Calculate approximate pH of the resultant solution formed by titration of 25mL of 0.04 M Na2CO3 with 50mL of 0.025M HCl [Given : pKa1 = 6.4 and pKa2 = 10.3; for H2CO3]

Na2CO3+ HCl →NaHCO3+ NaClmilli moles= 1= 1.25 1-1=01.25-1 = 0.2511Na2CO3 is the limiting reagent and so all of will be converted to NaHCO3 which will further react with the leftover HCl in the following reaction. NaHCO3+ HCl →H2CO3+ NaClmilli moles10.2500 1 - 0.25 = 0.750.25 - 0.25 = 00.250The resultant solution contains a weak diprotic acid H2CO3 and an incomplete amphiprotic salt NaHCO3. The amphiprotic substance will not show its acidic behaviour as there is a stronger acid H2CO3 is present. The system is a buffer

Calculate approximate pH of the resultant solution formed by titration of 25mL of 0.04 M Na2CO3 with 50mL of 0.025M HCl [Given : pKa1 = 6.4 and pKa2 = 10.3; for H2CO3]

Na2CO3+ HCl →NaHCO3+ NaClmilli moles= 1= 1.25 1-1=01.25-1 = 0.2511Na2CO3 is the limiting reagent and so all of will be converted to NaHCO3 which will further react with the leftover HCl in the following reaction. NaHCO3+ HCl →H2CO3+ NaClmilli moles10.2500 1 - 0.25 = 0.750.25 - 0.25 = 00.250The resultant solution contains a weak diprotic acid H2CO3 and an incomplete amphiprotic salt NaHCO3. The amphiprotic substance will not show its acidic behaviour as there is a stronger acid H2CO3 is present. The system is a buffer