M6 - Topic Quiz - QC & QA

C) 31.61 g/Eq

The gram equivalent weight of potassium permanganate (KMnO₄, MW = 158.03 g/mol) in an acidic medium is:<br>A. 158.03 g/Eq<br>B. 79.02 g/Eq<br>C. 31.61 g/Eq<br>D. 52.68 g/Eq

A) 20.15 g/Eq

Compute for the gram equivalent weight of MgO (MW = 40.30 g/mol)<br>A. 20.15 g/Eq<br>B. 0.0403 g/Eq<br>C. 0.403 g/Eq<br>D. 0.2015 g/Eq

D) 0.049 g/Eq

The molecular weight of sulfuric acid is 98. Its milliequivalent weight is:<br>A. 98 g/Eq<br>B. 49 g/Eq<br>C. 0.098 g/Eq<br>D. 0.049 g/Eq

B) 5.0 mEq

How many mEq of Ca(OH)₂ are present in 25.0 mL of 0.10 M Ca(OH)₂?<br>A. 2.5 mEq<br>B. 5.0 mEq<br>C. 7.5 mEq<br>D. 10.0 mEq

B) 126.9 g/Eq

A sample contains I2 (MW: 253.81), which acts as an oxidizing agent according to the reaction: I2+2e- → 2I- What is the gram equivalent weight of iodine (I₂)?<br>A. 63.45 g/Eq<br>B. 126.9 g/Eq<br>C. 253.8 g/Eq<br>D. 507.6 g/Eq

A) 0.5N H2SO4

If the gram molecular weight of sulfuric acid is 98. Which of the following will be used to label the container of a solution containing 49 grams per liter of solution?<br>A. 0.5N H2SO4<br>B. 1N H2SO4<br>C. 1M H2SO4<br>D. 0.2M H2SO4

B) 1.24

A solution with a final volume of 500 mL was prepared by dissolving 25 mL of methanol (density= 0.7914 g/mL) in chloroform. Calculate the molarity of methanol in the solution. MW= 32.<br>A. 0.12<br>B. 1.24<br>C. 12.4<br>D. 124

A) 0.1034 N

Sulfamic acid (H3NSO3) is a primary standard that can be used to standardized sodium hydroxide. What is the normality if 33.26 mL reacts with 0.3337 g sulfamic acid. MW=97<br>A. 0.1034 N<br>B. 0.1004 N<br>C. 0.1005 N<br>D. 0.403 N

B) 0.150 mol

How many moles of HCl are contained in 75.0 mL of a 2.00 M HCl solution?<br>A. 0.0375 mol<br>B. 0.150 mol<br>C. 1.50 mol<br>D. 26.7 mol

C) 16.53

The molarity of concentrated HCl purchased in the laboratory is approximately 12.1 M. How many mL of this reagent should be diluted to 2 L to make 0.1 M?<br>A. 1.65<br>B. 6.53<br>C. 16.53<br>D. 165.3

D) 98.64%

A 0.8500 g sample of an impure pharmaceutical raw material containing potassium iodide (KI, MW = 166.00 g/mol) is dissolved in water. An excess of lead(II) nitrate is added to the solution, yielding a yellow precipitate of lead(II) iodide (PbI", MW=461.00 g/mol). After filtration, washing, and drying, the precipitate is found to have a mass of 0.5820 g. Calculate the percent purity of KI in the sample.<br>A. 24.66%<br>B. 49.32%<br>C. 68.45%<br>D. 98.64%

B) Proximate

Which of the following assays will involve total alkaloidal determination?<br>A. Specific<br>B. Proximate<br>C. Extraction<br>D. Ultimate

B) Gravimetric method

What assay method is illustrated in the assay of sodium chloride tablets wherein the salt precipitated is silver chloride, filtered, dried and residue is weighed?<br>A. Volumetric method<br>B. Gravimetric method<br>C. Complexation method<br>D. Gasometric method

C) Proximate assay

Assay of Atropine in Belladona is an example of which of the following?<br>A. Biological method<br>B. Ultimate assay<br>C. Proximate assay<br>D. Special method

A) Quantitative method

Which type of chemical analysis measures percentage content of the component present in a sample?<br>A. Quantitative method<br>B. Qualitative method<br>C. Proximate method<br>D. Gravimetric method

