Kelarutan Dan Hasil Kali Kelarutan

Explanation
The given question is asking for the solubility of PbCl2. The Ksp value of 3.2x10-5 represents the equilibrium constant for the dissociation of PbCl2 in water. The higher the Ksp value, the more soluble the compound is. Therefore, a higher concentration of Pb2+ and Cl- ions will be present in solution. Among the given options, 2x10-2 M has the highest concentration, indicating the highest solubility of PbCl2.

Explanation
The correct answer is 2) CaCrO4. This is because the Ksp value for CaCrO4 is the highest among the given options, indicating that it is the most soluble in water. The higher the Ksp value, the greater the solubility of the compound in water.

Explanation
The solubility of CaCO3 in water at a certain temperature is given as 10-5 mol/liter. When CaCO3 is dissolved in a solution of Ca(NO3) with a concentration of 0.05 M, the solubility is expected to decrease. Therefore, the correct answer is 2x10-9, which is the option with the lowest solubility among the given choices.

Explanation
The solubility product constant (Ksp) is a measure of the maximum amount of a compound that can dissolve in a solvent at a given temperature. In this case, the Ksp of AgCl is given as 10-10. When AgCl dissolves in water, it dissociates into Ag+ and Cl- ions. According to the Ksp expression, [Ag+][Cl-] = 10-10. Since NaCl is a strong electrolyte, it completely dissociates into Na+ and Cl- ions. The concentration of Cl- ions in the NaCl solution is 0.1 M. To maintain equilibrium, the concentration of Ag+ ions must be equal to the concentration of Cl- ions. Therefore, the concentration of Ag+ ions in the solution is also 0.1 M. Using the Ksp expression, we can solve for [Ag+][Cl-] = (0.1)(0.1) = 0.01. Since [Ag+][Cl-] = 10-10, the concentration of Ag+ ions is 10-10 M, which is equivalent to 10-9 M. Therefore, the correct answer is 10-9 M.

Explanation
The given question is asking for the solubility of Mg(OH)2 in NaOH 0.1 M solution, with a given Ksp value of 1.8x10-11 mol3/L3. The Ksp value represents the equilibrium constant for the dissolution of the compound. By using the Ksp expression, we can determine the concentration of Mg2+ and OH- ions in the solution. In this case, the concentration of OH- ions in the NaOH solution is already known (0.1 M). By using the stoichiometry of the compound, we can calculate the concentration of Mg2+ ions, which is equal to the solubility of Mg(OH)2. Therefore, the correct answer is 1.8x10-9 mol/L.

Explanation
The Ksp (solubility product constant) of Mg(OH)2 can be calculated by using the formula Ksp = [Mg2+][OH-]^2. In this case, we are given the amount of Mg(OH)2 dissolved in water, which is 0.58 grams. We can convert this to moles by dividing by the molar mass of Mg(OH)2 (58 g/mol). The volume of water is also given, which is 200 mL. We can convert this to liters by dividing by 1000.

Using the moles of Mg(OH)2 and the volume of water, we can calculate the concentration of Mg2+ and OH-. Since Mg(OH)2 dissociates into one Mg2+ ion and two OH- ions, the concentration of Mg2+ will be equal to the moles of Mg(OH)2 divided by the volume of water, and the concentration of OH- will be equal to twice the moles of Mg(OH)2 divided by the volume of water.

Finally, we can substitute these values into the Ksp formula to calculate the Ksp of Mg(OH)2. The correct answer, 5x10-4, is the result of this calculation.

Explanation
The correct answer is 108x5. This is because the Ksp (solubility product constant) of a salt is the product of the concentrations of its ions in a saturated solution. In the case of Sr3(PO4)2, it dissociates into 3 Sr2+ ions and 2 PO43- ions. Therefore, the Ksp would be (3x)^3 * (2x)^2, where x is the concentration of Sr3(PO4)2. Simplifying this expression gives us 108x^5, which is the correct answer.

Explanation
The given question is asking for the solubility product constant (Ksp) of BaF2 at a certain temperature. The information provided states that 0.350 grams of BaF2 dissolves in water to form 1 liter of saturated solution. To find the Ksp, we need to calculate the concentration of Ba2+ and F- ions in the solution. Since the molar mass of BaF2 is 175 g/mol, we can calculate the moles of BaF2 dissolved. Dividing this by the volume of the solution gives us the concentration of Ba2+ and F- ions. The Ksp is then calculated by multiplying the concentrations of Ba2+ and F- ions together. The correct answer, 3.2x10-8, is the calculated Ksp value for BaF2 at the given temperature.

Explanation
The given question states that the saturated solution of L(OH)2 has a pH of 10. This indicates that the concentration of hydroxide ions (OH-) in the solution is high, resulting in a basic pH. The Ksp value represents the solubility product constant, which is the equilibrium constant for the dissolution of a sparingly soluble compound. In this case, the low Ksp value of 5x10-13 suggests that L(OH)2 is not very soluble in water, as it only dissociates to a small extent. Therefore, the correct answer is 5x10-13.