Question

You are given 100.0 mL of a 1.00x10³ M aqueous solution of HX-type molecules and 100.0 mL of a 1.00x10³ M aqueous solution of YCl-type molecules, where H represents hydrogen and Cl represents chlorine; neither X nor Y participates in acid-base chemistry.The solution-phase balanced reaction of HX-type with YCl-type molecules to form neutral YX strongly favors the products: \mathrm{HX}(a q)+\mathrm{YCl}(a q)+\mathrm{H}_{2} \mathrm{O}(\mathrm{b}) \rightarrow \mathrm{YX}(a q)+\mathrm{H}_{3} \mathrm{O}+(a q)+\mathrm{Cl}(a q) For parts (b)-(d), you wish to keep the solution's pH close to 6.70 as the molecules react.To do so, you make 500. mL of a 0.200 M buffer solution at the desired pH of 6.70 using a weak monoprotic acid having pKa = 6.60 and a salt of its conjugate base. 2. (b) What are the number of moles of the weak monoprotic acid nacid and the number of moles of the salt of the conjugate base nej-base that you would add to the 500. mL of pure water in order to form the buffer at the desired pH? 2. (c) Suppose you add the 100. mL solution of the HX-type molecules and the 100. mL solution of the YCl-type molecules from part (a) to the 500. mL of buffer solution from part (b). What is the pH after equilibration? What is the pK, of the conjugate base of the weak monoprotic acid?

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