Question

Calculate the [OH-], the pH and the % ionization for 0.25 mol/L ammonia solution.

Answer 1

I don't want the answer. I'm confused about how to get the equation (the R in RICE table), and how they just pulled Kb from their @ss (all that was given is above).

Answer 2

How is Kb = 1.8X10^-5 ?
Where is this coming from?!

Answer 3

@Compassionate @ikram002p @YanaSidlinskiy @MrNood @gorv @tester97 @ShadowLegendX @thadyoung @marylou004 @Joel_the_boss

Answer 4

Any ideas gorv or ikram002p?

Answer 5

concentration is give in Q ...u know the formula??

Answer 6

no I do not

Answer 7

wait, the morality equation?

Answer 8

M = mol/L
.25 = NH4/L

Answer 9

NH4 = 18 g/mol
but where does the .25 and *10^-5 come into play?
@gorv

Answer 10

http://chemistry.bd.psu.edu/jircitano/acidbase.html

Answer 11

lol it is ammonia solution not ammonia alone

Answer 12

NH4OH=0.25

Answer 13

\[35 g/mol * L ^{-1} = 0.25 M\]
What do you mean? How do I find Kb from this?

Answer 14

@gorv

Answer 15

what we have to do here buddy??

Answer 16

use ice table?

Answer 17

http://www.chemteam.info/AcidBase/Calc-Kb-from-data.html

Answer 18

u calculated pH??

Answer 19

check this link ...we will calculate pH and thn use as told in link..if got any prob ...jst tag me up i willl be here :)

Answer 20

cool beans.
so I'm finding pH first, then Kb

Answer 21

yeah ...first link is for pH