Advertisements
Advertisements
Question
Derive the equation pH + pOH = 14.
Advertisements
Solution
The ionic product of water is given as:
Kw = [H3O+][OH–]
Now, Kw = 1 × 10–14 at 298 K
Thus, [H3O+][OH–] = 1.0 × 10–14
Taking logarithm of both the sides, we write
log10[H3O+] + log10[OH–] = –14
–log10[H3O+] + {– log10[OH–]} = 14
Now, pH = –log10[H3O+] and pOH = –log10[OH–]
∴ pH + pOH = 14
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:
0.002 M KOH
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
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 ______.
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
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.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Define pOH.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
The pH of a monoacidic weak base is 11.5. The concentration of OH− ions in this solution is ____________ M.
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]
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
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:
Define pOH.
Derive relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pOH.
Define pH.
Define pOH.
