The following is/are example/s of metal-ion indicators. I. Murexide II. Calmagite III. Pyrocatechol violet IV. Ferric alum

Assay of diluted HCl is expressed in:

Standard solution in precipitation method of analysis

Use to prevent one element from interfering in the analysis of another element

Argentometric titration is titration with ______ ion.

Fajans titration uses ____ indicator.

Reasons why residual titration are performed.

Solutions containing all the reagents and solvents used in the analysis, but no deliberately added analyte.

Describes how close a measured value is to the true value.

Primary standard in the standardization of perchloric acid

Primary standard in the standardization of sodium methoxide.

The term dried to constant weight means that two consecutive weighing do not differ by more than:

Other name of systematic error

Ferric ammonium sulfate is used as indicator in the standardization of:

The end point of using number ferric ammonium sulfate is:

Limit moisture in nonaqueous titrimetric analysis is less than:

Complete reaction: H2C6H4O6 + NaOH - □

A ligand that binds to a metal ion through only one atom.

Which of the following is added to maintain the pH of sodium thiosulfate in optimum range for the stability of the solution?

Standard solution in non-aqueous titrimetric analysis-acidimetry

Standards solutions are also known as:

If starch is used as an indicator, the end point is/are:

Types of chemical reaction used in the volumetric analysis

Use of KI in the preparation of iodine solution.

Other name of ferrous phenanthroline.

Color of the complex resulting from reaction with ferrous phenanthroline:

Primary standard in the standardization of ceric sulfate solution

In the standardization of iodine solution, why is there a need to boil the solution of arsenic trioxide?

Indicator in iodometric method of analysis.

A molecule which provides groups of attachment to metal ions.

HCl + Calcium carbonate will react to form a primary product known as:

The reaction between HCl and calcium carbonate can be seen in the standardization of:

A substance which gains electrons in a redox reaction.

The equilibrium constant for the reaction of the metal ion with a ligand is called ____.

NaCl ____ the stability of EDTA complex.

Organic solvents _______ the stability of EDTA complex.

Indicator in Redox Titration using KMnO4

Developed in 1883, this method of analysis remains as one of the accurate and widely used method for determining nitrogen in substance.

Most suitable indicator to use in titration of organic acids

Which of the following statement/s is/are correct? I. Non-aqueous alkalimetry is used when the analyte is weakly acidic II. Non-aqueous alkalimetry is used when analyte is acid halide. III. Non-aqueous alkalimetry is used when the analyte contains heterocyclic nitrogen compound. IV. Non-aqueous alkalimetry is used when analyte is barbiturate.

Indicator/s used in nonaqueous titrimetry I. Nile blue II. Crystal violet III. Malachite green IV. Phenolphthalein

Standard solutions in nonaqueous alkalimetry. I. Lithium methoxide II. Perchloric acid III. Hydrogen bromide IV. Sodium hydroxide

The use of chloroform in sodium thiosulfate solution.

Which of the following statement/s is/are correct? I. The utility of starch as indicator is reduced in the presence of organic solvent. II. The utility of starch as indicator is reduced in the presence of electrolytes. III. The utility of starch as indicator is reduced at temperature above 25 °C. IV. The utility of starch as indicator is reduced at temperature of 25°C.

When a weak base is to be titrated with weak acid, the indicator used is:

The formula to compute the equivalent weight of a reducing agent.

The use of sodium bicarbonate in the standardization of iodine solution ______.

Method/s determining the total nitrogen in a sample

To keep samples moisture free, the appropriate apparatus to use is:

The following is/are true about EDTA: I. EDTA forms strong 1:1 complexes with most metal ions. II. It prevents metal-catalyzed oxidation of food. III. It is a pentadentate molecule IV. It contains 3 oxygen and 2 hydrogen atoms that are capable of entering complexation reaction with metal ion.

Sulfamic acid (H3NSO3) is a primary standard that can be used to standardized sodium hydroxide. What is the molarity if 33.26 mL reacts with 0.3337 g sulfamic acid. MW=97

A 0.2185 g sample of NaCl was assayed using Volhard method using 50 mL of 0.998N silver nitrate and 11.9 mL of 0.1350N ammonium thiocyanate. Calculate the NaCl in the sample. MW NaCl = 58.45

A 4.59 mL sample of HCl, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a titration. Calculate the % w/w HCl.

What is the titer value for 0.05 M calcium chloride with 2 moles of water? MW= 142.9

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/w. MW=98

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

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= 14

How many grams of Cupric (II) Sulfate pentahydrate should be dissolves in a volume of 500 ml to make $$8 \times 10^{-3} M$$ solution? MW= 249.54

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?

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.

The above solution (question no.61) has a density of 1.454 g/mL. Find the molality of methanol.

What is the use of HgI2 in the preparation of starch TS?

Process of measuring the actual quantity mass, volume, force, etc. that correspond to an indicated quantity on the scale of an instrument.

