[Olympiad] The solubility of BaSO₄ is 1.05 × 10⁻⁵ mol/L. Calculate its solubility product (Ksp).
-
1.10 × 10⁻¹⁰
-
1.05 × 10⁻¹⁰
-
2.10 × 10⁻⁵
-
1.10 × 10⁻⁵
📝 Detailed explanation
Ksp = [Ba²⁺][SO₄²⁻]. Since it's a 1:1 salt, Ksp = s² = (1.05 × 10⁻⁵)² = 1.1025 × 10⁻¹⁰.
← Previous
→ Next
Space — Show answer
🎯 Take a test on the topic «Variant #5 of the University Scholarship Examination»
This topic contains 49 questions.
Test your knowledge!
🔐 Log in to take the test
📚 All tests by subject «Bio+Chem»
View all collections and topics in Bio+Chem
Go to subject →
