Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Joules23 on March 08, 2008, 07:28:13 PM
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Calculate the pH after 0.020 mol NaOH is added to 1.00 L of each of the solutions below.
(a) 0.121 M HONH2 (Kb = 1.1 10-8)
(b) 0.121 M HONH3Cl
(c) pure H2O
(d) a mixture containing 0.121 M HONH2 and 0.121 M HONH3Cl
My attempt for (a)
HONH2 +OH- -> HONH- + H2O
.121----.02----.121
.101----0------.141
pH=pKa + Log (B/A)
pH=6.04 + log (.141/.101)
pH=6.18
(c) -log(1E-14/.02)= 12.03
im not sure how to do part b, or d
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How does HONH2 react with water? Hint: in a way it is similar to ammonia, it is a Brønsted-Lowry base.
Are you sure you have no idea how to do c? If so, you should get back to the water ion product (http://www.chembuddy.com/?left=pH-calculation&right=water-ion-product).
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Ok i got part (c) thanks, but still stuck on part a..
HONH2 + H20 -> HONH3+ + OH-
so would adding NaOH decrease HONH2 and increase OH-
-------------HONH2 + H20 -> HONH3+ + OH-
Before NaOH--.121------------.121--------0
After NaOH---.101------------.121-------.02
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Ok i got part (c) thanks, but still stuck on part a..
HONH2 + H20 -> HONH3+ + OH-
so would adding NaOH decrease HONH2 and increase OH-
Yes. Now, for obvious reasons NaOH is completely dissociated. HONH2 is a vey weak base. Will it be able to dissociate enough to change pOH just from NaOH? What is the pOH (or pH) of 0.121 HONH2 solution?
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Will it be able to dissociate enough to change pOH just from NaOH?
No?
What is the pOH (or pH) of 0.121 HONH2 solution?
pOH = 8.88
pH = 5.12
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What is the pOH (or pH) of 0.121 HONH2 solution?
pOH = 8.88
pH = 5.12
Show how you got these numbers. First of all - you have solution of base, yet your pH is acidic. But you have not simply switched pH with pOH - 8.88 is not a correct answer too :(
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ok i just redid it and i got pH = 9.56 .. i dont know what i did wrong last time, but i did it quickly so i probably enetred something incorrect int he calculator
1.1E-8=(x^2/.121)
x=3.648E-5=[OH-]
-log[OH-]=4.44=pOH
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9.56 it is :)
Now, what about b? What is HONH3Cl? How does it dissociate? Is there anything acidic/basic in the dissociation products?
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HONH3Cl --> HONH3+ + Cl-
no, so pH will be the same?
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No. HONH2 and HONH3+ are base and conjugated acid, just like NH3 and NH4+...
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HONH3+ + OH- --> HOHN2 + H2O
.121-------0-----------0
.101------.02----------0
?
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Or
HONH3+ <-> H+ + HONH2