Advertisements
Advertisements
Question
Define pOH.
Advertisements
Solution
The pOH of a solution can be defined as the negative logarithm to the base 10, of the molar concentration of OH− ions in solution.
pOH = -log10[OH-]
RELATED QUESTIONS
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
The solubility of Sr(OH)2 at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
The pH of 10−8 M of HCl is ______.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Answer the following in brief :
The pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Calculate the pH and pOH of 0.0001 M HCl solution.
The pH of a monoacidic weak base is 11.5. The concentration of OH− ions in this solution is ____________ M.
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]
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
The pH of 10−5 M KOH solution will be ____________.
Calculate the pH of 0.04 M HNO3 solution.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
Assertion (A): Increasing order of acidity of hydrogen halides is \[\ce{HF < HCl < HBr < HI}\]
Reason (R): While comparing acids formed by the elements belonging to the same group of periodic table, \[\ce{H - A}\] bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Define pOH.
Define pH.
Define pH.
Define pH.
Define pOH.
Define pH.
