Show the calculation of the ph of a solution obtained by adding 0.0100 mole of h+ to a buffer of ph 9.26 which originally contains 0.100 m nh4cl and 0.100 m nh3. nh3+h2o --> nh4+ + oh- kb= 1.8*10^-5

You have not specified any indication of volume, but I will assume this is in a vessel of 1.00 L.
If 0.0100 mole of H+ is added to this buffer, then in the equilbrium
                    NH3+H2O ⇄ NH4+ + OH-
the H+ reacts with OH- and decreases [OH-] and shifts the equilibrium to the products. [NH4+] will increase by 0.0100 M and [NH3] will decrease by 0.0100M. So the new concentrations are [NH4+] = 0.110 M and [NH3] = 0.09 M. Then
                      [OH-] = [NH3]/[NH4+] * Kb
                                = 0.09/0.110 *1.8*10^-5
                                = 1.47 x 10^-5
and pOH = -log(1.47 x 10^-5) = 4.8318.
Since pH + pOH = 14,
                               pH = 14 - 4.8318 = 9.168
The answer to this question is therefore 9.168.

1. and 2. question: in which equation? or i don't understand you, 3. a), 4. c), 5. c), 6. b), 7. d), 8. d) if small number is underlined(behind symbol) , b) if big number is underlined(in front of symbol)9. what is underlined there? 10. c)