A nitric acid solution is found to have a pH of 2.70. Determine [H3O+],[OH-], and the number of moles of HNO3 required to make 5.50L of the

solution.

a. pH = -log(H^+). Calculate (H^+).

b. (H^+)(OH^-) = Kw = 1E-14. Solve for OH^-.
c. M = moles/L soln.
You have M and L, solve for moles.

To determine [H3O+], [OH-], and the number of moles of HNO3 required to make the solution, we need to use the concept of pH and the dissociation of water.

1. Calculate [H3O+]:
pH is the negative logarithm (base 10) of the concentration of H3O+ ions in a solution. The formula is:
pH = -log[H3O+]

Rearranging the formula to solve for [H3O+]:
[H3O+] = 10^(-pH)

In this case, the pH is 2.70, so:
[H3O+] = 10^(-2.70)

Calculating it, we find the concentration of H3O+ ions in the solution.

2. Calculate [OH-]:
Since water is neutral, the concentration of H3O+ ions and OH- ions are always equal. This means that if we know [H3O+], we can find [OH-].

[OH-] = [H3O+]

Using the value of [H3O+] calculated in step 1, we can determine [OH-].

3. Calculate the number of moles of HNO3:
To calculate the number of moles of HNO3 required to make the solution, we need to use the volume of the solution and the molarity of the nitric acid.

Molarity (M) is defined as moles of solute per liter of solution. The formula is:
M = moles/L

Rearranging the formula to solve for moles:
moles = M x L

Here, we have the volume (5.50 L) of the solution. We need the molarity of HNO3, which is a different value not provided in the question. Once you have the molarity, you can use the formula to calculate the number of moles of HNO3.

By following these steps, you can determine [H3O+], [OH-], and the number of moles of HNO3 required to make the nitric acid solution.