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The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what?
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The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 ...
Understanding Solubility and Solubility Product
The solubility product (Ksp) is a constant that reflects the extent to which a sparingly soluble salt dissolves in water. For barium sulfate (BaSO4), the dissolution can be represented as:
BaSO4 (s) ⇌ Ba²⁺ (aq) + SO4²⁻ (aq)
Given Data
- Solubility of BaSO4 = 2.42 × 10^-3 g/L
- Molar mass of BaSO4 = 233.39 g/mol (approximately)
Calculating Molar Solubility
- To find the molar solubility (S), convert grams per liter to moles per liter:
- S = (2.42 × 10^-3 g/L) / (233.39 g/mol)
- S ≈ 1.04 × 10^-5 mol/L
Expression for Ksp
- The Ksp expression for BaSO4 is:
Ksp = [Ba²⁺] [SO4²⁻]
- From the dissolution reaction, we can see that for every mole of BaSO4 that dissolves, one mole of Ba²⁺ and one mole of SO4²⁻ are produced.
Calculating Ksp
- Therefore, at equilibrium:
- [Ba²⁺] = S and [SO4²⁻] = S
- Ksp can be expressed as:
Ksp = S × S = S²
- Plugging in the molar solubility:
Ksp = (1.04 × 10^-5)²
Ksp ≈ 1.08 × 10^-10
Final Result
- The solubility product for BaSO4 at 298 K is approximately 1.08 × 10^-10. This value indicates the extent to which BaSO4 can dissolve in water, showcasing its low solubility.
The solubility product (Ksp) is a constant that reflects the extent to which a sparingly soluble salt dissolves in water. For barium sulfate (BaSO4), the dissolution can be represented as:
BaSO4 (s) ⇌ Ba²⁺ (aq) + SO4²⁻ (aq)
Given Data
- Solubility of BaSO4 = 2.42 × 10^-3 g/L
- Molar mass of BaSO4 = 233.39 g/mol (approximately)
Calculating Molar Solubility
- To find the molar solubility (S), convert grams per liter to moles per liter:
- S = (2.42 × 10^-3 g/L) / (233.39 g/mol)
- S ≈ 1.04 × 10^-5 mol/L
Expression for Ksp
- The Ksp expression for BaSO4 is:
Ksp = [Ba²⁺] [SO4²⁻]
- From the dissolution reaction, we can see that for every mole of BaSO4 that dissolves, one mole of Ba²⁺ and one mole of SO4²⁻ are produced.
Calculating Ksp
- Therefore, at equilibrium:
- [Ba²⁺] = S and [SO4²⁻] = S
- Ksp can be expressed as:
Ksp = S × S = S²
- Plugging in the molar solubility:
Ksp = (1.04 × 10^-5)²
Ksp ≈ 1.08 × 10^-10
Final Result
- The solubility product for BaSO4 at 298 K is approximately 1.08 × 10^-10. This value indicates the extent to which BaSO4 can dissolve in water, showcasing its low solubility.
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The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what?
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The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what?.
The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility of BaSo4 in water is 2.42 into 10 to the power minus 3 gram per litre at 298 Kelvin the value of solubility product will be what?.
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