# Using the general format of the Ksp equation figure out the molarity of both [K+] and [HC4H4O6-] if the theoretical Ksp= 3.8*10^-4 (Ksp= [K+][KC4H4O6-]

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Asked Mar 9, 2020
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Using the general format of the Ksp equation figure out the molarity of both [K+] and [HC4H4O6-] if the theoretical Ksp= 3.8*10^-4 (Ksp= [K+][KC4H4O6-]

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Step 1

All known compounds can be dissolve in certain solvents whereas they remain insoluble in other solvents. The solubility of any substance can be determined with the help of solubility product.

Step 2

Solubility product of any compounds can be defined as the mathematical product of dissolved ion concentrations of any compound raised to the power of their stoichiometric coefficients. It is represented as Ksp.

Step 3

The ionization of given potassium salt can be written in the given way:

Hence the Ksp expression must be:

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