Advertisements
Advertisements
प्रश्न
Derive the relation pH + pOH = 14.
Derive the relationship between pH and pOH.
उत्तर
Relationship between pH and pOH:
The ionic product of water is given as:
Kw = [H3O+][OH–]
Now, Kw = 1 × 10−14 at 298 K
Thus, [H3O+][OH-] = 1 × 10−14
Taking the 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
संबंधित प्रश्न
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
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 0.2M Ca(OH)2 + 25 mL of 0.1M HCl.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Calculate the pH and pOH of 0.0001 M HCl solution.
Which of the following is INCORRECT statement?
An aqueous solution of which of the following will have a pH greater than 7?
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]
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
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 an aqueous solution is Zero. The solution is ____________.
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.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
Derive the relationship between pH and pOH.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Define pOH.
Define pOH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Derive the relation pH + pOH = 14.
