0 votes, 0 avg 44 Created by Kamran FatehTitration Complete QuizTitration is a laboratory method used to determine the concentration of a solution by gradually adding a reagent of known concentration until a reaction reaches completion, often indicated by a color change. This technique is essential in chemistry for analyzing acids, bases, and other reactive substances in various samples. 1 / 60Which of the following is the primary objective of a titration? To determine the color of the solution To measure the temperature of the solution To find the concentration of an unknown solution To observe the boiling point of the solution 2 / 60In an acid-base titration, the point at which the acid has completely reacted with the base is called the End point Equivalence point Halfway point Starting point 3 / 60Which of the following indicators would be suitable for a titration between a strong acid and a weak base? Methyl orange Phenolphthalein Bromothymol blue All 4 / 60If 25.0 mL of 0.1 M NaOH is required to completely neutralize 50.0 mL of HCl, what is the concentration of the HCl? 0.025 M 0.05 M 0.1 M 0.2 M 5 / 60Which piece of laboratory equipment is primarily used to deliver the titrant in a titration? Beaker Pipette Burette Flask 6 / 60What is the role of the indicator in a titration? To speed up the reaction To provide a color change at the endpoint To stabilize the solution To measure the pH directly 7 / 60In a titration of a weak acid with a strong base, the pH at the equivalence point is: Less than 7 Exactly 7 Greater than 7 cannot be determined 8 / 60Which of the following is a common indicator used in Complexometric titrations Erichrome Black T Bromothymol blue KMnO4 None 9 / 60What is the typical color change observed with Eriochrome Black T as an indicator in complexometric titrations? Red to blue Yellow to red Blue to red Colorless to pink 10 / 60Hardness of water can be determined by which titration Acid-base Complexometric Iodometric Precipitation 11 / 60Which of the following indicators is commonly used in redox titrations Methyl orange Starch Bromothymol blue Methyl Red 12 / 60Which of the following is used as an indicator in the titration of iodine with hypo? Methyl red Methyl orange Starch Potassium ferricyanide 13 / 60The amount of NaOH used in the titration of 100 ml 0.1 N HCl is 4g 0.04g 2g 0.4g 14 / 60The pH range of methyl orange as an indicator is 3-5 8-9 2-4 6-8 15 / 60What will be the pH at the equivalence point in the titration of a weak acid and a strong base? 0 Greater than 7 Less than 7 7 16 / 60Which of the following represents the equivalence point in the graph of pH Vs volume of titrant? Point at the highest pH Point at the greatest magnitude of the slope of the curve Point at the lowest pH Point at the least magnitude of the slope of the curve 17 / 60The normal rain water is acidic due to SO2 NO2 NH3 CO2 18 / 60The equivalent weight of an acid can be calculated by Molecular weight × basicity Molecular weight/basicity Molecular weight × acidity Molecular weight/acidity 19 / 60The ideal indicator for the titration of strong acid and weak base should have pH range between 5-8 4-6 8-10 7-8 20 / 60Which of the following titrations will have the equivalence point at a pH more than 8? HCl and NH3 CH3COOH and NH3 HCl and NaOH CH3COOH and NaOH 21 / 60What is the molarity of the solution of barium hydroxide, if 35 ml of 0.1 M HCl is used in the titration of 25 ml of the barium hydroxide solution? 0.37 0.07 0.28 0.14 22 / 60Which of the following is used as an indicator in the titration of a weak acid and a strong base? Bromothymol blue (6 to 7.5) Methyl orange (3 to 4) Methyl red (5 to 6) Phenolphthalein (8 to 9.6) 23 / 60What is the concentration of the sulphuric acid solution, if 100 ml of the solution is neutralised by 50 ml of 0.5 M Ba(OH)2 solution? 0.25M 50M 0.50M 0.75M 24 / 60A difference between strong and weak acid is presence and absence of halogen ions negative and positive pH complete and partial ionization proton donation and electron acceptance 25 / 60If 30 ml of acid is neutralised by 15 ml of 0.2 N alkali, then the concentration of acid is 0.4 N 0.1 N 0.25 N 0.50 N 26 / 60Find the concentration of HCl, if 10 ml of 0.5 M Ca(OH)2is required to titrate 50 ml of HCl. 5 M 1/10 M 1/5 M 10 M 27 / 60Which of the following is the primary function of a redox indicator in redox titrations? To maintain the pH of the solution To facilitate the redox reaction To signal the endpoint by changing color To prevent side reactions 28 / 60In iodometric titrations, why is starch used as an indicator? It reacts directly with iodine It provides a color change at the endpoint It stabilizes the iodine solution It accelerates the redox reaction 29 / 60Which of the following redox titration methods is suitable for determining the concentration of chloride ions? Iodometric titration Permanganate titration Ceric sulfate titration Volhard method 30 / 60Why is potassium dichromate (K₂Cr₂O₇) often used as a primary standard in redox titrations? It is inexpensive It is unstable and reacts readily It has a known purity and high molar mass It requires no indicator for endpoint detection 31 / 60What is the purpose of redox titration? To determine the