Advertisements
Advertisements
Question
Derive the relationship between pH and pOH.
Advertisements
Solution
The ionic product of water is
KW = \[\ce{[H3O+][OH–]}\]
Now, KW = 1 × 10−14 at 298 K and thus
\[\ce{[H3O+][OH–]}\] = 1 × 10−14
Taking logarithm of both sides,
\[\ce{log10[H3O+] + log10[OH–]}\] = −14
Multiply the entire equation by '−1'
\[\ce{(-log10[H3O+]) + (-log10[OH–])}\] = 14
Now pH = \[\ce{- log10[H3O+]}\] and pOH = \[\ce{- log10[OH–]}\]
∴ pH + pOH = 14
RELATED QUESTIONS
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
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.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
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.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Among the following, the CORRECT increasing order of acidity:
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 least basic hydroxide from the following is:
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
A sample of air turns lime water milky and also turns acidified potassium dichromate green in aqueous solution has low pH. This is due to the presence of pollutants.
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of \[\ce{NH^+_4}\] is 0.20 M. If the equilibrium constant, Kb tor NH3 equals 1.8 × 10-5, what is the pH of the solution?
Define pOH.
Derive relationship between pH and pOH.
Define pH.
Define pOH.
Derive relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define pH.
