Determine the OH, pH and pOH of a solution with a H concentration of 4.2 * 10(-9)M
Thanks everyone for your help!!
2006-11-19 11:00:36 · 5 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
ok anna.
the ionic product of water = [H+] [OH-]
the value of this is constant as is 1*10(-14) mol2dm-3
thus
1*10^-14=[4.2*10^-9]*[OH-] (which u are tryina find)
1*10(-14)/4.2*10(-9)= [OH-]
[OH-]=whatever answer u get when u put this in the calc
pH = -log [H+] REMEBER THE NEGATIVE!
= - log 4.2*10(-9)
= whatever answer u get when u put thisin ur calc (lol)
pOH= -log [OH-] REMEMBER THE NEGATIVE
= -log [the answer from the first part]
its basic
pH is MORE THAN 7!!
2006-11-19 11:16:54 · answer #1 · answered by Anonymous · 0⤊ 0⤋
The pH scale is the acid scale with 1 being the most acidic and 14 being the most basic. The pOH scale is just opposite of that.
The substance metioned above with pH 8.4 would make it a basic substance since 7 is considered neutral.
2006-11-19 11:03:53 · answer #2 · answered by mmonkeyccup 2 · 0⤊ 0⤋
its basic. all bases have pH > 7 and pOH < 7. if its pH or pOH =7, its neutral. pH is the negative log to base10 of H ion concerntration. i.e to find pH of your solution = -log 10 [4.2*10(-9)].
also pH +pOH = 14.
2006-11-19 11:11:48 · answer #3 · answered by kamozi 1 · 0⤊ 0⤋
pH above 7 is basic, so 8.4 would be basic and pH below 7 is acidic
2006-11-19 11:03:30 · answer #4 · answered by lilndnchick 1 · 0⤊ 0⤋
It's a base
2006-11-19 11:03:17 · answer #5 · answered by The Cheminator 5 · 0⤊ 0⤋