an aqueous buffer solution contains 0.018mol/L NaHCO3 and 0.024mol/L Na2CO3. A)d
ID: 476959 • Letter: A
Question
an aqueous buffer solution contains 0.018mol/L NaHCO3 and 0.024mol/L Na2CO3. A)determine the pH of the solution using Henderson hasselbach. B)determine pH of solution after 1.00mL of 6.00M HCl is added to 499.0 mL of the buffer solution. Assume final volume is 500.0mL. an aqueous buffer solution contains 0.018mol/L NaHCO3 and 0.024mol/L Na2CO3. A)determine the pH of the solution using Henderson hasselbach. B)determine pH of solution after 1.00mL of 6.00M HCl is added to 499.0 mL of the buffer solution. Assume final volume is 500.0mL. an aqueous buffer solution contains 0.018mol/L NaHCO3 and 0.024mol/L Na2CO3. A)determine the pH of the solution using Henderson hasselbach. B)determine pH of solution after 1.00mL of 6.00M HCl is added to 499.0 mL of the buffer solution. Assume final volume is 500.0mL.Explanation / Answer
A] NaHCO3 ------> Na2CO3
pH = pka + log [NaHCO3] / [Na2CO3]
pH = 10.3 + log [0.024/0.018]
pH = 10.425
B]
NaHCO3 --------> Na2CO3
On addtion of HCl
Moles of NaHCO3 = Molarity*V = 0.018*499 = 8.982 millimoles
Moles of Na2CO3 = 0.024*499 = 11.976 millimoles
Moles of HCl = 6 millimoles
NaHCO3 -------> Na2CO3 + H+
Equilibrium shifts to left forming more NaHCO3
8.982 11.976 6
8.982+6 11.976-6 0
pH = 10.3 + log [11.976-6] / [8.982+6]
pH = 9.9
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