Question

04 Question (1 point) @ See page 729 A buffer solution inckudes a weak acid and its conjugate base. 4th attempt Feedback del See Periodic Table ’See Hint Include states of matter. Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH3 and NHACI. Write the equation so that its equilibrium constant is equivalent to Ka NH;(aq) + H2O(1) _ NII;(aq) +OH"(aq) 3rd attemnt 04/18 TRY AGAIN VIEW SOLUTION C 14 OF 18 QUESTIONS COMPLETED

Answer 1

I think we can not have equilibrium constant to Ka here. some kind of typo is there or information is missing here.

This buffer is made by adding salt of weak base to it.

thus,

$NH^{_{3(aq)}} + H2O \rightleftharpoons NH^{4+} + OH^{-}$

base         huge    excess limited quantity of OH-

               excess

NH4+ is excess from above reaction as well as from NH4Cl.

now NH4+ is WEAKLY acidic and if you consider Ka here, it will be

$NH4+ \leftrightharpoons NH3 + H^{^{+}}$

So, there is no way to see K = Ka correlation here.