the acid-base reaction between HCl and NaOH produces a solution with a pH of 7 at the equivalance point (NaCl+H2O). why does an acid-base indicator that changes color at pH 5 or 9. work just as well for this reaction as on that changes colors at pH 7

Calculate the expected pH based on how the solution was prepared, again allowing for any dilution taking place. For Solutions 7 and 8, make sure to take into account the acid–base reaction that occurs when an acid or base is added to the buffer.

When a solution is titrated with an base, an indicator (HIn) changes from yellow to blue (In). The Ka of the indicator is 8.00e - 06. At what pH will the indicator color change first be visible? pH = 6.0969 X 0%

1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point. c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant.  Calculate the molarity of the NaOH solution.  The titration reaction equation is:NaOH (aq)  +  HCl (aq)  →  NaCl (aq)  +  H 2O (l)