Question

What is the concentration in M) of hydroxide ions in a solution at 25°C with pH 4.1537 (A) 4.15 (B) 9.85 (C) 1.42-100 (D) 7.03*10" (E) none of the above

Answer 1

The correct answer is option 'E': None of the above.

Step-by-step explanation:

Given that pH of the solution is 4.1537

From the basic relation of acids and bases we know that

`pH+pOH=14\\\\\therefore pOH=14-pH\\\\pOH=14-4.1537\\\\\therefore pOH=9.8463`

From the definition of pOH we have

`pOH=-log[OH^(-)]`

where

[OH] is the concentration of hydroxide ions in moles/Liter (M)

Applying values and subsequently solving we get

`9.8463=-log[OH^(-)]\\\\\therefore [OH^(-)]=antilog(-9.8463)\\\\\therefore [OH^(-)]=10^(-9.8463)M`

`\therefore [OH^(-)]=14.246* 10^(-11)}M`