Hey there! Sign in to join this conversationNew here? Join for free
x Turn on thread page Beta

Acid dissociation constants watch

Announcements
    • Thread Starter
    Offline

    0
    ReputationRep:
    hey i would really appreaciate if someone could help me, what is the reason for leaving water out in the acid dissociation constant. In my books it says, that water is in excess, so if it is excess, why doesnt it alter the equilibvrium position to the right, according to le chatliers priciple.
    So when ethanoic acid is in water, only 0.1 % disscoiates, but isnt the large concetration of water likey to push the quilibrium to the other side?
    HELP PLEASE IM STUCK!!!
    Offline

    0
    ReputationRep:
    errrrk

    Could Kw have anything to do with it?

    Kw=[H+][OH-], where [H+] = [OH-]?
    Offline

    0
    ReputationRep:
    water is a liquid, and hence cannot be used in Ka expressions as only (aq) and (g) apply in Ka expressions, as liquids are fully concentrated.

    is this why?
    Offline

    0
    ReputationRep:
    wot it is is the water is in such a large excess that even when u alter its volume or concentration a lot it makes no impact on the Ka sum. e.g the amount u alter it makes no change to the overall value of the water!!
    hope this makes sense, im not too good at explaining wot i mean!!
 
 
 
Poll
Do you like carrot cake?

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Write a reply...
Reply
Hide
Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.