- #1
RNix25
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I've been working on this one for a few days, and I just can't seem to get the right answer.
Consider the reaction I2(s) --> I- (aq) + IO3- (aq)
Balanced= 3I2 + 6OH- --> 5I- + IO3- + 3H2O
deltaG°= -153.8 kJ/mol
The question: What pH is required for the reaction to be at equilibrium at 298 K when [I-]= 0.5 M and [IO3-]= 0.5 M
I know the answer is 9.21, but I just can't figure out how to get there. I started by finding Keq, which is 9.113 * 10^26, but I'm stumped from there. I would be extremely appreciative for a walkthrough to the final answer.
Consider the reaction I2(s) --> I- (aq) + IO3- (aq)
Balanced= 3I2 + 6OH- --> 5I- + IO3- + 3H2O
deltaG°= -153.8 kJ/mol
The question: What pH is required for the reaction to be at equilibrium at 298 K when [I-]= 0.5 M and [IO3-]= 0.5 M
I know the answer is 9.21, but I just can't figure out how to get there. I started by finding Keq, which is 9.113 * 10^26, but I'm stumped from there. I would be extremely appreciative for a walkthrough to the final answer.