What pH is needed to produce this value of Q if the concentration and pressure values are. Q= 1.38*10^-26

Br2=2.50*10^-4M
Br-=12.10M
SO4^2-=8.75M
Pso2=1.50*10^-5

You must have an equation (or an expression) and H^+ must be included.

We had to calculate H^+ concentration using Q which was 2.7x10^-27

The concentration I got was 6040M H^+ but if you look at the pH for that it is a negative value...
SO4^2-(aq)+4H^+(aq)+2Br^-(aq) -> Br2(aq)+SO2(g)+2H2O(l)
That is the full balanced equation for the question.

I have the same issuee The H^+ concentration is 3685 on my example, however when i enter -log[H+] I get a negative numbe which isn't the pH :(

Waait, The answer should be a negative number because that just means that the concentration is TOO high! pH is the negative log of the hydrogen ion concentration. Recall that pH can be negative when the hydrogen ion concentration is very high.

So, Since your [H+]= 6040 M
-log[6040]=
-3.78 = pH
:D

Yes it should be negative because i got an negative and it gave me this response. Although negative values are possible for concentrated acids, this is too low to make the reaction practical in a laboratory. Using a more oxidizing acid, such as nitric acid, would be a more efficient way to produce bromine from bromide ions.

To determine the required pH to produce a specific value of Q, we need to know the chemical equation involved and the expression for Q in terms of concentration and partial pressure.

Assuming the reaction involves the formation of products using any of the provided reactants (Br2, Br-, SO4^2-, or Pso2), we need to write the balanced chemical equation first. Without that information, it's difficult to proceed further.

Once you have the balanced chemical equation, you can determine the expression for Q by using the law of mass action, which is typically given by the product of the concentrations (raised to the power of their stoichiometric coefficients) divided by the product of the activities of the reactants (raised to the power of their stoichiometric coefficients).

Q = ([Br-]^n * [SO4^2-]^m) / ([Br2]^x * [Pso2]^y)

Here, the exponents 'n', 'm', 'x', and 'y' correspond to the stoichiometric coefficients of each reactant/product in the balanced chemical equation.

Once you have the expression for Q, you can substitute the given values:
Q = 1.38 * 10^-26
[Br2] = 2.50 * 10^-4 M
[Br-] = 12.10 M
[SO4^2-] = 8.75 M
[Pso2] = 1.50 * 10^-5

Then solve the equation for the pH. Note that pH is related to [H+] concentration according to the equation: pH = -log[H+].

Without the specific chemical equation and the values of the stoichiometric coefficients, it is not possible to determine the required pH to produce the given value of Q.