Part a a solution is made by mixing 9.00 mmol (millimoles) of ha and 3.00 mmol of the strong base. what is the resulting ph? express the ph numerically to two decimal places.

Assuming that the reaction is unimolecular on both reactant and product sides such that:

HA  +  OH-   -->  A-  +  H2O

Therefore the amount of A- left is:

mmol HA = 9.00 - 3.00 = 6.00 
mmol A- = 3.00 

pKa = - log Ka = 5.25 

Calculating for pH:
pH = 5.25 + log 3.00/6.00

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.