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The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer?.

Solutions for The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11. Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.

Here you can find the meaning of The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer?, a detailed solution for The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice The percentage of copper in a copper(II) salt can be determined by using a thiosulphate titration. 0.305 gm of a copper(II) salt was dissolved in water and added to, an excess of potassium iodide solution liberating iodine according to the following equation2Cu2 (aq) + 4I– (aq) 2CuI(s) + I2(aq)The iodine liberated required 24.5cm3 of a 0.100 mole dm-3 solution of sodium thiosulphate2S2032- (aq) + I2(aq) →2I– (aq) + S4062- (aq)the percentage of copper, by mass in the copper (ll) salt is. [Atomic mass of copper = 63.5]a)64.2b)51.0c)48.4d)25.5Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice Class 11 tests.