• Phenol OH groups have an approximate pKa of 10, while NaHCO3 (the conjugate acid of Na2CO3) has a pKa of 10.3. This means the phenol and it’s conjugate base (phenoxide) should exist in equilibrium (1:1) in the basic solution; however, phenoxide is the major product of this reaction. What might account for this shift in equilibrium? (Hint: data on the previous page and in the first step of the procedure will help you) • Would sodium bicarbonate (NaHCO3) work as the base in this experiment? Explain why or why not.

your answer would be “dry”

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.