MCQ – Volumetric Analysis Sr. No . 1
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The number of gm-equivalent of the solute per liter of solution is known as a) Normality c) Molarity b) Molality d) Mole fraction The number of gm-mole of the solute per liter of solution is known as a) Normality c) Molarity b) Molality d) Mole fraction The number of gm-mole of the solute per kg of solution is known as a) Normality c) Molarity b) Molality d) Mole fraction The ratio of number of gm-mole of a component to total number of gmmole in mixture or solution is known known as a) Normality c) Molarity b) Molality d) Mole fraction The number of gms of solute per 100 ml of solvent is known as a) Normality Normalit y c) % weight by volume b) Molality d) Mole fraction The chemical reagent from which solution of required concentration can be prepared is a) Secondary standard c) Dilute solution b) Concentrated solution d) Primary standard In neutralization neutralizat ion titration, acid react with a base to form a) Salt and water c) salt and acid b) Neutral solution d) Concentrated solution In strong acid – strong base titration, the pH of mixture at initial stage is find out by formula H + a) P = -log[H ] + b) [H ] = NaV a – Nb Vb / (Va + Vb) OH c) P = -log[OH ] d) [OH ] = NbV b – NaVa/ (Va + Vb) In strong acid – strong base titration, the pH of mixture before equivalence point is find out by formula H + a) P = -log[H ] + b) [H ] = NaV a – Nb Vb / (Va + Vb) OH c) P = -log[OH ] d) [OH ] = NbV b – NaVa/ (Va + Vb) In strong acid acid – strong base titration, the pH of mixture after equivalence point is find out by formula H + a) P = -log[H ] + b) [H ] = NaV a – Nb Vb / (Va + Vb) OH c) P = -log[OH ] d) [OH ] = NbV b – NaVa/ (Va + Vb) The PH of titration mixture for Strong acid – Strong base titration at equivalence point is a) 4 c) 2.7 b) 7 d) 9.2 The titration in which voltage or potential of the titration mixture is measured with the help of redox electrode is a) Precipitation titration c) Acid base titration
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b) Complexometric titration d) Potentiometric titration The titration in which there is formation of co-ordination complex is a) Precipitation titration c) Acid base titration b) Complexometric titration d) Potentiometric titration Stability of coordination complex depends upon a) PH of titration mixture b) Ability of metal ion and ligand to form complex c) Nature of complex d) All of above If the titration mixture contains two metal ions ,then quantity of one of them can be found by masking other metal is a) EDTA titration c) Masking method b) Redox method d) Complexometric method A ligand is molecule or ion which can donate a pair of electron for formation of a) Co ordinate bond with metal ion b) Covalent bond with metal ion c) Ionic bond with metal ion d) None of these The indicator which is not added in titration flask but kept on a spot plate is a) Self indicator c) External indicator b) Internal indicator d) None of these Internal indicators for redox titration is a) Strong oxidizing agent or strong reducing agent b) Weak oxidizing agent or weak reducing agent c) Weak oxidizing agent or strong reducing agent d) Strong oxidizing agent or weak reducing agent +4 +4 In a Potentiometric titration of Ce ion vs Fe ion solution , electrode potential at equivalence point is a) 0.71 V c) 0.75 V b) 1.45 V d) 1.1 V An equivalent quantity of I 2 liberated from oxidizing reagent during titration