Calculate the concentration of ion in the given solution using Ksp

Submitted by odonnek2 on Mon, 2012-07-23 21:22

Calculate the concentration of fluoride ions in a saturated solution of chromium fluoride (CrF_{3}). K_{sp}(CrF_{3}) = 6.6 x 10^{-11}.

Ksp are just a type of equilibrium constant where the Ksp is equal to the the product of the concentration of the dissolved ions raised to the power of their coefficients. For instance, in this case the equation showing the dissolving of CrF3 would be

CrF_{3} (s) ----> Cr^{3+} (aq) + 3 F^{- }(aq)

Therefore, the Ksp expression must be

Ksp = [ Cr3+ ] [ F- ]^{3}

Given the balanced equation for the dissociation of the CrF3, if the [Cr3+] is given a value of x, then the [F-] must be 3x. Plugging into the Ksp expression yields

Ksp are just a type of equilibrium constant where the Ksp is equal to the the product of the concentration of the dissolved ions raised to the power of their coefficients. For instance, in this case the equation showing the dissolving of CrF3 would be

CrF

_{3}(s) ----> Cr^{3+}(aq) + 3 F^{- }(aq)Therefore, the Ksp expression must be

Ksp = [ Cr3+ ] [ F- ]

^{3}Given the balanced equation for the dissociation of the CrF3, if the [Cr3+] is given a value of x, then the [F-] must be 3x. Plugging into the Ksp expression yields

Ksp = [ Cr3+ ] [ F- ]

^{3 }= [ x ] [ 3x ]^{3 }= 9x^{4}Since the value of the Ksp is known, x can be calculated along with [F

^{-}] or 3 x.spock

Mon, 2012-07-23 22:34