D) 113.7%

Calculate the percent purity of a potassium iodide sample (MW = 165.90) if a 0.47 g specimen yields 0.7564 g of silver iodide precipitate (MW = 234.76) upon gravimetric analysis.<br>A. 83.7%<br>B. 93.7%<br>C. 103.7%<br>D. 113.7%

C) Buret

A precisely manufactured glass tube with graduations enabling to measure the volume of liquid delivered through the stopcock at the bottom.<br>A. Separatory funnel<br>B. Graduated cylinder<br>C. Buret<br>D. Pipet

B) Wash bottle

What is the name of the apparatus used to wash down drops of standard solution clinging to the tip of the burette?<br>A. Cassia flask<br>B. Wash bottle<br>C. Babcock bottle<br>D. Acetylization flask

D) treatment with a solution of sodium chromate in sulfuric acid

What would be the most effective manner of cleaning glass apparatus?<br>A. rinsing with nitric acid<br>B. soaking in acetic<br>C. soaking in detergent<br>D. treatment with a solution of sodium chromate in sulfuric acid

A) Volumetric flask

What is used for quantitative preparation of a standard solution (aka volumetric solution)?<br>A. Volumetric flask<br>B. Pipet<br>C. Burette (or Buret)<br>D. Graduated Cylinder

A) It increases the solubility.

In the standardization of iodine solution, why is there a need to boil the solution of arsenic trioxide?<br>A. It increases the solubility.<br>B. It makes the solution stable.<br>C. It makes it acidic.<br>D. Boiling is not needed.

D) Sulfuric acid

The reaction between HCI and calcium carbonate can be seen in the standardization of:<br>A. Silver nitrate<br>B. Ammonium thiocyanate<br>C. Edetate disodium<br>D. Sulfuric acid

C) Arsenic trioxide

The 0.1 N iodine solution is standardized using<br>A. Potassium permanganate<br>B. Potassium hydrogen phthalate<br>C. Arsenic trioxide<br>D. Sodium carbonate

B) Sodium tartrate dihydrate

Primary standard used to standardized Karl Fischer reagent is:<br>A. Anhydrous sodium carbonate<br>B. Sodium tartrate dihydrate<br>C. Potassium hydrogen phthalate<br>D. Sodium oxalate

C) Potassium biphthalate

The primary standard used in the standardization of non-aqueous acidimetry is:<br>A. Sodium carbonate<br>B. Tromethamine<br>C. Potassium biphthalate<br>D. Benzoic acid

a) End point

The terms used when equivalent amounts of each reactant have reacted are the following, except:<br>a. End point<br>b. Equivalence point<br>c. Stoichiometric point<br>d. Theoretical point

D) I, II & III

Which of the following are components of a blank titration analysis?<br>I. Solvent<br>II. Reagent<br>III. Indicator<br>IV. Analyte<br>A. I, II, III, & IV<br>B. I, II & IV<br>C. II, III & IV<br>D. I, II & III

B) 7.15 mg

What is the titer value for 0.05M calcium chloride with 2 moles of water? MW= 142.9g/mol<br>A. 3.57 mg<br>B. 7.15 mg<br>C. 73.5 mg<br>D. 53.7 mg

B) Titer value

This is the weight of the substance chemically equivalent to 1 mL of the standard solution.<br>A. Equivalent weight<br>B. Titer value<br>C. Normality factor<br>D. Molarity

C) 92%

Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10 mL of 1.392 M HCl and heating to dissolve the solid and expel CO2. The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight % of the calcite in the limestone. MW=100<br>A. 29%<br>B. 39%<br>C. 92%<br>D. 96%

B) 99.5%

A pharmacist is verifying a raw batch of Sodium Carbonate (Na₂CO₃). The USP monograph states that: Each mL of 1 N Sulfuric Acid is equivalent to 53.00 mg of Na₂CO₃. A sample weighing 2.500 g requires 46.20 mL of sulfuric acid titrant that has been standardized to 1.015N. What is the percent purity of the Sodium Carbonate sample?<br>A. 95.4%<br>B. 99.5%<br>C. 100.4%<br>D. 102.0%

B) 20%

A 10 mL sample of sulfuric acid solution required 16.85 mL of NaOH solution in a titration. Each mL of the NaOH solution was equivalent to 0.2477 g of potassium hydrogen phthalate. Calculate the sulfuric acid content in %w/v. MW=98<br>A. 10%<br>B. 20%<br>C. 30%<br>D. 40%

