Answer:

Explanation:
Hello there!
In this case, given the solubilization of cadmium (II) hydroxide:

The solubility product can be set up as follows:
![Ksp=[Cd^{2+}][OH^-]^2](https://tex.z-dn.net/?f=Ksp%3D%5BCd%5E%7B2%2B%7D%5D%5BOH%5E-%5D%5E2)
Now, since we know the concentration of cadmium (II) ions at equilibrium and the mole ratio of these ions to the hydroxide ions is 1:2, we infer that the concentration of the latter at equilibrium is 3.5x10⁻⁵ M. In such a way, the resulting Ksp turns out to be:

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Oxidation
iron+oxygen happened
The answer is D. 459 g As
Answer:
The molarity of this solution is 0.156 M
Explanation:
Step 1: Data given
Mass of Ba(OH)2 = 1.90 grams
Molar mass Ba(OH)2 = 171.34 g/mol
Volume of the solution = 71.1 mL = 0.0711 L
Step 2: Calculate moles Ba(OH)2
Moles Ba(OH)2 = mass Ba(OH)2 / molar mass Ba(OH)2
Moles Ba(OH)2 = 1.90 grams / 171.34 g/mol
Moles Ba(OH)2 = 0.0111 moles
Step 3: Calculate molarity
Molarity solutin = moles Ba(OH)2 / volume solution
Molarity solution = 0.0111 moles / 0.0711 L
Molarity solution = 0.156 M
The molarity of this solution is 0.156 M