solve pls The Kb of hydroxylamine NH2OH is 110 Times 108 A b

solve pls

The Kb of hydroxylamine, NH2OH, is 1.10 Times 10-8. A buffer solution is prepared by mixing 120mL of a 0.34M hydroxylamine solution with 60mL of a 0.26M HCL solution. Find the pH of the resulting solution. Express your answer using one decimal place.

Solution

NH2OH(aq) + H2O(l) --> HONH3+(aq) + OH-

moles of NH2OH = 0.12 * 0.34 = 0.0408 = moles of OH-

moles of [H+] = 0.06 * 0.26 = 0.0156

remaining moles of NH2OH = 0.0242

[NH2OH] = 0.0242/0.180 = 0.1344 M

salt prepared = 0.0156 moles HONH3+

[HONH3+] = 0.0156 / 0.180 = 0.0867 M

now,

Kb = [HONH3+][OH-]/ [NH2OH]

1.1x10^-8 = 0.0867 * x / 0.1344

x = 1.7 * 10^-8

pOH = 7.768

pH = 6.232