operating before using the hood.

A

C. The hood may be used as a permanent storage area for volatile chemicals when an
appropriate storage cabinet is not available

59
Q
  1. In purifying a material by crystallization choose the solvent according to the following EXCEPT ____________

A. solubility
B. vapor pressure
C. reactivity
D. polarity

A

B. vapor pressure

60
Q
  1. The dynamic range in analytical measurement refers to the range where ___________

A. the instrument reading is constant
B. the detection limit lies
C. the sensitivity of the instrument is highest
D. the instrument reading is linearly related to the input value

A

B. the detection limit lies

61
Q
  1. What is the law that states the linear relationship between absorbance and concentration of an absorbing species?

A. Boyles Law
B. Beer-Lambert’s Law
C. Charles Law
D. Avogadro’s Law

A

B. Beer-Lambert’s Law

62
Q
  1. Determine the actual volume contained in a 50.0 mL volumetric flask given the following data:
    Mass of water: 50.1227 g, Density of water at 25°C: 0.99707 g/mL

A. 50.27 mL
B. 50.37 mL
C. 50.17 mL
D. 50.45 mL

A

A. 50.27 mL

63
Q
  1. A lab analyst dissolved 4.021 g of NaOH in water and made up the solution to 1 litre with water. He then pipetted 10.00 mL of this solution into a flask and titrated it with 0.050 M HCl solution from a burette. A volume of 20.32 mL of acid had been used at the endpoint. Examining this result, the lab supervisor could deduce that _____________

A. the NaOH absorbed H2O from the air after its mass was measured
B. the burette was rinsed with water instead of HCI
C. the analysis is as accurate as can be expected using this apparatus
D. the pipette was rinsed with water instead of NaOH

A

C. the analysis is as accurate as can be expected using this apparatus

64
Q
  1. In which of the following titrations does pH = 7.0 occur at the equivalence point?

I. Strong acid/strong base
II. Weak acid/strong base
Ill. Strong acid/Weak base

A. II and III only
B. Ill only
C. I only
D. II only

A

C. I only

65
Q
  1. The following are good sampling practices EXCEPT

A. Collect the sample in a container made of material that will chemically react with the sample.
B. Sample frequently enough to allow for the identification or process cycles.
C. Take several Increments and composite them to form the sample.
D. if possible, mix the material before getting the sample.

A

A. Collect the sample in a container made of material that will chemically react with the sample.

66
Q
  1. In liquid-liquid extraction, it is often necessary to determine which liquid is aqueous and which liquid is nonaqueous. To test the liquids, add a drop of water to the top layer. If the drop dissolves in the top layer, the top layer is __________

A. aqueous
B. denser
C. miscible
D. nonaqueous

A

A. aqueous

67
Q
  1. The process in which the sample is heated to the boiling point of the solvent and volatile analytes are concentrated in the vapour phase, condensed and collected.

A. distillation
B. liquid-liquid extraction
C. evaporation
D. oven drying

A

A. distillation

68
Q
  1. Glass container is NOT suitable for __________

A. oil and grease determination
B. microbiological analyses
C. all of the choices
D. inorganic trace analyses

A

D. inorganic trace analyses

69
Q
  1. The maximum holding time for acid preserved samples that will be subjected to determination of
    metals is

A. 48 hours
B. 3 months
C. 6 months
D. 1 week

A

C. 6 months

70
Q
  1. The substance which does the dissolving and must be greater than 50% of the solution is called ___________.

A. solute
B. solvent
C. mixture
D. solution

A

B. solvent

71
Q
  1. Quantitative chemical analysis of weighing a sample, usually of a separated and dried precipitate is called __________.