C) Number of mEq

Two substances reacting upon reaching the end point must have the same<br>A. Normality<br>B. Volume<br>C. Number of mEq<br>D. Weight

B) 30 g

The molecular weight of NaOH is 40. How many grams of sodium hydroxide pellets are needed to make 500 mL of 1.5 N solution?<br>A. 20 g<br>B. 30 g<br>C. 40 g<br>D. 60 g

C) I, II, and III only

Standard solutions in nonaqueous alkalimetry.<br>I. Lithium methoxide<br>II. Perchloric acid<br>III. Hydrogen bromide<br>IV. Sodium hydroxide<br>A. I only<br>B. I and II only<br>C. I, II, and III only<br>D. I, II, III and IV

C) Non-aqueous acidimetry

Perchloric acid in glacial acetic acid and perchloric acid in dioxane are volumetric solution used in what type of analysis?<br>A. Direct acidimetry<br>B. Direct alkalimetry<br>C. Non-aqueous acidimetry<br>D. Non-aqueous alkalimetry

D) No indicator is suggested

When a weak base is to be titrated with weak acid, the indicator used is:<br>A. Phenolphthalein<br>B. Methyl orange<br>C. Methyl red<br>D. No indicator is suggested

A) Yellow

Methyl orange in base medium is colored:<br>A. Yellow<br>B. Pink<br>C. Colorless<br>D. Green

B) Pink

Phenolphthalein in alkali medium is colored:<br>A. Yellow<br>B. Pink<br>C. Colorless<br>D. Blue

D) I, II, and IV

Which of the following statement/s is/are correct?<br>I. Non-aqueous alkalimetry is used when the analyte is weakly acidic<br>II. Non-aqueous alkalimetry is used when analyte is acid halide.<br>III. Non-aqueous alkalimetry is used when the analyte contains heterocyclic nitrogen compound.<br>IV. Non-aqueous alkalimetry is used when analyte is barbiturate.<br>A. I only<br>B. I and II only<br>C. I, II, and III only<br>D. I, II, and IV

C) Methyl orange

When a strong acid is titrated against a weak base, the most suitable indicator is:<br>A. Phenolphthalein<br>B. Bromothymol blue<br>C. Methyl orange<br>D. Thymol blue

C) Phenolphthalein

Most suitable indicator to use in titration of organic acids<br>A. Methyl red<br>B. Methyl orange<br>C. Phenolphthalein<br>D. Eriochrome Black T

C) Phenolphthalein

The indicator commonly used in the assay of a weak acid reacting with a strong base is:<br>A. Methyl orange<br>B. Methyl red<br>C. Phenolphthalein<br>D. Crystal violet

A) Acidimetry

The measurement of a weak base in nonaqueous medium of a given sample by titration with standard perchloric acid:<br>A. Acidimetry<br>B. Alkalimetry<br>C. Complexometry<br>D. Redox titration

C) II, III, IV

The following is/are true about auxiliary complexing agent.<br>I. Eriochrome black is an example of an auxiliary complexing agent<br>II. Auxiliary complexing agents are also ligands.<br>III. Auxiliary complexing agents binds the metal strong enough to prevent the hydroxide from precipitating, but weakly enough to give up the metal ion when EDTA is added.<br>IV. It is used to permit many metals to be titrated in alkaline solution with EDTA.<br>A. I only<br>B. II, III<br>C. II, III, IV<br>D. III, IV

B) 92.4%

A 0.6500 g sample of impure calcium carbonate (MW: 100.09 g/mol) was dissolved and titrated with 0.0500 M EDTA. The titration required 120 mL of EDTA to reach the endpoint. What is the % purity?<br>A. 88.5%<br>B. 92.4%<br>C. 99.9%<br>D. 102.3%

B) 9.99 mg

A 50 mL aliquot of solution containing 0.450g of magnesium sulfate in 0.500 L required 37.6 mL of EDTA solution for titration. How many mg of calcium carbonate will react with 1 mL of this EDTA solution? MW MgSO4 = 120.37; MW CaCO3 = 100.09 g/mol<br>A. 0.995 mg<br>B. 9.99 mg<br>C. 99.94 mg<br>D. 9943 mg

