28. 25.00 mL of a solution of a weak monoprotic acid, HX, was titrated with a 0.0640 M solution of NaOH, requiring 18.22 mL to neutralize the acid. If the Ka for the acid is 3.60*10-6, calculate the number of moles of a salt, NaX, that must be added to produce a pH of 6.00 in 150.00 mL of the original solution. You may assume that the temperature is 25 °C. It is impossible for a solution with this composition to have a pH of 6.00 0.00117 mol 0.0252 mol 0.0466 mol O 1.17 mol

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A: Here the Ph will be equal to Pka.

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Q: The Images provided are the way they want the problem to be solved, it's weird and I'm sorry about…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.