Advertisements
Advertisements
Question
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Advertisements
Solution
\[\ce{KOH_{(aq)} ↔ K^+_{(aq)} + OH^-_{(aq)}}\]
`["OH"^-] =["KOH"]`
`=> ["OH"^-] = .002`
Now `"pOH" = - log["OH"^-]`
= 2.69
`therefore pH = 14 - 2.69`
= 11.31
Hence, the pH of the solution is 11.31
RELATED QUESTIONS
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
The pH of 10−8 M of HCl is ______.
Which of the following solution will have a pH value equal to 1.0?
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Which of the following is INCORRECT statement?
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
Which of the following when dissolved in water results in neutral solution?
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
Neutral solutions have the pH of ______.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Derive relationship between pH and pOH.
Derive the relationship between pH and pOH.
Derive a relationship between pH and pOH.
Define pOH.
Derive relationship between pH and pOH.
Define pH.
Define pH.
Define pH.
Define pOH.