A) Ligand

A molecule which provides groups of attachment to metal ions.<br>A. Ligand<br>B. Chelate<br>C. Metal<br>D. Complex

b) Decreases

NaCl ______ the stability of Metal-EDTA complex.<br>a. Increases<br>b. Decreases<br>c. No effect<br>d. None of the choices

B) I and II

The following is/are true about EDTA:<br>I. EDTA forms strong 1:1 complexes with most metal ions.<br>II. It is a chelating agent that prevents metal-catalyzed oxidation of food and pharmaceuticals.<br>III. It is a pentadentate molecule<br>IV. It contains 3 oxygen and 2 hydrogen atoms that can enter complexation reaction with metal ion.<br>A. I only<br>B. I and II<br>C. II and III<br>D. III and IV

B) Masking agent

In complexometric titration, what is used to prevent one metal ion from interfering in the analysis of another metal ion?<br>A. Buffering agent<br>B. Masking agent<br>C. Auxiliary complexing agent<br>D. Metallochromic indicator

B) Hydroxynaphthol blue

The indicator for EDTA titration against CaCO3 is:<br>A. Thymol blue<br>B. Hydroxynaphthol blue<br>C. Methyl red<br>D. Methylene blue

D) 6.24%

A 0.2185 g sample containing sodium chloride (NaCl) was analyzed using the Volhard titration method. An excess of 50.0 mL of 0.0998 N silver nitrate (AgNO₃) was added to precipitate the chloride ions. The excess silver ions were then back-titrated with 11.9 mL of 0.1350 N ammonium thiocyanate (NH₄SCN). Calculate the percent purity of NaCl in the sample<br>A. 42.6%<br>B. 62.4%<br>C. 90.5%<br>D. 6.24%

C) Fajans

Who introduced the use of adsorption dyes as indicators in precipitation titrations?<br>A. Volhard<br>B. Mohr<br>C. Fajans<br>D. Gay-Lussac

B) Mohr

Who introduced the use of 0.1 N silver nitrate as the titrant and potassium chromate TS as the indicator in the volumetric precipitation of chlorides?<br>A. Liebig<br>B. Mohr<br>C. Volhard<br>D. Fajans

C) Silver nitrate, with ammonium thiocyanate as back titrant

Ferric alum is used as the indicator in a volumetric precipitation method when the titrant is:<br>A. Potassium permanganate<br>B. EDTA<br>C. Silver nitrate, with ammonium thiocyanate as back titrant<br>D. Sodium hydroxide

A) Arrhenius

The assay procedures in volumetric precipitation were introduced by the following scientists, except:<br>A. Arrhenius<br>B. Mohr<br>C. Fajans<br>D. Volhard

C) H2SO4

What is the acid needed in Permanganometry?<br>A. HCl<br>B. HNO3<br>C. H2SO4<br>D. CH3COOH

C) II, III, and IV

Which of the following statement/ is/are correct?<br>I. KMnO4 can be standardized using arsenic trioxide<br>II. KMnO4 serves as indicator in acidic solution.<br>III. Hydrogen peroxide can be analyzed using KMnO4.<br>IV. KMnO4 in acidic solution is reduced to colorless Mn+2<br>A. I and II<br>B. I, II, and III<br>C. II, III, and IV<br>D. II and IV

A) Oxalic acid

To remove stain of KMnO4, the most effective chemical substance is :<br>A. Oxalic acid<br>B. Sodium thiosulfate<br>C. Vinegar<br>D. Bromine solution

D) Permanganate solution

Which of the following is the indicator used in permanganate titration?<br>A. Methyl orange<br>B. Phenolphthalein<br>C. Methyl red<br>D. Permanganate solution

D) I, II, and II

Which of the following statements is/are correct?<br>I. Potassium dichromate is an oxidizing agent<br>II. Potassium dichromate is used chiefly for the determination Fe+2<br>III. Potassium dichromate to chromous ion, gains 6 electrons<br>A. I only<br>B. II only<br>C. III only<br>D. I, II, and II

C) I, II, and III

Which of the following conditions decrease the effectiveness of starch as an indicator?<br>I. Presence of organic solvents<br>II. Presence of electrolytes<br>III. Temperature above 25 °C<br>IV. Temperature at 25 °C<br>A. I only<br>B. I and II<br>C. I, II, and III<br>D. I, II, III and IV