against Na 2S2O3 is a) Iodimetric titration c) Precipitation titration b) Potentiometric titration d) none of these The titration of KMnO 4 against oxalic acid or FeSO 4 is example of a) Iodimetric titration c) Precipitation titration b) Potentiometric titration d) Redox titration The titration during which reactant react to form ………… is precipitation titration. a) Water soluble solid product b) Metal indicator complex c) Water insoluble solid product d) Water soluble indicator In Precipitation titration , organic dye is used as a) Absorption indicator c) self indicator b) Adsorption indicator d) External indicator The weak acid – weak base titration are not performed practically because a) Reaction between weak acid and weak base is slow. H b) P change at equivalence point is not sharp c) Difficult to notice correct end point d) All of above All the indicators for acid- base titration are
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a) Weak organic acid or weak organic base b) Strong organic acid and weak organic base c) Weak organic acid and weak organic base d) None of these Colour change at PH interval for the organic acid indicator is H H a) 4 P units c) 2 P units H H b) 0 P units d) 1 P units The solution of known concentration is a) Dilute solution c) concentrated solution b) Standard solution d) none of these The chemical reagent from which solution of exact concentration cannot be prepared is a) Secondary standard c) Dilute solution b) Concentrated solution d) Primary standard In Mohr’s method of precipitation titration, 1 ml 1M AgNO3 = ….. . mg Cl = 80 mg Br = …….mg I a) 36.5 , 126 c) 34.5 , 128 b) 37.5 , 125 d) 35.5 , 127 The reagent which forces other molecule or ion to liberate electron in a) Oxidizing agent c) reducing agent b) Molecule d) atom The reagent which forces other molecule or ion to capture electron in a) Oxidizing agent c) reducing agent b) Molecule d) atom The reagent of known concentration which is taken in burette is a) Titrand c) Titration b) Titrant d) End point The unknown solution whose concentration is to be determined by titration is a) Titrand c) Titration b) Titrant d) End point Addition of titrant from burette into titration flask till titrant react completely is a) Titrand c) Titration b) Titrant d) End point In weak acid – strong base titration ,the PH of titration mixture at initial stage is find out by formula H + a) P = -log[H ] H b) P of acidic buffer= P Ka + log [salt] / [weak acid] H c) P = ½ PKw + ½ PKa – ½ pC OH d) P = -log[OH ] In weak acid – strong base titration ,the PH of titration mixture before equivalence point is find out by formula H + a) P = -log[H ] H b) P of acidic buffer= P Ka + log [salt] / [weak acid] H c) P = ½ PKw + ½ PKa – ½ pC OH d) P = -log[OH ] In weak acid – strong base titration ,the PH of titration mixture at equivalence point is find out by formula H + a) P = -log[H ] H b) P of acidic buffer= P Ka + log [salt] / [weak acid] H c) P = ½ PKw + ½ PKa – ½ pC
