Using the equation:
Ba(OH)2(s) --> Ba2+(aq) + 2OH-(aq)
<--
Delta H = 7820kJ
-How would the solubility of solid Ba(OH)2 in water be affected by an increase in pH? How about a decrease in pH? Need to use Le Chatelier's principal in reasoning
Ba(OH)2(s) --> Ba2+(aq) + 2OH-(aq)
<--
Delta H = 7820kJ
-How would the solubility of solid Ba(OH)2 in water be affected by an increase in pH? How about a decrease in pH? Need to use Le Chatelier's principal in reasoning
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To increase the pH, you're basically increasing the OH- concentration. If you do this, the reaction will shift in the reverse direction, by Le Chatelier's principle, where you shift away from an increase, thus producing more Ba(OH)2. The opposite goes for reducing the pH, where OH- will be reduced so the reaction will make less Ba(OH)2 and more Ba2.+