1
answer
0
watching
196
views
10 Nov 2019
A 20.00 mL solution of HClO_4 of unknown concentration is titrated with 33.55 mL of 0.09945 M NaOH solution. (a) Calculate the concentration of the unknown HClO_4 solution. (b) What is the pH of the solution before titration was started? (c) What is the pH of the solution when 75.00% of the acid has been neutralized? 45.51 mL of a 0.1011 M NaOH solution is used to neutralize 50.00 mL of an unknown acid. (a) Calculate the concentration of the unknown acid solution. The equivalence point was pH = 9.011 (b) What is the pK_a of the weak acid?
A 20.00 mL solution of HClO_4 of unknown concentration is titrated with 33.55 mL of 0.09945 M NaOH solution. (a) Calculate the concentration of the unknown HClO_4 solution. (b) What is the pH of the solution before titration was started? (c) What is the pH of the solution when 75.00% of the acid has been neutralized? 45.51 mL of a 0.1011 M NaOH solution is used to neutralize 50.00 mL of an unknown acid. (a) Calculate the concentration of the unknown acid solution. The equivalence point was pH = 9.011 (b) What is the pK_a of the weak acid?
Jamar FerryLv2
9 Apr 2019