When referring to percent ionization values given in a acid/base table,
how to determine what is the hydrogen ion concentration of a 0.10 mol/L solution of hydrofluoric acid?
The following answers the question but it doesn't involve percent ionization unless you want to calculate it from the Ka values in the table.
HF ==> H^+ + F^-
Use the ICE table.
Initial concentration
Change in conen and
Equilibrium concn.
Iinitial concn:
(HF) = 0.1 M
(H^+) = 0
(F^-) = 0
Change in concn:
(H^+) = +x
(F^-) = +x
(HF) = -x
Equilibrium concn:
(HF) = 0.1-x
(H^+) = 0 + x = x
(F^-) = 0 + x = x
Write the Ka expression. For HF it is
(H^+)(F^-)/(HF) = Ka.
Look up Ka in your tables, plug in the equilibrium concn from above, and solve for x. That is the (H^+).
To determine the hydrogen ion concentration of a 0.10 mol/L solution of hydrofluoric acid using percent ionization values given in an acid/base table, we need to follow a few steps:
Step 1: Locate the percent ionization value for hydrofluoric acid in the table.
The percent ionization value represents the amount of acid that has dissociated into ions in solution. It is usually given as a percentage.
Step 2: Convert the percent ionization into a decimal.
Divide the given percent by 100 to convert it to a decimal form.
Step 3: Calculate the ionized portion of the acid.
Multiply the initial concentration of the acid (0.10 mol/L) by the decimal value obtained in Step 2. This will give you the concentration of the hydrogen ions that have been ionized.
Step 4: Determine the hydrogen ion concentration.
The concentration of the hydrogen ions is equal to the concentration of the ionized portion of the acid. Therefore, the hydrogen ion concentration is the value obtained in Step 3.
By following these steps, you can determine the hydrogen ion concentration of a 0.10 mol/L solution of hydrofluoric acid using the percent ionization values given in an acid/base table.