What is the ph of a 0.0288 m solution of ammonia (kb 1.8 x 10-5)?

10.86

Explanation:

Given that:

Concentration = 0.0288 M

Consider the ICE take for the dissociation of ammonia as:

                                      NH₃    +   H₂O    ⇄     NH₄⁺ +    OH⁻

At t=0                          0.0288                             -              -

At t =equilibrium        (0.0288-x)                         x           x            

The expression for dissociation constant of ammonia is:

x is very small, so (0.0288 - x) ≅ 0.0288

Solving for x, we get:

x = 7.2×10⁻⁴  M

pOH = -log[OH⁻] = -log(7.2×10⁻⁴) = 3.14

Also,

pH + pOH = 14

So, pH = 10.86

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

i think   the answer is c hope i'm right