Describe mathematically, the effect of a change in pH of 1.0 would have on # of H+ ions in solution?
2007-10-16 10:44:08 · 6 answers · asked by Keeks 3 in Science & Mathematics ➔ Chemistry
pH is defined as:
pH = -log(H+)
So, a change of 1.0 in pH will make an important change on number of H+ ions, Guess what, this change depends on the actual value of pH. It is not the same to change pH from 7.0 to 8.0 than to change pH from 11.0 to 12.0 You may demonstrate this by rearranging the equation above to obtain the concentration of H+ in solution. then calculate the difference of H+ concentration between pH 7.0 and pH 8.0, Do the same with pH's 11.0 and 12.0 You will find the difference between these two pH increments will be different. If you want a general expression for this, derivate the equiation, so you will not obtain a straight line, but rather a exponential equation.
2007-10-16 10:54:02 · answer #1 · answered by Manuelon 4 · 0⤊ 0⤋
10 times
2007-10-16 17:47:39 · answer #2 · answered by JAMES 4 · 0⤊ 0⤋
The pH is equal to -Log[H+]
So if you substitute 1 for the pH and solve for H+ you can get the value you're looking for.
pH = -Log[H+]
1 = -Log[H+]
-1 = Log[H+]
10^(-1) = [H+] and that should be the increase/decrease of H+ as a result of a pH change of 1.
2007-10-16 17:50:37 · answer #3 · answered by harshil.patel@sbcglobal.net 2 · 0⤊ 0⤋
I believe that with every change of 1 you have 10 times more H+ Ions.
ph 7 is 10^-7 , a ph 6 has 10^-6, check please
2007-10-16 17:49:57 · answer #4 · answered by Elke B 4 · 0⤊ 0⤋
i just learned that same thing in school >.<
well having a pH of 1.0 would make the solution more acidic....but i dont think that is what the question is asking...not sure, sorry.
2007-10-16 17:51:24 · answer #5 · answered by Anonymous · 0⤊ 0⤋
lots more H+ ions in a pH level of 1...than in any other level...however..there are a few OH-...but they are in massively unequal ratios
2007-10-16 17:47:13 · answer #6 · answered by S D 2 · 0⤊ 0⤋