1. The problem statement, all variables and given/known data Calculate the equilibrium constant if you are given gibbs energy for the following molecules NH3=-26kJ/mol H2O-237.13kJ/mol NH4+=-79.31kJ/mol OH-=157.3kJ/mol How many moles of NH4Cl must be added to 1.0L of 0.10M NH3 to make a buffer whose pH is 9.0? 2. Relevant equations Henderson hasselbach equation, delta G=RTlnK 3. The attempt at a solution 1) How do you calculate equilibrium constant if you don’t have the temperature to use G=RTlnK 2) For the second half the question, I am thinking of using Henderson hasselbach equation to determine the concentration of NH4Cl. If not, how should I go about solving this question.