What is the pH of a solution with a [ ^- OH] of 4.1 *10 ^- ³ M? A) "-2.39" B) "2.39" C) "11.6" D) "-11.6" E) "7.00"

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Quizplus · Accepted Answer

The given notation [F1F1F1S1^F1F1F10OH] refers to the concentration of ions in the solution. It does not provide any direct information about the pH of the solution. To calculate pH, we need to use the formula: pH = -log[H+] where [H+] is the concentration of hydrogen ions in the solution. Since the problem does not provide the concentration of hydrogen ions directly, we need to find it through a series of calculations. Step 1: Identify the relevant acid-base equilibrium. The formula contains several polyatomic ions, but the only one that can act as an acid or a base is H^. This ion can either accept a proton (H+) to form H2, or it can donate a proton to form ^F1F1F10. H^ H+ + ^F1F1F10 Step 2: Write the expression for the acid dissociation constant (Ka). Ka = [H+][^F1F1F10]/[H^] Step 3: Substitute the given concentrations into the expression for Ka. [F1F1F1S1^F1F1F10OH] = [H^] + [^F1F1F10] = 4.1 x 10^-13 M + 1.3 x 10^-9 M = 1.3000000000000041 x 10^-9 M [F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10³ M] = [H+] + [^F1F1F10] = x + 1.3 x 10^-9 M Ka = (x)(1.3 x 10^-9 M)/(1.3000000000000041 x 10^-9 M) = x Step 4: Solve for x using the quadratic formula. Ka = x^2/(1.3 x 10^-9 - x) x = 9.69 x 10^-7 M Step 5: Calculate pH. pH = -log[H+] pH = -log(9.69 x 10^-7) pH = 6.015 The closest answer choice to 6.015 is C, "11.6". However, this answer is not correct. Looking at the answer choices, it seems that there may be a formatting error in the problem. The answer that comes closest to the calculated pH of 6.015 is actually A, "2.39".

What Is the PH of a Solution with a [