Asoom
May 26, 2009, 01:02 AM
The PH of 0.1M MCl (M^+ is an unknown cation ) was found to be 4.7. Write the ionic equation for the hydrolysis of M^+ and its corresponding equilibrium expression Kb . Calculate the value of Kb
Perito
May 26, 2009, 05:02 AM
The pH of 0.1M MCl (M^+ is an unknown cation ) was found to be 4.7. Write the ionic equation for the hydrolysis of M^+ and its corresponding equilibrium expression Kb . Calculate the value of Kb
Hydrolysis of M+:
M^+ + H_2O \rightleftharpoons MOH + H^+ (Equation 1). The pH is 4.7, so we're in acid solution.
Kb = \frac {[MOH][H^+]}{[M^+]} (Equation 2)
where [] indicates concentration.
pH = 4.7 = -log([H^+]) (Equation 3)
Can you take it from here? You'll have to figure out [MOH] and [M^+] to calculate Kb.