Advertisements
Advertisements
प्रश्न
Define pOH.
Advertisements
उत्तर
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-]
संबंधित प्रश्न
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.
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.
The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
The pH of 10−8 M of HCl is ______.
Which of the following solution will have a pH value equal to 1.0?
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Calculate the pH and pOH of 0.0001 M HCl solution.
Among the following, the CORRECT increasing order of acidity:
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 ____________.
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?
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10−9) is ____________.
Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
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 ____________.
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?
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
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?
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Define pH.
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Derive the relation pH + pOH = 14.
Define pOH.