Also known as Eosin Y.

The active fraction of starch which reacts with iodine to form an intense blue color

When a reducing analyte is titrated directly with iodine, the method used is called

The 0.1 N iodine solution is standardized using

Iodimetry is an indirect analysis of:

Which of the following statement/s is/are correct according to USP 27? I. In azeotropic method of water of analysis toluene is used as solvent. II. In azeotropic method of analysis toluene and xylene are used as solvents. III. In azeotropic method of analysis toluene, xylene, and water are used as solvents.

What weight of arsenic trioxide (93.73%) would be used as a sample so that 26.6 mL of 0.1120 N iodine would be needed to titrate it? MW = 197.46

The type of alkaloidal assay where the total alkaloid is determined.

Which of the following statement/s is/are correct? I. Method I of water content determination in USP 27 is the azeotropic toluene distillation method. II. Method II of water content determination in USP 27 is the titrimetric method. III. Method III of water content determination in USP 27 is the gravimetric method. IV. Method I of water content determination in USP 27 is the Karl Fischer method.

Residue on ignition is also called:

Primary standard used to standardized Karl Fischer reagent is:

Method 1 for determining alcohol-soluble extractives is also known as:

Which of the following statement/s is/are correct I. Iodine value is a quantitative measure of the amount of unsaturated fatty acid in fats. II. Method I of determining iodine value is also known as Hanus method. III. Wij's method is also a method of determining iodine value. IV. Hubl's method is official method of determining iodine value.

Koettsdorfer number is also known as:

The gram-equivalent weight of sodium oxalate (MW = 134 g/mole) is:

Orthophenanthroline TS is used as indicator in

A sample of Chlorpheniramine maleate weighing 0.502 g was assayed by nonaqueous titrimetry using 22.2 mL of perchloric acid with normality of 0.1125. Calculate the % purity of the sample. Each mL of 0.1 N perchloric acid is equivalent to 19.54 mg of C16H19CLN2·C4H4O4.

Calculate the weight of oxalic acid required to prepare 1000 mL of 0.5 N of the solution. MW = 126

If 10 g of olive oil required 20 mL of 0.0211 N NaOH in the titration of the free fatty acids. What is the acid number of the oil?

Does the acid value of the above conform with the official requirement? (In 10 g of olive oil, the specification is <5 mL of 0.1 N NaOH.)

In phenol contain determination of a volatile oil, the layer in the graduated neck of the cassia flask read 2.3 mL obtained from a sample of 10 mL of the oil after treatment with KOH solution. The % phenol is:

A 4.0570 g sample of chlorinated lime was mixed with enough water to make 1000 mL. A 100 mL of the mixture was treated with potassium iodide and acetic acid, then titrated with 22.4 mL of sodium thiosulfate solution. A 20 mL sample of sodium thiosulfate was found to be equivalent to 0.2996 g of pure iodine. Calculate the available chlorine in the sample. MW Iodine = 126.9 ; MW Cl = 35.45

Military standard table is also known as:

The % hexane extractive obtained from 27.5820 g of crude drug yielding a residue of 0.9155 g of extractive is:

Calculate the menthyl acetate content in % if 9.5 g sample of peppermint oil was refluxed with 25 mL of 0.5 N alcoholic KOH and required 22.5 mL of 0.4900 N HCl for the residual titration. The blank was run using the same volume of 0.5 N alcoholic KOH and required 26.0 mL of 0.4900 N HCl to bring about the end point. Each mL of 0.5 N alcoholic KOH consumed in the saponification is equivalent to 99.15 mg menthyl acetate.

Calculate the % alkaloid extracted from a bark of plant using 1.0215 g of the crude drug; the volume of 0.0245 N sulfuric acid added to the extract was 25.7 mL, the excess was back titrated by 21.75 mL of 0.0225 N sodium hydroxide solution. Each mL of 0.02 N sulfuric acid is equivalent to 3.8858 mg of the alkaloid.

Determine the iodine value of an unknown sample of oil weighing 0.21 g if 26 mL and 12 mL of 0.1100 N of sodium thiosulfate are required for the blank and residual titration respectively.

Identify the sample of the above question with USP requirement of:

Find the acid value of oleic acid sample weighing 2 g which require 45 mL of 0.1102 N NaOH to bring about the end point.

If a sample of white wax is found to have an ester value of 65.7 and a saponification value of 74.2, what is the acid value of the sample?

A 50 mL aliquot of solution containing .450 g of magnesium sulfate in 0.5 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 magnesium sulfate = 120.37; MW CaCO3 = 100

The following is/are true about auxillary complexing agent. I. Eriochrome black is an example of an auxillary complexing agent II. Auxillary complexing agents are also ligands III. Auxillary 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. IV. It is used to permit many metals to be titrated in alkaline solution with EDTA.