A. Gravimetric analysis
B. Elemental analysis
C. Volumetric analysis
D. Titrimetric analysis

A

A. Gravimetric analysis

72
Q
  1. Which of the following is a primary standard for use in standardizing bases?

A. Acetic acid
B. Sulfuric acid
C. Potassium hydrogen phthalate
D. Ammonium hydroxide

A

C. Potassium hydrogen phthalate

73
Q
  1. How many grams of Sodium Persulfate (Na2S2O) are required to prepare a 1 L solution of Sodium Persulfate with concentration of 10% (w/v). This solution is widely used as oxidizing reagent for Total Organic Carbon analyzer (TOC).

A. 100 g of Sodium Persulfate
B. 101 g of Sodium Persulfate
C. 102 g of Sodium Persulfate
D. 99 g of Sodium Persulfate

A

A. 100 g of Sodium Persulfate

74
Q
  1. How many grams of sodium hydroxide is needed to prepare 500 mL of 0.5 N sodium hydroxide? (Sodium 22.99 g/mole, Oxygen 16.00 g/mole, Hydrogen= 1.008 g/mole)

A. 13.8115
B. 15.7470 g
C. 9.9995 g
D. 10.2515 g

A

C. 9.9995 g

75
Q
  1. What is the light source used in the visible range to 340-1000 nm ?

A. nerst blower (400-20,000)
B. tungsten
C. deuterium (190-370nm)
D. Incandescent

A

B. tungsten

76
Q
  1. Minimum concentration of a substance that can be measured and reported with 99% confidence that the analyte concentration is greater than zero refers to

A. Lower Warning Limit
B. Method Detection Limit
C. Lower Control Limit
D. Limit of Quantitation

A

B. Method Detection Limit

77
Q
  1. Which of the following instruments uses a cuvette?

A. Gas Chromolograph
B. UV-Vis Spectrophotometer
C. pH Meter
D. Flame-AAS

A

B. UV-Vis Spectrophotometer

78
Q
  1. The most appropriate technique to determine levels of the Pb^2+ ion in blood is _____________

A. atomic absorption spectroscopy
B. mass spectrometry
C. infrared spectroscopy
D. high-performance liquid chromatography

A

A. atomic absorption spectroscopy

79
Q
  1. Analytical methods or instruments’ performance aim for ___________

A. Low signal-to-noise ratio
B. High variability
C. Low dynamic range
D. High signal-to-noise ratio

A

D. High signal-to-noise ratio

80
Q
  1. A graphical representation of measuring signal as a function of quantity of analyte is called __________
    A. Absorbance Chart
    B. Calibration curve
    C. Quality Control Chart
    D. none of the choices
A

B. Calibration curve

81
Q
  1. For the reaction, Fe^3+ (aq) + SCN^- (aq) <=> FeSCN^2+(aq). The equilibrium constant for this week’s reaction can best be determined by means of

A. lon-exchange
B. Conductance
C. Spectrophotometry
D. Chromatography

A

C. Spectrophotometry

82
Q
  1. A food scientist has a sample of a plantoil and wants to determine if the oil contains saturated or unsaturated fatty acids. Which of the following spectroscopic techniques would be most useful for this purpose?

A. mass spectroscopy/Gas Chromatography
B. ultraviolet spectroscopy
C. infrared spectroscopy
D. visible spectroscopy

A

C. infrared spectroscopy

83
Q
  1. What is a graph showing the detectors response as a function of elution time: band’s shapes, position, resolution?

A. monitor display
B. chromatogram
C. quality control chart
D. calibration curve

A

B. chromatogram

84
Q
  1. A stable light source in AAS analysis, which is necessary to emit the sharp characteristic spectrum of the element to be determined is called

A. Tungsten lamp
B. hollow cathode lamp
C. deuterium lamp
D. Nerst blower

A

B. hollow cathode lamp

85
Q
  1. It is a hazardous waste characteristic which applies to wastes that have the potential to contaminate groundwater if improperly disposed of. These materials are regulated as hazardous waste due to their potential to leach out specific toxic substances in a landfill.

