The pH of a 0.1 M MCl (M+ is an unknown cation) was found tobe 4.7. Write a net

Question

The pH of a 0.1 M MCl (M+ is an unknown cation) was found tobe 4.7. Write a net ionic equation for the hydrolysis of M+ and itcorrespoding equilibrium expression Kb. Calculate thevalue of Kb. Please show steps so I can fully understand the problem. Thankyou The pH of a 0.1 M MCl (M+ is an unknown cation) was found tobe 4.7. Write a net ionic equation for the hydrolysis of M+ and itcorrespoding equilibrium expression Kb. Calculate thevalue of Kb. Please show steps so I can fully understand the problem. Thankyou Please show steps so I can fully understand the problem. Thankyou

Explanation / Answer

      M+ +H2O <===> MOH +H+        Because PH = 4.7 ==> [H+] = 2.0 x 10-5M     0.1M                                                                          MCl is 0.1 M ==> [M+] = 0.1M      -x                                            x              x ------------------------------------------ 0.1-x                               x          x          From given,we know [H+] = 2.0 x 10-5 M = x ==> Ka =(2.0 x 10-5 M)2 / (0.1 -2.0 x 10-5M) = 4.0 x 10--9                                                    (comparewith 0.1 , this number is very small and we can ignor) ===> Kb =Kw / Ka = 2.5 x10-6 ===> Kb =Kw / Ka = 2.5 x10-6

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