As a chemist for an agricultural products company, you have just developed a new

Question

As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the potential to kill weeds effectively. A sparingly soluble salt, Herbigon is dissolved in 1 M acetic acid for technical reasons having to do with its production. You have determined that the solubility product Ksp of Herbigon is 8.30×106. Although the formula of this new chemical is a trade secret, it can be revealed that the formula for Herbigon is X-acetate (XCH3COO, where "X" represents the top-secret cation of the salt). It is this cation that kills weeds. Since it is critical to have Herbigon dissolved (it won't kill weeds as a suspension), you are working on adjusting the pH so Herbigon will be soluble at the concentration needed to kill weeds. What pH must the solution have to yield a solution in which the concentration of X+ is 1.50×103 M ? The pKa of acetic acid is 4.76. Express your answer numerically.

Explanation / Answer

Apply the equation for Ksp

XCH3COO ========= X + CH3COO

Ksp = [X] * [CH3COO]

8.3 x 10-6 = (1.5 x 10-3) *x

x = CH3COO = 5.53 x 10-3 M

Apply handersson hasselbach equation

PH = PKa + log (CH3COO- / CH3COOH)

Concentration of CH3COOH = 1 M

PH = 4.76 + log (5.53 x 10-3 / 1 )

PH = 4.76 - 2.25 = 2.5029

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