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d) P = -log[OH ] In weak acid – strong base titration ,the PH of titration mixture after equivalence point is find out by formula H + a) P = -log[H ] H b) P of acidic buffer= P Ka + log [salt] / [weak acid] H c) P = ½ PKw + ½ PKa – ½ pC OH d) P = -log[OH ] In weak base – strong acid titration ,the PH of titration mixture at initial stage is find out by formula H + a) P = -log[H ] OH b) P of basic buffer= P Ka + log [salt] / [weak base] H c) P = ½ PKw - ½ PKb + ½ pC H OH d) P = 14 - P In weak base – strong acid titration ,the PH of titration mixture before equivalence point is find out by formula H + a) P = -log[H ] b) POH of basic buffer= P Ka + log [salt] / [weak base] H c) P = ½ PKw - ½ PKb + ½ pC H OH d) P = 14 - P In weak base – strong acid titration ,the PH of titration mixture at equivalence point is find out by formula H + a) P = -log[H ] OH b) P of basic buffer= P Ka + log [salt] / [weak base] H c) P = ½ PKw - ½ PKb + ½ pC H OH d) P = 14 - P In weak base – strong acid titration ,the PH of titration mixture after equivalence is find out by formula a) PH = -log[H+] OH b) P of basic buffer= P Ka + log [salt] / [weak base] H c) P = ½ PKw - ½ PKb + ½ pC H OH d) P = 14 - P 40 ml of 0.2 N HNO3 solution is titrated against 0.2 N NaOH from burette. H The P of mixture at initial stage is ….. a) 0.92 b) 0.29 b) 1.46 d) 1.00 40 ml of 0.2 N HNO3 solution is titrated against 0.2 N NaOH from burette. H The P of mixture at 22.5 ml NaOH addition stage is ….. a) 3.32 c) 7.00 b) 2.32 d) 0.92 40 ml of 0.2 N HNO3 solution is titrated against 0.2 N NaOH from burette. H The P of mixture at 24 ml addition stage is ….. a) 0.92 c) 0.29 b) 1.46 d) 7.00 40 ml of 0.2 N HNO3 solution is titrated against 0.2 N NaOH from burette. H The P of mixture at 25 ml addition stage is ….. a) 0.92 c) 11.49 b) 1.46 d) 1.00 10 ml of Na2CO3 on titration against 0.05 N HCl from burette, gives end pt 6.7 ml, using methyl orange indicator. Hence normality of Na 2CO3 is ………….N a) 0.0225 c) 0.1 b) 0.052 d) 0.0335
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20 ml NaHCO3 solution is titrated against N/40 H 2SO4 solution gives end point 16.2 ml using phenolphthalein indicator. The gm/lit of NaHCO 3 is…….. a) 1.7 c) 7.2 b) 2.7 d) 3.7 If 0.1 N Ce+4 ion solution from burette is added in 100 ml 0.1 N Fe+2 ion solution in flask. The electrode potential of mixture is………volts at 10 ml Ce+4 added. a) 1.1 c) 1.4 b) 0.69 d) 0.96 If 0.1 N Ce+4 ion solution from burette is added in 100 ml 0.1 N Fe+2 ion solution in flask. The electrode potential of mixture is………volts at 100 ml Ce+4 added. a) 1.1 c) 1.4 b) 0.69 d) 0.96 If 0.1 N Ce+4 ion solution from burette is added in 100 ml 0.1 N Fe+2 ion solution in flask. The electrode potential of mixture is………volts at 120 ml Ce+4 added. a) 1.1 c) 1.4 b) 0.69 d) 0.96 If 0.1 N Ce+4 ion solution from burette is added in 100 ml 0.1 N Fe+2 ion solution in flask. The electrode potential of mixture is………volts at 50 ml Ce+4 added. a) 0.69 c) 1.4 b) 0.75 d) 0.96 + A given solution of Fe is diluted to volume 250 ml. 25 ml of this solution +2 in titration against 0.05 N KMnO 4 takes 18.4 ml up to end point. The Fe ion quantity in the given solution is …… a) 412.36 mg c) 134.21 mg b) 341.25 mg d) 513.36 mg 75 ml of 0.2 N NaOH is diluted to 250 ml volume. Normality of diluted solution is ……… a) 0.06 N b) 0.04 N c) 0.01 N d) 0.05 N If 0.5 M K2Cr2O7 (mole.wt-294) solution will be required to make 5 lit. of 0.1 N solution. The volume of stock solution will be ………ml a) 266.76 b) 166.67 c) 149.36 d) 21.6 A solution is prepared by dissolving 20 ml ethyl alcohol (density- 0.86) in 100 ml water. The mole fraction of ethyl alcohol and water , in solution is a) 0.327 b) 0.721 c) 0.937 d) 0.793 50 ml of the water sample requires 12.5 ml of the EDTA from burette, in H +2 the titration at P 12. The amount of Ca ions is……..mg per litre. a) 250 b) 125 c) 215 d) 150 ++ If 50 ml of a solution containing Ca is titrated against 0.035 M disodium EDTA from burette to get the end point 20.4 ml in the complex metric ++ titration . The amount of Ca in solution is………mg per lit. a) 671.2 b) 172.6 c) 762.1 d) 571.2 The weight of H2C2O4.2H2O (Mole.Wt.= 126) required to make 500 ml of 0.2 N solution is a) 6.3 gm b) 3.6 gm C) 5.6 gm d) 4.6 gm The weight of KMnO 4 required to make 500 ml 0.1 N KMnO 4, for titration in acidic medium………….. gm a) 6.15 b) 1.56 c) 2.65 d) 4.12
