A student following the procedure in this experiment prepared a solution by allowing 26.00 mL of a 0.120 M aqueous solution of NaOH to react with 50.00 mL of a 0.208 M aqueous solution of a weak acid, HA. The student diluted the resulting solution to a volume of 100.0 mL with distilled water. The student ten used a pH meter to determine the pH of the solution and found it to be 4.73.
* please answer all questions and show work*
A student following the procedure in this experiment prepared a solution by allowing 26.00 mL. of a 0.120 M aqueous solution of NaOH to react with 50.00 mL of a 0.208 M aqueous solution of a weak acid, HA. The student diluted the resulting solution to a volume of 100.0 mL. with distilled water. The student then used a plH meter to determine the pH of the solution and found it to be 4.73. 1.) What is the [ HO 1 for this solution? 2.) How many moles of the weak acid were initially added to the solution? Moles HA = 3.) How many moles of OH were initially added to the solution? Moles OH' = 4.) Complete and balance the equation for the neutralization reaction in this problem: HA (aq) + NaOH (aq) â 5.) Determine the number of moles of HA and A at equilibrium. Moles HA Moles A,- [HA] 6) Determine the molar concentrations of HA and A at equilbrium. IA 1 K. 7.) Calculate the value of K, for HA
