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This is a classic acid/base problem. The answer to this question can be found by using the following equation, which relates pH and concentration of an acid: pH = -log[H+] + log(Ka) 9.2% dissociated means that for every 1 mole of HA, there are 9.2 moles of H+. Therefore, the Ka (the equilibrium constant for HA) is equal to 10-7 mol/L ionized. Plugging in these values into our equation gives us a solution with a pH of 8.6. This answer is correct because the pH of an acidic solution can’t be larger than 0 and a basic solution’s pH can’t be less than 14. If we apply our equation to this problem, it becomes: -log[0.92] + log(100) -log(-9100) + 100 100 (Since Ka=10100/molarity) = 9950 moles of H+. Plugging in these values into our equation yields us a final pH value of 13.06, which is greater than 14 but not as high as 12. Our answer for the question “What Is The Ph Of The Solution


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