C) To prevent bacterial growth

The use of chloroform in sodium thiosulfate solution.<br>A. To stabilize the solution<br>B. To increase its solubility<br>C. To prevent bacterial growth<br>D. To maintain pH of the solution

A) Sodium bicarbonate

Which of the following is added to maintain the pH of sodium thiosulfate in optimum range for the stability of the solution?<br>A. Sodium bicarbonate<br>B. Chloroform<br>C. Thymol<br>D. Sodium carbonate

C) As a preservative

What is the use of HgI2 in the preparation of starch TS?<br>A. To increase the solubility of starch<br>B. To impart color<br>C. As a preservative<br>D. To stabilize the pH

C) III only

Which of the statement/s is/are correct?<br>I. Direct titration of a reducing agent with iodine is called iodometry.<br>II. In iodimetry, an oxidizing agent is added to excess I- to produce iodine which us then titrated with sodium thiosulfate.<br>III. In iodimetry, starch TS can be added at the beginning of the titration.<br>IV. In iodometry, starch TS can be added at the beginning of the titration.<br>A. I only<br>B. II only<br>C. III only<br>D. IV only

B) Amylose

The active fraction of starch which reacts with iodine to form an intense blue color<br>A. Amylopectin<br>B. Amylose<br>C. Glucose<br>D. Sucrose

C) Residual iodometry using excess bromine

Phenol is assayed using this method of analysis.<br>A. Residual alkalimetry<br>B. Volumetric precipitation<br>C. Residual iodometry using excess bromine<br>D. Iodimetry

A) 90.44

A sample of 0.1350 g of As2O3 (MW: 197.84 g/mol) was assayed iodimetrically using 23.4 mL of 0.1055 N iodine solution. The percentage purity of the sample is:<br>A. 90.44<br>B. 90.23<br>C. 89.0<br>D. 90.54

B) 15.1%

The Kjeldahl procedure was used to analyzed 256µL of a solution containing 37.9 mg protein/mL. The liberated ammonia was collected in 5 mL of 0.0336 M HCl, and the remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the weight % of nitrogen in the protein? MW= 14g/mol<br>A. 3.86%<br>B. 15.1%<br>C. 51.5%<br>D. 5.65%

B) Silver nitrate

Standard solution in precipitation method of analysis<br>A. Disodium edetate<br>B. Silver nitrate<br>C. Sodium Methoxide<br>D. Perchloric acid

A) Reduction-Oxidation

What chemical reaction is involved during an analysis wherein there occur a change of valence of reacting substances?<br>A. Reduction-Oxidation<br>B. Precipitation<br>C. Neutralization<br>D. Complexation

B) Volumetric precipitation

In qualitative analysis where would adsorption indicators be used?<br>A. Complexation reaction<br>B. Volumetric precipitation<br>C. Acidimetry<br>D. Alkalimetry

C) Back and blank titration

When an alkaloid is subjected to titration analysis using ultimate assay method, what are possible types of titrations based on the number of volumetric solutions?<br>A. Direct titration and blank titration<br>B. Direct and residual titration<br>C. Back and blank titration<br>D. Residual and back titration

C) Ferric alum

Which among the following list of indicators is not used in acid-base titrations?<br>A. Methyl red<br>B. Phenolphthalein<br>C. Ferric alum<br>D. Methyl orange

B) Disappearance of blue color

The end point of iodometry using starch TS as indicator is:<br>A. Appearance of blue color<br>B. Disappearance of blue color<br>C. Appearance of second precipitate<br>D. Disappearance of green-blue color

B) Phenolphthalein TS

What is the indicator used in the assay of a weak acid reacting with a strong base?<br>A. Methyl red TS<br>B. Phenolphthalein TS<br>C. Thymol blue<br>D. Methyl orange TS

B) Cerimetry

Orthophenanthroline TS is used as indicator in<br>A. Permanganometry<br>B. Cerimetry<br>C. Iodometry<br>D. Iodimetry

B) Complexometry

Most of the official drugs containing Calcium and Magnesium are determine by:<br>A. Iodometry<br>B. Complexometry<br>C. Permanganometry<br>D. Dichromatometry

D) Residual titration

This analysis is done by dissolving the substance under examination in an accurately measured quantity of standard solution known to be in excess and back titrating the excess solution with another standard solution.<br>A. Gravimetric analysis<br>B. Acidimetric analysis<br>C. Direct alkalimetric analysis<br>D. Residual titration

