Question

Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M KOH(aq). Use the ionization constant for HClO.HClO.

What is the pH before addition of any KOH?KOH?

pH=pH=

What is the pH after addition of 25.0 mL KOH?25.0 mL KOH?

pH=pH=

What is the pH after addition of 35.0 mL KOH?35.0 mL KOH?

pH=pH=

What is the pH after addition of 50.0 mL KOH?50.0 mL KOH?

pH=pH=

What is the pH after addition of 60.0 mL KOH?60.0 mL KOH?

pH=pH=

https://sites.google.com/site/chempendix/ionization

Answer 1

* Before addition of any KOH the pH is completely dependent of the H+ ions coming from ionization of HClO.

  

* When we add 25 ml KOH,it starts reaction with HClO.

* After adding 35 ml of KOH

  

* After adding 50 ml KOH,

mol of HClO=0.01 mol

  mol of 50 mL of KOH = 0.2 mol/L * 50 mL * 1 L/1000 mL = 0.01mol

Same mole number indicates the Neutralisation point.

* As equivalence point is reached after 50 ml KOH addition,further KOH addition will increase the OH- concentrationin in the solution.So, we can calculate pH from the pOH value.