Question: (a) What is the pH of 0.0333 M HNO3? Is the solution neutral, acidic or basic? (b) what is the pOH of 0.0347 KOH? Is the solution neutral, acidic or basic?
My Approach:
(a) I found pOH as 1.48 and then I calculated the pH using the Kw and got 12.5. It was also a basic solution.
(b) I found pH at 1.46 and then figured out pOH at 12.5...My conclusion is that it was basic solution.
So what do you think? Am I correct? What do you i need to fix? Thanks for all the help I get!
2007-03-10 19:20:01 · 3 answers · asked by Jimmy 3 in Science & Mathematics ➔ Chemistry
HNO3 is a strong acid HNO3>> H+ + NO3-
Concentration of H+ = 0.0333 M
pH= - log H+ = - log 0.0333 = 1.48 ( it is acid)
When you know concentration of H+ you have not use Kw
KOH is a strong base KOH >> K+ + OH-
Concentration of OH- = 0.0347 M
pOH = - log OH- = - log 0.0347 = 1.46
pH + pOH = 14
pH = 14 - pOH = 14 - 1.46 = 12.5 (it is basic )
2007-03-10 22:40:52 · answer #1 · answered by Anonymous · 0⤊ 0⤋
As long as pH and pOH add up to 14.0, you're on the right track!
pH < 7 = acidic
pH > 7 alkaline
pOH < 7 = alkaline
pOH > 7 = acidic
2007-03-10 19:39:43 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
U found the pH Of an acid soln greater than 7!!!!!!!!!!
its impossible, surely there lies some mistake. Otherwise the approach u have taken is correct.
Same in the case of (b). U found the pH of an alkaline soln less than 7 ie acidic. It's impossible.
2007-03-10 22:45:49 · answer #3 · answered by s0u1 reaver 5 · 0⤊ 0⤋