  We have classified the silver halides like AgBr as insoluble compounds, but in truth, a small amount of these compounds does dissolve in water:AgBr (s) Ag^+(aq) + Br^–(aq)The equilibrium constant for this type of reaction is given the special name of “solubility product” and denoted by the symbol Ksp.(14a): Suppose a 10.0-g chunk of silver bromide is dropped into 150.0 mL of pure water. If the solubility product Ksp for silver bromide is 5.0×10-13 at 25 °C, then what will be the equilibrium concentrations of silverand bromide ions in the solution?(14b): What will happen to the concentration of dissolved silver bromide if more solid AgBr is added to thebeaker?

Question

We have classified the silver halides like AgBr as insoluble compounds, but in truth, a small amount of these compounds does dissolve in water:
AgBr (s) Ag^+(aq) + Br^–(aq)
The equilibrium constant for this type of reaction is given the special name of “solubility product” and denoted by the symbol Ksp.
(14a): Suppose a 10.0-g chunk of silver bromide is dropped into 150.0 mL of pure water. If the solubility product Ksp for silver bromide is 5.0×10-13 at 25 °C, then what will be the equilibrium concentrations of silver
and bromide ions in the solution?
(14b): What will happen to the concentration of dissolved silver bromide if more solid AgBr is added to the
beaker?

Step 1

a) Solubility product may be defined as the product of concentration of dissolved ions each raised to the power equals to their respective stoichiometric coefficients.

Mathematically,

Let’s say we have a chemical reaction as:

Step 2

Here the chemical reaction is:

Step 3

Molarity= It may be defined as the moles of solute ...

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