What is the concentration of the Ag+ ion in a saturated solution of AgCl?(Ksp for AgCl = 1.7 × 10−10)
Correct answer: C. 1.3 × 10−5 M
- A. 1.7 × 10−10 M
- B. 3.4 × 10−10 M
- C. 1.3 × 10−5 M
- D. 2.6 × 10−5 M
Explanation
The solubility product constant (Ksp) for AgCl is given by the equation Ksp = [Ag+][Cl-]. In a saturated solution of AgCl, the concentration of silver ions [Ag+] is equal to the concentration of chloride ions [Cl-]. Let this common concentration be x. Therefore, Ksp = x2. Given that Ksp = 1.7 × 10−10, we solve for x by taking the square root: x = √(1.7 × 10−10) = 1.3 × 10−5 M. This means the concentration of Ag+ ions in the saturated solution is 1.3 × 10−5 M. The other options are incorrect as they either misuse the Ksp value or misinterpret the stoichiometry of the equilibrium.
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