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The solubility product of a sparingly soluble salt BA2 is 4 × 10–12. The solubility of BA2 is[1999]
- a)4 × 10–4
- b)4 × 10–12
- c)4 × 10–3
- d)1 × 10–4
Correct answer is option 'D'. Can you explain this answer?
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The solubility product of a sparingly soluble salt BA2 is 4 × 10...
Solubility product = [x] [2x]2 = 4x3
∴ x = 10–4
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The solubility product of a sparingly soluble salt BA2 is 4 × 10...
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The solubility product of a sparingly soluble salt BA2 is 4 × 10...
The solubility product (Ksp) of a sparingly soluble salt BA2 is 4.
The solubility product (Ksp) is an equilibrium constant that describes the degree to which a sparingly soluble salt dissolves in water. It is calculated by taking the product of the concentrations of the ions in the saturated solution.
In this case, the solubility product (Ksp) of the salt BA2 is 4. This means that when the salt dissolves in water, it will dissociate into the ions B+ and A2-, and the product of their concentrations in the saturated solution will be equal to 4.
The solubility product expression for BA2 can be written as:
Ksp = [B+] * [A2-]
Note that the concentrations of the ions are raised to the power of their coefficients in the balanced chemical equation for the dissociation of the salt. In this case, the coefficient for B+ is 1 and for A2- is 1, so their concentrations are not raised to any power.
If the concentrations of B+ and A2- in the saturated solution are known, the solubility product can be calculated by multiplying their concentrations.
The solubility product (Ksp) is an equilibrium constant that describes the degree to which a sparingly soluble salt dissolves in water. It is calculated by taking the product of the concentrations of the ions in the saturated solution.
In this case, the solubility product (Ksp) of the salt BA2 is 4. This means that when the salt dissolves in water, it will dissociate into the ions B+ and A2-, and the product of their concentrations in the saturated solution will be equal to 4.
The solubility product expression for BA2 can be written as:
Ksp = [B+] * [A2-]
Note that the concentrations of the ions are raised to the power of their coefficients in the balanced chemical equation for the dissociation of the salt. In this case, the coefficient for B+ is 1 and for A2- is 1, so their concentrations are not raised to any power.
If the concentrations of B+ and A2- in the saturated solution are known, the solubility product can be calculated by multiplying their concentrations.
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The solubility product of a sparingly soluble salt BA2 is 4 × 10–12. The solubility of BA2 is[1999]a)4 × 10–4b)4 × 10–12c)4 × 10–3d)1 × 10–4Correct answer is option 'D'. Can you explain this answer?
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The solubility product of a sparingly soluble salt BA2 is 4 × 10–12. The solubility of BA2 is[1999]a)4 × 10–4b)4 × 10–12c)4 × 10–3d)1 × 10–4Correct answer is option 'D'. 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 solubility product of a sparingly soluble salt BA2 is 4 × 10–12. The solubility of BA2 is[1999]a)4 × 10–4b)4 × 10–12c)4 × 10–3d)1 × 10–4Correct answer is option 'D'. 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 solubility product of a sparingly soluble salt BA2 is 4 × 10–12. The solubility of BA2 is[1999]a)4 × 10–4b)4 × 10–12c)4 × 10–3d)1 × 10–4Correct answer is option 'D'. Can you explain this answer?.
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