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The volume of concentrated H 2SO4 (98%) required to make 1 lit. of 2N H2SO4 is……….ml, if the density of concentrated H 2SO4 is 1.8 gm/ml. a) 54.44 b) 52.11 c) 55.56 d) 56.41 If 5.3 gm of Na2CO3 anhydrous is dissolved in water to make 1200 ml of solution, then molarity of solution is ……. M a) 0.024 b) 0.24 c) 0.42 d) 0.042 If 5.3 gm of Na2CO3 anhydrous is dissolved in water to make 1200 ml of solution, then normality of solution is ……. N a) 0.084 b) 0.84 c) 0.48 d) 0.048 Equivalent weight of K 2Cr2O7 (mole.Wt.=294) is ……… using ion electron method a) 63 b) 49 c) 94 d) 36 Equivalent weight of H 2C2O4.2H2O (mole.Wt.=120) is ……… using ion electron method a) 63 b) 49 c) 94 d) 36 Equivalent weight of KBrO 3 (mole.Wt.=167) is ……… using ion electron method a) 63 .87 b) 49 .14 c) 27.83 d) 36.27 If 15.3 ml of 0.1 N KOH solution from burette is added in 25 ml 0.08 N H H2SO4, the P of mixture is …… a) 3.19 b) 4.21 c) 0.19 d) 1.93 If 30 ml 0.12 N HCl solution from burette is added in 20 ml 0.11 N sodium H bicarbonate solution in flask.. The P of titration mixture is a) 6.917 b) 1.796 c) 2.647 d) 1.621 100 ml of 0.1 N weak acid (Ka = 1.2 x 10 ) in conical flask is titrated against 0.2N NaOH from burette. The PH at initial stage of titration is a) 4.2 b) 6.38 c) 3.96 d) 6.39 100 ml of 0.1 N weak acid (Ka = 1.2 x 10 ) in conical flask is titrated against 0.2N NaOH from burette. The PH at equivalence point of titration is a) 9.87 b) 6.38 c) 3.96 d) 6.39 100 ml of 0.1 N weak acid (Ka = 1.2 x 10 ) in conical flask is titrated against 0.2N NaOH from burette. The PH at 51 ml addition stage of is a) 4.2 b) 6.38 c) 3.96 d) 11.12 Match the following 1) Neutralization Titration P) formation of coordination compound 2) Precipitation titration Q) oxidation reduction reaction 3) Redox titration R) Formation of salt and water 4) Complexometric titration S) formation of precipitate a) 1-R , 2- S , 3- Q , 4- P b) 1- Q , 2- R , 3- P ,4- S Match the following 1) Methyl Orange 2) Phenolphthalein 3) Bromothymol blue 4) Alizarin Yellow R a ) 1- R , 2- P , 3- S , 4- Q b) 1- Q , 2- R , 3- P ,4- S
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Match the following 1) Phenol red
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c) 1- R , 2- P , 3- S , 4- Q d) 1- S , 2- Q ,3- R , 4- P P) Yellow – orange red Q) Yellow - blue R) Orange - yellow S) Colourless - pink c) 1-R , 2- S , 3- Q , 4- P d) 1- S , 2- Q ,3- R , 4- P
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2) Methyl red 3) Phenolphthalein 4) Methyl orange
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a ) 1- R , 2- P , 3- S , 4- Q b) 1-R , 2- S , 3- Q , 4- P Match the following 1) Methyl orange 2) Phenolphthalein 3) Methyl red 4) Bromothymol blue a ) 1- R , 2- P , 3- S , 4- Q b) 1- S , 2- Q ,3- R , 4- P Match the following 1) Phenol red 2) Alizarin Yellow R 3) Methyl Orange 4) Phenolphthalein
Q) Colourless - pink R) Yellow - Red S) Red - yellow c) 1- Q , 2- R , 3- P ,4- S d) 1- S , 2- Q ,3- R , 4- P
