An aqueous solution contains dissolved NH4Cl and NH3. The equilibrium concentrat

Question

An aqueous solution contains dissolved NH4Cl and NH3. The equilibrium concentration of NH3 is 0.550 M and the pH is 8.95. Determine the equilibrium concentration of NH4. Calculate pH after 0.10 moles of NaOH(s) is added to 1.00 L of this solution. Assume there is no change in volume upon addition of the NaOH. The Kb of NH3 is 1.8 x10^-5. An aqueous solution contains dissolved NH4Cl and NH3. The equilibrium concentration of NH3 is 0.550 M and the pH is 8.95. Determine the equilibrium concentration of NH4. Calculate pH after 0.10 moles of NaOH(s) is added to 1.00 L of this solution. Assume there is no change in volume upon addition of the NaOH. The Kb of NH3 is 1.8 x10^-5.

Explanation / Answer

pOH = pKb + log (salt) / (base)

14 - pH = -log(1.8*10^-5) + log (salt) / (0.55)

14 - 8.95 = -log(1.8*10^-5) + log ((x) / (0.55))

X = 1.1108 M

pOH = pKb + log ((salt) - (base) / (base) + (base))

14 - pH = (-log(1.8*10^-5)) + log ((1.1108 - 0.1) / (0.55 + 0.1))

pH = 9.0635

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