Final answer:
The Solubility Product Constant for silver cyanide suggests low equilibrium concentrations of silver and cyanide ions when dissolved in water. Using the example of silver chloride with a similar Ksp, the resulting concentrations are also low. The correct option for the given question is 'C. Low'.
Step-by-step explanation:
Solubility Product Constant (Ksp) is an equilibrium constant that applies to the dissolving of a sparingly soluble ionic compound. When a compound like silver cyanide is dissolved in water, its equilibrium concentrations of silver (Ag+) and cyanide (CN-) ions can be deduced from its Ksp value.
In the case of silver cyanide, since you've mentioned its Ksp value is very low (-1.2x10 is not a standard scientific notation, assuming it should be 1.2x10 to a negative power), this indicates a very low solubility in water. Therefore, the equilibrium concentrations of Ag+ and CN- ions in the solution would be considered low as per Le Chatelier's principle.
Using the given data for silver chloride, with a Ksp of 2.79 × 10-10, the concentrations for Ag+ and Cl- are both at 1.67 × 10-5 M. This would demonstrate a low solubility similar to what we would expect for silver cyanide with a small Ksp.
The correct option in the final answer would hence be 'C. Low' equilibrium concentrations of silver and cyanide ions based on the Solubility Product Constant provided.