A. Reactivity
B. Corrosivity
C. Toxicity
D. Ignitability

A

C. Toxicity

86
Q
  1. In handling acid wastes, what type of protective gloves should be used?

A. Rubber gloves
B. Cloth gloves
C. Disposal plastic gloves
D. Surgical gloves

A

A. Rubber gloves

87
Q
  1. According to Revised DAO 04-36, the appropriate waste labels shall include __________

A. all of the choices
B. Generator ID Number
C. Volume of Waste
D. Container Material

A

A. all of the choices

88
Q
  1. The following acids and acid mixtures can be collected and placed in glass containers EXCEPT for __________

A. Sulfuric acid
B. Hydrofluoric acid
C. Aqua regia
D. Hydrochloric acid

A

B. Hydrofluoric acid

89
Q
  1. When working with concentrated acids except hydrofluoric acid, which of the following statements are TRUE?

I. Acid-resistant gloves covering the whole arm or Nitrile gloves should be worn.
II. Half- or full-faced masks with gas- and/or vapor removing respirators should be worn.
III. Wearing safety boots or foot covering is optional as long as the person is working under the hood.
IV. Wearing of apron is optional as long as laboratory gown is worn.

A. I & II
B. II & III
C. all of the choices
D. I & IV

A

A. I & II

90
Q
  1. The fire triangle consists of which of the following?

A. Oxygen, Heat, Material
C. Air, Fuel, Spark
B. Air, Heat, Fire
D. Oxygen, Heat, Fuel

A

D. Oxygen, Heat, Fuel

91
Q
  1. In order to properly maintain chemical laboratory equipment one should perform the following EXCEPT _________

A. place the equipment in hot humid location
B. regular calibration of equipment
C. regular inspection of operational components
D. thorough cleaning with the proper materials

A

A. place the equipment in hot humid location

92
Q
  1. Which is TRUE about laboratory fume hoods?

A. all of the choices
B. Provides further protection by diluting low concentration of flammable gases below explosion
limits.
C. It protect you from being exposed in chemical fume.
D. Must always be on.

A

A. all of the choices

93
Q
  1. What is the type of chemical that can cause an allergic reaction in the airways following inhalation
    of the chemical?

A. Corrosive
B. Respiratory Sensitizer
C. Oxidizer
D. Carcinogen

A

B. Respiratory Sensitizer

94
Q
  1. Which of the following may be disposed in the sink?

A. 0.1M H2SO4
B. 1 g/ml PC14
C. none of the choices
D. 200g/ml PC14

A

C. none of the choices

95
Q
  1. Ammonia solution can be stored with following chemicals EXCEPT for _________

A. cyclohexane solution
B. acetic acid solution
C. 2-propanol solution
D. sodium hydroxide solution

A

B. acetic acid solution

96
Q
  1. Which of the following can cause ERRORS during the sample preparation stage?

I. Loss of sample during weighing or dissolution
II. Contamination by impurities in reagents and in the environment
III. Changes in mass due to varying humidity and temperature
IV. Obtaining inhomogeneous sample from the bulk

A. I and II only
B. I, III, and IV
C. I, II, and III
D. I, II, III, and IV

A

D. I, II, III, and IV

97
Q
  1. What will you perform to know that the Atomic absorption spectrometer continues to work
    properly?

A. Calibration check
B. Blank
C. QC sample recoveries
D. Standard addition

A

A. Calibration check

98
Q
  1. Consider that you are working with Vitamin C tablet production, to which standard/s should your quality management should subscribe?

A. GMP
B. HACCP
C. ISO 9001:2008
D. All of the choices

A

D. All of the choices

99
Q
  1. The test that decides whether a datum from a given set could be rejected or NOT is

A. T-test
B. Z-test
C. Q-test
D. F-test

A

C. Q-test

100
Q

Saying that the concentration of Total cyanide (CN) In drinking water is 0.05 mg/L, which is below the maximum allowable level of 0.07 mg/L as per DOH DAO No. 20070012 when it is actually above that limit is

A. accurate
B. false negative
C. precise
D. false positive

A

B. false negative

CHEMICAL TECHNICIAN (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions