30 ml of 0.1N HCI is added from burette into 20 ml of 0.11 N NaHCO3solutions in flask. Calculate pH of the titration mixture.

To calculate the pH of the titration mixture, we first need to determine the moles of HCl and NaHCO3.

1. Calculate the moles of HCl and NaHCO3:

   Moles of HCl = Normality x Volume(L) = 0.1N x 30/1000 L = 0.003 moles Moles of NaHCO3 = Normality x Volume(L) = 0.11N x 20/1000 L = 0.0022 moles

2. Determine the limiting reactant:

   Since HCl is in excess (0.003 moles > 0.0022 moles), the reaction will go to completion and all of the NaHCO3 will react. The reaction is as follows:

   HCl + NaHCO3 -> NaCl + H2O + CO2

   This means that 0.0022 moles of HCl will react with 0.0022 moles of NaHCO3, leaving 0.003 - 0.0022 = 0.0008 moles of HCl unreacted.

3. Calculate the pH:

   The pH of a solution is given by the formula pH = -log[H+], where [H+] is the concentration of H+ ions in the solution. The unreacted HCl will dissociate completely into H+ and Cl- ions, so the concentration of H+ ions will be equal to the concentration of the unreacted HCl.

   [H+] = 0.0008 moles / total volume(L) = 0.0008 moles / (30+20)/1000 L = 0.016 M

   Therefore, pH = -log(0.016) = 1.80

So, the pH of the titration mixture is 1.80.