Correct Answer: Option C:<span> The equilibrium position will shift to the right toward the products.
Reason:
1) This problem is based on </span>Le Chatelier's principle. It is stated as '<em>any</em><span><em> changes in the temperature, volume, or concentration of a system will result in predictable and opposing changes in the system in order minimize this change and achieve a new equilibrium state.</em>'
2) In present case, the reaction involved is:
</span><span> CH3CO2H(aq) + H2O(l) ⇄ CH3CO2-(aq) + H3O+(l)
</span>Hence, when the concentration of acetic acid (reactant) is increased, the equilibrium will shift to right to minimize the effect of change in concentration of reactant.
Thermal energy from the sun that has transferred to the sidewalk
Answer:
D) 1.6 x 10⁻¹⁴
Explanation:
The solubility-product equilibrium constant for Ag₂SO₃ is given by the expression
Ksp = [Ag⁺]² [SO₃²⁻]
where [Ag⁺] and [SO₃²⁻] are the concentration of the species dissolved in solution for the equlibrium
Ag₂SO₃ (s) ⇄ 2 Ag⁺ + SO₃²⁻
we are given the concentration of Ag⁺ and from the stoichiometry of the equilibrium, the concentration of SO₃²⁻ is half that value, so
[Ag⁺]² = 3.2 x 10⁻⁵ M
[SO₃²⁻] = 3.2 x 10⁻⁵ M / 2 = 1.6 x 10⁻⁵ M
plugging these values into the solubility product constant equation we have
Ksp = (3.2 x 10⁻⁵)² x (1.6 x 10⁻⁵) = 1.6 x 10¹⁴
Therefore D is the correct answer.
