If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,10 mol∙dm–3), calculate the pH at the equivalence point of the titration

You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?

a) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid to prepare a buffer with a pH = 3.50. Assume there is no change in volume upon addition of the sodium formate. b) Write the predominant chemical reaction that occurs when 0.050 mol of HClO4 is added to 1.00 L of the buffer prepared in part a and calculate the pH of the solution.

A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. The ka of ammonia is 5.68 X 10-10.  The pKa of ammonia is 9.25.  These questions are challenging so this is very similar to the one online but the answers will be a little different.    What is the initial pH of the solution?     A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 15.0 mL of HCl is added?      Calculate the pH at the equivalence point.         Calculate the pHat one-half equivalence point.       A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. What is the pH when 38.0 mL of HCl has been added?