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Posted by on Tuesday, April 1, 2014 at 10:50pm.

calculate the pH in a solution prepared by dissolving .10 mol of solid NH4Cl in .500 L of .40 M NH3. Assuming no volume change.

  • Chemistry - , Tuesday, April 1, 2014 at 11:05pm

    This is a buffer problem.
    Use the Henderson-Hasselbalch equation.

  • Chemistry help - , Tuesday, April 1, 2014 at 11:33pm

    calculate the pH in a solution prepared by dissolving .10 mol of solid NH4Cl in .500 L of .40 M NH3. Assuming no volume change. Without the use of Henderson-hasselbalch

  • Chemistry - , Tuesday, April 1, 2014 at 11:44pm

    The HH equation is much easier but here is the other.
    (NH3) = 0.40M
    (NH4Cl) = (NH4^+) = (Cl^-) = mols/L = 0.1mol/0.500L = 0.2M
    ...........NH3 + HOH ==> NH4^+ + OH^-
    I........0.40..........0.20.......0
    C..........-x.............x.......x
    E.........0.40-x.......9,.20+x....x

    Kb = (NH4^+)(OH^-)/(NH3)
    Substitute the E line into Kb above and solve for x = (OH^-). Convert that to pH.
    Note: The NH4Cl is a common ion to the NH3 solution (the NH4^+ is the common ion) and the addition of the NH4^+ forces the ionization due to Kb to the left and that limits the basicity. You can assume, to make the solution easier, that 0.200+x = 0.200 and 0.4-x = 0.4.

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