Part B To calculate the concentration of silver ions in the simulation, you need to convert the number of dissolved ions Into moles. Then divide this
number of moles by the volume in liters.
How would the concentration of silver ions compare in a 1.0 x 10-16L saturated solution to a 1.5 x 10-16L saturated solution? Write a hypothesis
first, and then test your hypothesis using the simulation. To simulate a saturated solution, put in enough silver bromide that you can clearly see
that it stops dissolving. Calculate the concentrations of silver lons at both of these volumes.

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.