If 1 liter solution has 4.4mol HCl, 4.6mol NaOH and 0.50mol HA is added together what is the pH when the resulting solution reaches equilibrium?
As we can see from the question that no. of moles of H+ are 4.4+0.50.hence total no. of H+ moles= 4.9.
No.of moles of OH- are 4.6 moles.
Hence 4.6 moles of H+ will react with 4.6 moles of OH- .to form 4.6 moles of H2O.
Thus (4.9-4.6) moles of H+ will remain unreacted.Hence pH of resultant 1 litre solution in equilibrium is to be calculated.
concentration of H+ ion= No. of moles/no. of litres of solution
= 0.3/1= 0.3M
pH= -(log(H+)) = -(log(0.3))= 1-0.4771 = 0.5229.
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