How do you determine concentration levels of hydrogen ions?

Answer 1

You do the inverse.

For example, let's say [H^+] of 0.00100 M is 3. ( it is 3 lol)

You're asking how to make 3 to 0.00100

Put 3 on the calculator, and press the log (inverse)

Answer 2

First, pH relates to concentration of hydrogen ions, and the question asks for HYDROXIDE ion concentration. So, you have to find the pOH (14 - pH), and then the formula is

[concentration OH- (Hydroxide) ions] = 10^-pOH

For example, If I had a pH of 3.0, I would find the pOH (14-3.0=11 pOH) and then plug it in to the formula. So,

[OH-] = 10^-11, or 0000000000.1 (1.0 x 10^-11)

Answer 3

Using this formula Kw=[H3O+]x[OH-]=10^-14.

Find the Conc. of [H3O+]

then use the next formula pH=-log10[H3O].

E.g. [OH-]=4M.

[H3O]x[4]=10^-14.

[H3O]=2.5x10^-15.

so, pH of (OH)= -log10(2.5x10^-15)

= 14.6 DONE ^_^

Answer 4

The pH is the negative of the logarithm (to the base 10) of the activity of hydrogen ions.

So pH = -log(activity of H+)

For example, if the activity of H+ was 0.0000001 mol per litre (as it would be in pure water at 25 0C), this is equal to 10^(-7) mol per litre.

the log of 10^(-7) is -7

and the -log of 10^(-7) is 7

so the pH is 7

Answer 5

the pH is the negative exponent of moles per liter. for instance a pH of 9 would be 10 to the -9 moles per liter, pH of 6 would be 10^-6 mols per liter, etc.

Answer 6

10^-pH will give you the hydronium ion concentration

Answer 7

pH = -log[H3O+] so take the antilog of the pH

Example:

When pH = 5.0 then [H3O+] = 10-pH = 10-(5.0) = 1.0*10-5 mol/L

Answer 8

1.0 X 10 - 14

Is the concentration, Molarity.

- log(1.0 X 10 -14 M)

= 14 pH

========which means that H + concentration is nil.

Answer 9

Roughly but very cheap this can be done by pH-indicator paperstrips, more precize by using a laboratory pH meter.