Calculate [H3O+] for each of the following solutions.
a)pH = 8.59
i got 3.00e-9 but it said it was wrong. what am i doing wrong. im using the equation 10-ph = [H30+]
nvm i got it thanks anyways:)
wait.. im now stumped on this one
Calculate the pH of each of the following solutions.
[OH - ] = 1.1 10-11 M
Convert OH to pOH, then
pH + pOH = pKw = 14.
[H3O+] = 5.9×10−2 M CALCULATE pH
WHAT IS THE pH
[H3O+] = 5.9×10−2 M
To calculate the concentration of H3O+ (hydronium ions) using pH, you need to reverse the equation you mentioned. Instead of 10 to the power of negative pH, you need to use 10 raised to the power of negative pH to get the concentration of H3O+.
The correct equation is:
[H3O+] = 10^(-pH)
Let's apply this to the given pH of 8.59:
[H3O+] = 10^(-8.59)
[H3O+] = 1.35 x 10^(-9) (rounded to two significant figures)
So the correct value of [H3O+] for a pH of 8.59 is 1.35 x 10^(-9). Your original answer of 3.00 x 10^(-9) was incorrect because you kept the negative sign with pH instead of reversing it to a positive exponent.