Abuffer solution is made using a weak acid, ha, with a pka of 5.28. if the ratio of a– to ha is 1.0 × 102, what is the ph of the buffer?

pH of a buffer solution can be calculated using the following equation:  

pKa is given as 5.28  

the ratio of A⁻ to HA is given as 1.0 × 10²

putting all the values in the equation;  

pH=5.28+log [1.0 × 10²]  

pH=7.28

SO, when a buffer solution is made using a weak acid, HA, with a pka of 5.28. if the ratio of A⁻ to HA is 1.0 × 10², the pH of the buffer is 7.28.

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.