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c) 1- Q , 2- R , 3- P ,4- S d) 1-R , 2- S , 3- Q , 4- P P) Colour change at PH 8.3 – 10 Q) Colour change at PH 3.1 – 4.4 R) Colour change at PH 6.8 – 8.4 S) Colour change at PH 10.1 – 12 c) 1- R , 2- P , 3- S , 4- Q d) 1- S , 2- Q ,3- R , 4- P
a ) 1- R , 2- P , 3- S , 4- Q c) 1- Q , 2- R , 3- P ,4- S Match the following 1) Acetic acid 2) Sodium bicarbonate 3) Hydrochloric acid 4) Sodium hydroxide
c) 1-R , 2- S , 3- Q , 4- P d) 1- S , 2- Q ,3- R , 4- P
a) 1-R , 2- S , 3- Q , 4- P b) 1- Q , 2- R , 3- P ,4- S
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P) Colour change at PH 6 – 7.6 Q) Colour change at PH 4.2 – 6.3 R) Colour change at PH 3.1 – 4.4 S) Colour change at PH 8.3 – 10
a) 1-R , 2- S , 3- Q , 4- P b) 1- Q , 2- R , 3- P ,4- S Match the following 1) Phosphoric acid 2) Calcium hydroxide 3) Nitric acid 4) Potassium hydroxide a ) 1- R , 2- P , 3- S , 4- Q b) 1-R , 2- S , 3- Q , 4- P Match the following 1) Perchloric acid 2) Sodium hydroxide 3) Benzoic acid 4) Organic amines
a ) 1- R , 2- P , 3- S , 4- Q b) 1- S , 2- Q ,3- R , 4- P Match the following 1) Mohr’s Method 2) Fajan’s Method 3) Volhard Method 4) Idometric Titration
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P) Strong base Q) Strong acid R) weak acid S) weak base c) 1- Q , 2- R , 3- P ,4- S d) 1- S , 2- Q ,3- R , 4- P P) weak base Q) weak acid R) Strong acid S) Strong base
P) Strong base Q) Strong acid R) Weak acid S) Weak base c) 1- Q , 2- R , 3- P ,4- S d) 1-R , 2- S , 3- Q , 4- P P) Starch + Q) Fe 3 ion solution R) 5% K2CrO4 S) 0.5 % Organic dye c) 1- R , 2- P , 3- S , 4- Q d) 1- S , 2- Q ,3- R , 4- P
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Match the following 1) Self Indicator 2) Starch Indicator 3) Internal Indicator 4) External Indicator
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c) 1-R , 2- S , 3- Q , 4- P d) 1- S , 2- Q ,3- R , 4- P P) Zinc Q) AgCl R) K2Cr2O7 S) Na2C2O4
a ) 1- R , 2- P , 3- S , 4- Q c) 1- Q , 2- R , 3- P ,4- S b) 1- S , 2- Q ,3- R , 4- P d) 1-R , 2- S , 3- Q , 4- P Match the following 1) Mohr’s Method P) Self Indicator 2) Volhard’s Method Q) Adsorption Indicator 3) Fajan’s Method R) Formation of soluble coloured compounds 4) Redox Titration S) Formation of coloured precipitate a) 1-R , 2- S , 3- Q , 4- P c) 1- R , 2- P , 3- S , 4- Q b) 1- Q , 2- R , 3- P ,4- S d) 1- S , 2- Q ,3- R , 4- P Match the following 1) Primary Standard for Neutralisation titration. P) K 2Cr2O7 2) Primary Standard for Complexometric titration Q) AgNO 3 3) Primary Standard for Precipitation titration R) Potassium hydrogen phthalate 4) Primary Standard for Redox titration S) ZnSO 4 a ) 1- R , 2- P , 3- S , 4- Q b) 1-R , 2- S , 3- Q , 4- P
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P) Potassium Ferricynaide Q) Weak oxidizing or weak reducing agent R) KMnO 4 S) Iodimetric titration
a ) 1- R , 2- P , 3- S , 4- Q c) 1- Q , 2- R , 3- P ,4- S b) 1-R , 2- S , 3- Q , 4- P d) 1- S , 2- Q ,3- R , 4- P Match the following 1) Strong acid- Strong base Titration P) Not performed practically 2) Strong base -Weak acid titration Q) NH 4OH Vs HCl 3) Strong acid - Weak base titration R) NaOH Vs HCl 4) Weak acid - Weak base titration S) NaOH Vs CH 3COOH a ) 1- R , 2- P , 3- S , 4- Q b) 1- Q , 2- R , 3- P ,4- S Match the following 1) Oxidizing agent 2) Reducing agent 3) Salts 4) Metal
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c) 1- Q , 2- R , 3- P ,4- S d) 1- S , 2- Q ,3- R , 4- P
