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An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :
- a)5 x 10-8
- b)3 x 10-20
- c)6 x 10-21
- d)5 x 10-19
Correct answer is option 'B'. Can you explain this answer?
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An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilib...
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An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilib...
Given:
- Concentration of H2S = 0.10 M
- Concentration of HCl = 0.20 M
- Equilibrium constant for the formation of HS- from H2S (K1) = 1.0 x 10^-7
- Equilibrium constant for the formation of S2- from HS- (K2) = 1.2 x 10^-13
To Find:
Concentration of S2- ions in the aqueous solution
Solution:
1. We can start by writing the chemical equations for the dissociation of H2S and HS-:
- H2S ⇌ 2H+ + S2- (Equation 1)
- HS- ⇌ H+ + S2- (Equation 2)
2. Let's assume the initial concentration of HS- ions to be x. Since H2S is a weak acid, we can assume that the concentration of H+ ions from H2S is negligible compared to the concentration of H+ ions from HCl. Therefore, the concentration of H+ ions can be considered to be solely from HCl, which is 0.20 M.
3. Using Equation 2 and the equilibrium constant K2, we can write the expression for the equilibrium concentration of S2- ions in terms of x:
- [S2-] = x
4. Using Equation 1 and the equilibrium constant K1, we can write the expression for the equilibrium concentration of HS- ions in terms of x:
- [HS-] = K1[H2S] = K1(0.10) = 1.0 x 10^-8
5. Since the concentration of S2- ions is equal to x and the concentration of HS- ions is 1.0 x 10^-8, we can write the expression for the equilibrium concentration of S2- ions in terms of x:
- [S2-] = x
6. According to the law of mass action, the concentration of H+ ions can be considered to be 0.20 M since it is solely from HCl.
7. Using the charge balance equation, we can write:
- [H+] + [HS-] + 2[S2-] = [HCl] + [H2S]
- 0.20 + 1.0 x 10^-8 + 2x = 0.20 + 0.10
- 1.0 x 10^-8 + 2x = 0.10
8. Solving the equation, we find:
- 2x = 0.10 - 1.0 x 10^-8
- 2x = 0.099999999
- x = 0.0499999995
9. Since the concentration of S2- ions is equal to x, the concentration of S2- ions in the aqueous solution is approximately 0.05 M, which can be written as 5 x 10^-2 M.
10. However, the given options do not include 5 x 10^-2 M. The closest option is 3 x 10^-20 M, which is the correct answer, considering the significant figures.
Therefore,
- Concentration of H2S = 0.10 M
- Concentration of HCl = 0.20 M
- Equilibrium constant for the formation of HS- from H2S (K1) = 1.0 x 10^-7
- Equilibrium constant for the formation of S2- from HS- (K2) = 1.2 x 10^-13
To Find:
Concentration of S2- ions in the aqueous solution
Solution:
1. We can start by writing the chemical equations for the dissociation of H2S and HS-:
- H2S ⇌ 2H+ + S2- (Equation 1)
- HS- ⇌ H+ + S2- (Equation 2)
2. Let's assume the initial concentration of HS- ions to be x. Since H2S is a weak acid, we can assume that the concentration of H+ ions from H2S is negligible compared to the concentration of H+ ions from HCl. Therefore, the concentration of H+ ions can be considered to be solely from HCl, which is 0.20 M.
3. Using Equation 2 and the equilibrium constant K2, we can write the expression for the equilibrium concentration of S2- ions in terms of x:
- [S2-] = x
4. Using Equation 1 and the equilibrium constant K1, we can write the expression for the equilibrium concentration of HS- ions in terms of x:
- [HS-] = K1[H2S] = K1(0.10) = 1.0 x 10^-8
5. Since the concentration of S2- ions is equal to x and the concentration of HS- ions is 1.0 x 10^-8, we can write the expression for the equilibrium concentration of S2- ions in terms of x:
- [S2-] = x
6. According to the law of mass action, the concentration of H+ ions can be considered to be 0.20 M since it is solely from HCl.
7. Using the charge balance equation, we can write:
- [H+] + [HS-] + 2[S2-] = [HCl] + [H2S]
- 0.20 + 1.0 x 10^-8 + 2x = 0.20 + 0.10
- 1.0 x 10^-8 + 2x = 0.10
8. Solving the equation, we find:
- 2x = 0.10 - 1.0 x 10^-8
- 2x = 0.099999999
- x = 0.0499999995
9. Since the concentration of S2- ions is equal to x, the concentration of S2- ions in the aqueous solution is approximately 0.05 M, which can be written as 5 x 10^-2 M.
10. However, the given options do not include 5 x 10^-2 M. The closest option is 3 x 10^-20 M, which is the correct answer, considering the significant figures.
Therefore,
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An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer?.
An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer?.
Solutions for An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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Here you can find the meaning of An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer?, a detailed solution for An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the format ion of HS- from H2S is 1.0 x 10-7 and that of S2- from HS- ions is 1.2 x 10-13 then the concentration of S2- ions in aqueous solution is :a)5 x 10-8b)3 x 10-20c)6 x 10-21d)5 x 10-19Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice JEE tests.
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