Final answer:
Without the specific identity of the compound or its Ksp, we cannot calculate its exact solubility in 1 molar NaOH. However, the general approach involves using the molarity of NaOH to find the concentration of OH- ions, using Kw to find the concentration of H+ ions, and then determining the pH, before using the Ksp value for the compound to calculate its solubility.
Step-by-step explanation:
To provide correct answer by solving the solubility of an unknown compound in 1 molar NaOH, we must use a step-by-step approach. Although the question contains a typo referring to 'nios voltage', we can infer that it pertains to the solubility of a compound in a sodium hydroxide solution.
Firstly, the molarity of NaOH is 1 M, which indicates that there is 1 mole of NaOH per liter of solution. Since NaOH is a strong base and completely dissociates in water, the concentration of hydroxide ions [OH-] is also 1 M. Using the auto-dissociation constant for water (Kw = 1.0 x 10-14 at 25°C), we can calculate the concentration of hydrogen ions [H+] in the solution, which allows us to determine the pH.
Solubility Product Constant (Ksp) is an equilibrium constant for the dissolving process of a sparingly soluble salt. If we knew the Ksp of the compound in question, and assuming no common ion effect, we could calculate its molar solubility in the NaOH solution. For example, if we were dealing with aluminum hydroxide, Al(OH)3, and its Ksp was given, we could set up the equilibrium expression and solve for the solubility. However, without the identity of the compound or its Ksp value, we cannot provide a precise solubility value. Instead, a general process can be explained using examples and hypothetical values.