Does the pH of the solution increase, decrease, or stay the same when you:
a.) Add solid sodium oxalate (Na2 C2 O4) to 50ml of 0.015m oxalic acid
b.) Add solid ammonium chloride to 100ml of 0.016m HCl
c.) Add 20g of NaCl to 1.0L of 0.012m sodium acetate, NaCH3COO
Explain why?
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a) will certainly become less acidic. The pH will increase. That's because the oxalate ion concentration has increased, so the equilibrium between
oxalic acid <-------> oxalate ion and proton
will have to shift back to the left to re-establish.
So som of the freshly introduced oxalate ions combine with protons and form the oxalic acid molecule.
b) the ammonium ion is capable of releasing protons. If you add it to a neutral or alkaline solution it will release protons to form ammonia.
However, in the presence of a strong acid the effect will hardly be noticeable.
in theory it would reduce the pH by dissociating into NH3 and H+, but the actual change in pH would be very small.
c) there is not even a theoretical reason for any change in pH in this example. Both salts dissociate completely. The acetate ion itsself will cause the solution to be weakly alkaline, but addition of NaCl won't change anything.