Question

. Like any equilibrium constant, Kw, changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T? Explain with a reaction that includes heat as a reactant or product. (b) In many medical applications, the value of Kw at 37°C (body T) may be more appropriate than the value at 25°C, 1.0x10-14. The pH of pure at 37°C is 6.80. Calculate Kw, pOH and [OH-] at this T.

Answer 1

a

The answer is shown on the first uploaded image

b

`K_(w) = 2.5*10^(-14) J/kgK`

`pOH =6.80`

`[OH^(-)] =1.6*10^(-7) M`

Step-by-step explanation:

The explanation is shown on the second and third uploaded image