pKb

[Rohita Thammineni 2D]

Hi! On Achieve #10, are we supposed to convert to pOH and pKb when comparing to determine charged, neutral, or none? I'm a little confused on how this varies from Question #9 on the Achieve...

[Sophia Zhao]

If it helps, you can convert it. However, you can also note that since it's a base dissociating, you reverse the comparison you had to make in question 9.

[WendyN_L2]

Personally I don't thinks there's any need to convert it, just remember for weak acids when the pH is less than pKa, that means the neutral pronated HA is more dominate, otherwise if the pH greater pKa it is A- the charged species that is more predominate. For weak bases it is the opposite so pH < pKa it is now charged BH+, and if pH > pKa is it neutral B. Hope that helps

[SarahOMalley1D]

You don't need to convert it, but you definitely can if it helps you. I think we could be asked any variation of this question other than pKa vs pH for acids and pKb vs pOH for bases. For example, I'd be prepared to answer questions on pKb vs pOH for acids. Either way, you'll just need to keep relative concentrations of hydronium and hydroxide in mind.

[905767718]

There's no need to convert the values given in this problem as long as you can tell how strong each base is relative to the higher and lower concentration. If the pKb has a higher concentration than the solution, then it will be charged. The reverse applies that it will be neutrally charged.