B) Iodimetry

When a reducing analyte is titrated directly with iodine, the method used is called<br>A. Iodometry<br>B. Iodimetry<br>C. Cerimetry<br>D. Permanganometry

B) Reducing agent

Iodimetry is an indirect analysis of:<br>A. Oxidizing agent<br>B. Reducing agent<br>C. Acid<br>D. Base

D) Gravimetry

Which of the following is NOT a type of chemical reaction used in volumetric analysis?<br>A. Redox titration<br>B. Neutralization<br>C. Diazotization<br>D. Gravimetry

D) Sodium hydroxide solution

Which of the following standard solutions is not used in redox titration?<br>A. Sodium thiosulfate solution<br>B. Iodine solution<br>C. Bromine solution<br>D. Sodium hydroxide solution

D) Diazotization

Assay of sulfa drugs can be determined by this reaction with 0.1 M sodium nitrite.<br>A. Neutralization<br>B. Complexation<br>C. Precipitation<br>D. Diazotization

D) Diazotization titration

Which of the following is used in the analysis of aromatic compounds containing an amino group in the molecule?<br>A. Acid-base titration<br>B. Proximate assay<br>C. Acetylation process<br>D. Diazotization titration

d. 3 – 15 μm

The medium infrared region of the spectrometer used to identify a substance has a wavelength range of:<br>a. 200 – 380 nm<br>b. 380 – 780 nm<br>c. 780 – 3000 nm<br>d. 3 – 15 μm

d. All of the above

Region in an electromagnetic spectrum:<br>a. Visible<br>b. Infrared<br>c. Ultraviolet<br>d. All of the above

D) Concentration of the sample

Beer's plot in spectrometry is prepared to determine:<br>A. Absorbance of the sample<br>B. Absorbance of the blank<br>C. Wavelength to be used<br>D. Concentration of the sample

A) 16.15mcg

In using spectrophotometer to measure the concentration of a sample, the following data were obtained:<br>o absorbance of the standard solution = 0.39<br>o absorbance of the sample solution = 0.42<br>o concentration of the standard = 15mcg<br>The concentration of the sample is:<br>A. 16.15mcg<br>B. 17.5mcg<br>C. 15.75mcg<br>D. 16.0mcg

Beer-Lambert Law

The concentration of an unknown sample in spectrophotometric procedures can be calculated by<br>o Use of _________________<br>o Calculations using _______________

Lambert or Bouger's Law

The law related to spectrometry wherein the power of transmitted light decreases exponentially as the thickness of the solution increases arithmetically is ___________

b. 0.50

A solution has a concentration of 2.0 × 10+* M. The molar absorptivity is 2500 M+, cm+, and the path length is 1 cm. What is the absorbance?<br>a. 0.25<br>b. 0.50<br>c. 0.75<br>d. 1.00

D) Concentration of the sample

In spectrophotometry, Beer's plot is prepared in order to determine which of the following aspects?<br>A. Blank<br>B. Absorbance of the sample<br>C. Wavelength<br>D. Concentration of the sample

A) Prism

A spectrophotometer differs from a colorimeter because it consists of:<br>A. Prism<br>B. Lamp house<br>C. Cell compartment<br>D. Optical scale

C) Chromophore

Which of the following terms refer to the functional group of an organic molecule that absorbs maximum radiation in ultraviolet or visible regions?<br>A. Nitrile (C≡N)<br>B. Hydroxyl group (–OH)<br>C. Chromophore<br>D. Carbonyl (C=O)

D) Atomic Absorption Spectroscopy ® Absorption by free atoms

Which of the following analytical techniques is correctly matched with the principle that serves as the basis for its measurement?<br>A. UV-Vis Spectroscopy ® Vibrational transitions<br>B. IR Spectroscopy ® Nuclear spin transitions<br>C. NMR Spectroscopy ® Electronic transitions<br>D. Atomic Absorption Spectroscopy ® Absorption by free atoms

C) Beer's law

Which among the following laws is a fundamental law of fluorometry in the analysis of drugs?<br>A. Law of mass action<br>B. Boyle's law<br>C. Beer's law<br>D. Newton's law

A) Milliliter

The following are units of measurement generally used in spectrometry, EXCEPT___.<br>A. Milliliter<br>B. Angstrom<br>C. Micrometer<br>D. Nanometer