If the pH of a solution is 6, what are the hydrogen- and hydroxide-ion concentrations?
The PH of a 0.1 M MCl (M+ is an unknown cation) was found to be 4.7. Write the net ionic equation for the hydrolysis of M+ and its corresponding equilibrium expression Kb. Calculate the value of Kb.
Please Help!!!!!
To find the hydrogen-ion concentration (H+) and hydroxide-ion concentration (OH-) in a solution with a pH of 6, we can use the pH formula:
pH = -log10[H+]
pH is given as 6, so:
6 = -log10[H+]
Rearranging the equation:
[H+] = 10^(-pH)
[H+] = 10^(-6)
Therefore, the hydrogen-ion concentration in the solution is 10^(-6) M.
Since the solution is neutral, the hydroxide-ion concentration will also be 10^(-6) M.
Now, let's move on to the second part of your question.
The net ionic equation for the hydrolysis of M+ can be written as:
M+ (aq) + H2O (l) -> MOH (aq) + H+ (aq)
The equilibrium expression Kb can be written as:
Kb = [MOH] [H+] / [M+]
The concentration of MOH can be assumed to be equal to [OH-], which is equivalent to [H+] since the solution is neutral.
Therefore, the equilibrium expression can be simplified to:
Kb = [H+]^2 / [M+]
Since [H+] is 10^(-6) M, the value of Kb can be calculated by plugging in this value. However, the concentration of M+ is missing from the information you provided, so it is not possible to calculate the value of Kb without that information.
Please provide the concentration of M+ in the solution to proceed with the calculation.