Typically the concentration of hydronium, H3O, or hydroxide. OH , ions in an aqu
ID: 809935 • Letter: T
Question
Typically the concentration of hydronium, H3O, or hydroxide. OH , ions in an aqueous solution is less than 1 M. It is not uncommon to have hydronium ion concentrations that are much smaller. such as 2.60 x 10^-5 pH, therefore. is a convenient way to restate the hydronium concentration. pH is equal to the negative log of a hydronium ion concentration in solution: Access the pH calculation simulation. which will open in a new window. Edit the concentration by typing a value between 1.0 x 10^-7 and 1.8 x 10^1 into the space provided. Select a compound from the dropdown menu and click Dip. The pH value will display in the History field. You need Adobe Shockwave Player to run this simulation. Correct The basicity of amine depends on the electron-releasing ability of the amine, the crowding around the amine, and the ability of the amine to form hydrogen bonds. An amine must remove a hydrogen atom from water to form hydroxide ions and create a basic solution. Although trimethylamine has a more basic character than the other amines, the three bulky substituents make it a weaker base since a hydrogen atom has trouble accessing the nitrogen atom and forming the positive ion. Part C Use the data in the simulation to find the Ka value of HF. hydrofluoric acid. Express your answer to two significant figures.Explanation / Answer
I am not able to identify the data of simulation
however
If pH = 2.60
[H+] = 10^-2.60 = 2.51 X 10^-3 = [F-]
[HF] = 0.08 - 2.51 X 10^-3 = 0.0775
Ka = (2.51X10^-3)^2 / 0.0775 = 8.13 X 10^-5
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