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