calculate [H^+] and the pH of 0.025M of HNO3

To calculate [H+] and pH of a solution of HNO3, we need to consider the dissociation of HNO3 in water.

The balanced chemical equation for the dissociation of HNO3 is:

HNO3(aq) -> H+(aq) + NO3-(aq)

Given that the concentration of HNO3 is 0.025 M, and assuming complete dissociation, the concentration of H+ is also 0.025 M.

[H+] = 0.025 M

The pH of a solution can be calculated using the equation:

pH = -log[H+]

Substituting the value of [H+] into the equation:

pH = -log(0.025)

Using a calculator, we can calculate the pH:

pH ≈ 1.60

Therefore, the [H+] is 0.025 M and the pH is approximately 1.60.

To calculate the [H^+] concentration and the pH of a solution of HNO3, you need to know the dissociation equation of HNO3, as well as the dissociation constant.

The dissociation equation for HNO3 is:
HNO3 -> H+ + NO3-

The dissociation constant for HNO3 is not given, but we can assume the complete dissociation of HNO3 since it is a strong acid.

Since the concentration of HNO3 is given as 0.025M, we can assume that the concentration of [H+] is also 0.025M because the dissociation is complete.

To calculate the pH, we use the formula:
pH = -log[H+]

Using the concentration of [H+] as 0.025M, we can plug it into the formula:
pH = -log(0.025)

Using a scientific calculator, find the logarithm of 0.025, and then change the sign to negative to get the pH.

The answer will be the negative logarithm of 0.025, which is approximately 1.602.

Therefore, the [H+] concentration is 0.025M, and the pH is approximately 1.602.

HNO3 is a strong acid.

pH=-log[0.025M]

I will let you guess what the H+ concentration is.