The concentration of H2SO4 in a solution is 3.20 10-6 M. Assume the acid dissociates completely in solution.
What is the [H3O+] in the solution?
What is the [OH-] in the solution?
What is the pH of the solution?
What is the pOH of the solution?
OK SO I KNOW HOW TO DO THESE TYPES OF PROBLEMS, BUT I CANT SEEM TO START IT I MEAN, I ASSUEMED THAT THE MOLARITY WOULD = THE H3O+ ION BUT THAT WAS WRONG. HOW CAN I START THIS TO GET THE FIRST PART, THEN I CAN SOLVE IT?
If the sulfuric acid COMPLETELY dissociates, then the hydrogen ion concentration is 2*M (there are two H in H2SO4).
thanks!
To determine the [H3O+] in the solution, you can use the fact that the acid, H2SO4, dissociates completely in solution. This means that one molecule of H2SO4 will produce two H3O+ ions.
Step 1: Identify the relationship between the acid and H3O+ ions. In this case, for every 1 molecule of H2SO4, there will be 2 H3O+ ions.
Step 2: Use the given concentration of H2SO4 to calculate the concentration of H3O+ ions. Since the molarity of H2SO4 is given as 3.20 x 10^(-6) M, it means that for every 1 L of solution, there are 3.20 x 10^(-6) moles of H2SO4.
To calculate the concentration of H3O+ ions, you need to use the mole to mole ratio determined in Step 1. For every 1 mole of H2SO4, you have 2 moles of H3O+ ions. Therefore, the concentration of H3O+ ions would be 2 times the molarity of H2SO4.
[H3O+] = 2 * (3.20 x 10^(-6) M)
To solve this, multiply the molarity of H2SO4 by 2. The resulting value will give you the concentration of H3O+ ions in the solution.
Once you have calculated the concentration of H3O+ ions, you can proceed to determine the [OH-], pH, and pOH of the solution using additional equations.