Calculate the pH of a 0.2 M * 4 solution for which Kb = 1.8*10^-5 at 26 c . The equation for the reaction Nh3+H2O->NH4+oh

The pH of the solution is 11.24

Explanation:

We are given:

Molarity of ammonia = 0.2 M

The given chemical equation follows:

I:                0.2

C:               -x                      +x        +x

E:             0.2-x                     x          x

The expression for equilibrium constant follows:

Putting values in above expression, we get:

Neglecting the negative value of x as concentration cannot be negative.

So,

pOH is defined as the negative logarithm of hydroxide ion concentration present in the solution.

Putting values in above equation, we get:

We know:

Hence, the pH of the solution is 11.24

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.

answer; 4 electrons;