pH of a solution To find the concentration of an oxidizing or reducing agent To determine the temperature of a solution To measure the volume of a gas 32 / 60Which solution is often used as a self-indicating oxidizing agent in redox titrations? Sodium chloride (NaCl) Potassium permanganate (KMnO₄) Hydrochloric acid (HCl) Sodium hydroxide (NaOH) 33 / 60Which indicator is commonly used in iodine-based redox titrations? Phenolphthalein Methyl orange Starch Bromothymol blue 34 / 60What is the color change at the endpoint of a potassium permanganate titration? Pink to colorless Colorless to pink Blue to yellow Yellow to green 35 / 60What is complexometric titration primarily used for? Determining the concentration of acids and bases Measuring the concentration of oxidizing agents Determining metal ions in a solution Identifying the pH of solutions 36 / 60Which of the following is commonly used as a chelating agent in complexometric titrations? Phenolphthalein Potassium permanganate Ethylenediaminetetraacetic acid (EDTA) Sodium chloride 37 / 60EDTA is a type of: Acid-base indicator Complexing agent Reducing agent Precipitating agent 38 / 60In complexometric titration, the indicator Eriochrome Black T changes color when it: Binds to free metal ions Binds to EDTA Reaches endpoint in acidic solutions Is in the presence of strong oxidizers 39 / 60Which metal ion is typically determined using complexometric titration with EDTA? Chloride ions Iron ions Calcium ions Nitrate ions 40 / 60What color does the Eriochrome Black T indicator turn when the endpoint of a titration involving calcium ions is reached? Red to blue Yellow to red Green to purple Blue to yellow 41 / 60Which of the following metals cannot be easily titrated with EDTA due to its instability in solution? Magnesium Zinc Silver Copper 42 / 60The formation constant (Kf) for the EDTA complex with a metal ion is typically high because: EDTA forms weak bonds with metal ions EDTA has multiple binding sites, leading to a stable complex EDTA is soluble in both acidic and basic solutions EDTA does not form stable complexes with transition metals 43 / 60In complexometric titration, which of the following metals forms the most stable complex with EDTA? Calcium Magnesium Copper Sodium 44 / 60The EDTA molecule binds to metal ions through which type of binding? Ionic bonds only Van der Waals forces Coordinate covalent bonds Hydrogen bonds 45 / 60Which indicator is used in the complexometric titration of nickel ions with EDTA? Murexide Eriochrome Black T Phenolphthalein Methyl orange 46 / 60Precipitation titration is primarily based on: Acid-base reactions Oxidation-reduction reactions Formation of an insoluble precipitate Formation of a complex 47 / 60Which of the following is commonly used as a titrant in precipitation titration to determine chloride ions? EDTA Silver nitrate Sodium hydroxide Potassium permanganate 48 / 60In precipitation titration, the endpoint is detected by: pH change Redox potential change Formation of a colored precipitate Formation of a colorless solution 49 / 60The Mohr method is a type of precipitation titration used to determine: Sulfate ions Carbonate ions Chloride ions Nitrate ions 50 / 60In the Mohr method, the indicator used is: Eriochrome Black T Starch Phenolphthalein Potassium chromate 51 / 60In the Mohr method, the endpoint is indicated by the formation of which colored precipitate? Yellow Red Green White 52 / 60The Volhard method is typically used to determine: Chloride ions Nitrate ions Ammonium ions Sulfide ions 53 / 60Which of the following compounds acts as a back-titrant in the Volhard method? Silver nitrate Potassium chromate Ammonium thiocyanate Sodium chloride 54 / 60In the Fajans method, the indicator adsorption depends on: The ionic strength of the solution The presence of EDTA The formation of an insoluble precipitate The solubility product (Ksp) of the salt 55 / 60Which of the following indicators is commonly used in the Fajans method for the detection of chloride ions? Fluorescein Phenolphthalein Methyl orange Bromothymol blue 56 / 60In a back titration, the analyte is: Directly titrated with a standard solution Reacted with an excess of reagent, and the remaining reagent is then titrated Used to titrate another unknown solution Mixed with an indicator to observe a color change 57 / 60Which of the following is a primary reason to use back titration instead of direct titration? The analyte is very reactive The reaction between analyte and titrant is slow The analyte has no clear endpoint All of the above 58 / 60Which indicator would be suitable for a back titration involving the titration of excess acid with a base? Phenolphthalein Methyl orange Bromothymol blue Both a and b 59 / 60Back titration is often used to determine the concentration of: Weak acids and bases Insoluble salts Strong oxidizing agents All types of unknown solutions 60 / 60Back titration can be particularly useful in cases where: The end-point of direct titration is not clearly observable The reaction rate is extremely fast The analyte has a high molar mass The analyte is a strong acid or base Your score isThe average score is 80% 0% Restart quiz
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