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
APPEARS IN
RELATED QUESTIONS
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pKa.
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
The CORRECT match between transition metal ion and its colour in aqueous solution.
Aqueous solution of ____________ will turn red litmus blue.
The pH of 0.001 M HCl solution is ______.
Which of the following is CORRECT for an aqueous solution of NH4CN?
[Ka of HCN = 4.0 × 10−10, Kb for NH4OH = 1.8 × 10−5]
A lab assistant prepared a solution by adding a calculated quantity of HCl gas at 25°C to get a solution with [H3O+]= 4 × 10−5 M. Is the solution neutral (or) acidic (or) basic.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
Derive relationship between pH and pOH.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
The mole fraction of the solute molal aqueous solution is:
Derive relationship between pH and pOH.
Define pH.
Derive a relationship between pH and pOH.
Derive the relation pH + pOH = 14.
Define pH.
Define pH.