The following is/ are true about EDTA titration. I. EDTA titration is also known as complexometric titration. II. The equilibrium constant in EDTA titration is called EDTA indicator. III. For end-point detection, commonly used indicator is called EDTA indicator IV. EDTA titration technique includes displacement titration

Which of the following statement/s is/are true? I. A redox indicator is a compound that changes color when it goes from oxidized to reduced state II. Starch is a redox indicator III. Ferroin is a redox indicator IV. The hydrolysis is product of starch is glucose which is a reducing agent

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

Which of the following statements is/are correct? I. Potassium dichromate is an oxidizing agent II. Potassium dichromate is used chiefly for the determination Fe+2 and indirectly sample that will oxidized Fe+2 to Fe+3. III. Potassium dichromate to chronous ion, gains 6 electrons

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

Koppeschar's solution is also known as:

Assay of sulfa drugs can be determined by this reaction with sodium nitrite.

0.1 N Bromine is employed as:

A precisely manufactured glass tube with graduations enabling to measure the volume of liquid delivered through the stopcock at the bottom.

Dichlorophenol-indophenol solution is standardized using:

1 N HCl VS can be standardized using:

Method II of determining iodine value is also known as:

Residual titration method is also known as:

To determine the total ash, the sample is incinerated at a temperature of 675 ± 25°C. This temperature is represented by:

The standard substance used in checking the cleanliness of Abbe refractometer by determining its refractive index is:

Coulometric titration of water determination is also known as:

Perchloric acid in glacial acetic acid and perchloric acid in dioxane are volumetric solution used in what type of analysis?

The primary standard used in the standardization of the above VS is:

Which of the following statement/s is/are true? I. Phenol is assayed using residual iodometry using excess bromine solution. II. 0.1 N Bromine solution contains potassium bromide and potassium bromate. III. Bromine vapor is liberated from KBr and KBrO3 in basic environment.

A 1.5 g of liquefied phenol was dissolved in enough water to make 1000 mL. A 30 mL sample of the solution was treated with 30 mL of 0.1 N Bromine solution and HCl. The mixture was treated with KI and titrated with 8.7 mL of 0.1 N sodium thiosulfate. It was also found that 21 mL of 0.1 N sodium thiosulfate was required in the titration of the iodine liberated when 20 mL of the bromine solution was treated with KI and HCl. Compute for the % phenol in the sample. MW Phenol = 94.

Hydrolysis products of ASA:

The measurement of a base of a given sample by titration of standard acid is:

A characteristic of a substance which is suitable for non-aqueous titrimetry is:

To remove stain of KMnO4, the most effective chemical substance is:

The oxidation number of Mn in KMnO4 is:

Which of the following chemicals is not included in preparing the Karl Fischer reagent?

The process in which the exact concentration of solution is determined:

Titer is an expression of concentration of solution is determined:

Methyl orange in base medium is colored:

Assay of zinc oxide is what type of analysis?

The indicator used if weak acid is titrated with strong alkali:

Phenolphthalein in alkali medium is colored:

Suppository that does not melt at body temperature is what kind of defect?

Performs and evaluate microbiological assay, sterility, pyrogen, and bacteriological test, safety or acute toxicity test:

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.

When the alcoholic KOH is used to neutralize the acid and saponify the ester of 1 g of oil or fat, the constant determined is:

The instrument used to measure the optical activity of the sample is:

Analysis in which separation of the constituents from the sample is done and then weighing the product is:

The end point of iodometry using starch TS as indicator is:

Which of the following statement/s is/are correct? I. Ester value is the number of mg of KOH required to saponify the ester in 1 g of fat or oil. II. Ester value = saponification value + Acid value III. Ester value determination is applicable to fats, volatile oils, and alcohols.

Which of the following area is not a responsibility of quality control manager?

Hexane is the best solvent extracting:

What is the other name of Koettsdorfer number?

The unsaponifiable matter present in animal fats is:

The crude fiber of a drug usually consist of:

The unsaponifiable matter present in vegetable oils and fats is:

If a 0.47 g sample of potassium iodide yielded 0.7564 g of silver iodide precipitate by gravimetric assay, compute for the % purity of the potassium iodide. MW KI = 165.90; MW AgI = 234.76

Which of the following volumetric solutions is used in diazotization analysis of sulfa drugs?

Phenol is assayed using this method of analysis.

Calculate the molarity of sodium nitrite volumetric solution, if 31.6 mL of this solution reacts with 0.5004 g of sulfanilamide (C6H8N2O2S) to reach an end point. MW of sulfanilamide = 172.2

A 0.5110 g sample of sulfathiazole was assayed using 18.8 mL of 0.1005 M sodium nitrite solution in a titration. Each mL of 0.1 M sodium nitrite is equivalent to 25.53 mg of C9H9N3O2S2. Calculate the % C9H9N3O2S2 in the sample.

Which of the following standard solutions is not used in redox titration?

Assay of ASA (raw material) is an example of what method of analysis?

Assay of sodium nitrite is an example of what method of analysis?