The product of the concentrations of each ion in a saturated solution of a sparingly soluble salt at 298 K, raised to the power of their relative concentrations is:
Correct answer: A. Ksp
- A. Ksp
- B. Ka
- C. Kw
- D. Kb
Explanation
Solubility product, Ksp, is the mathematical product of the dissolved ions concentration raised to the power of their stoichiometric coefficients.An acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution.Kb is the base dissociation constant. The base dissociation constant is a measure of how completely a base dissociates into its component ions in water.The equilibrium constant, Kw, is called the dissociation constant or ionization constant of water.
Last updated
About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
Practise Chemical Equilibrium
625 free Chemical Equilibrium MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Exams that ask Chemistry questions like this
Chemistry is on 12 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
Related questions
1.8 x 10 -5 is the dissociation constant of:
1 mole of CH3COOH and 1 mole of C2H5OH react to produce 2/3 mole of CH3COOC2H5. The equilibrium constant is
1 mole of ethyl alcohol was treated with one mole of acetic acid at 25°C. 2/3 of the acid changes into ester at equilibrium. The equilibrium constant of the reaction will be:
2HF ⇌ H2 + F2 PCI5 ⇌ PCI3 + Cl2The statement that is false about the Ke of both the reactions is;
2O3 ⇌ 3O2 Ke = 1055 at 25°C, it explains