We have (a) 50.0 mL of 0.10 M NH3 solution, (b) 50.0 mL of 0.12 M HNO3 solution, (c) 50.0 mL of 0.12 M NaOH solution, and (d) 50.0 mL of 0.06 M HClO4 solution. Can you make a buffer by combining two of these solutions? If so, which ones? What would be the pH of the buffer solution? Please explain
By combining the solutions of the weak base NH3 (a) and the strong acid HClO4 (d) a buffer is formed.
HClO4 reacts with NH3 (decreasing it) and NH4 + is formed (increasing it), the initial moles of NH3 and HClO4 are calculated:
n NH3 = M * V = 0.1 M * 0.05 L = 0.005 mol
n NH4 + = 0.06 M * 0.05 L = 0.003 mol
The final moles of NH3 are calculated:
n NH3 = 0.005 - 0.003 = 0.002 mol
The pH is calculated:
pH = pKa + log n Salt / n Acid = 9.24 + log (0.002 / 0.003) = 9.06
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