Advertisements
Advertisements
प्रश्न
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
उत्तर
\[\ce{HBr + H_2O ↔ H_3O+ + Br-}\]
`["H"_3"O"^+] = ["HBr"]`
`=> ["H"_3"O"^+] = 0.002`
`therefore "pH" = - log ["H"_3"O"^+]`
= - log (0.002)
= 2.69
APPEARS IN
संबंधित प्रश्न
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Choose the most correct answer:
Which of the following solution will have a pH value equal to 1.0?
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.
Define pOH.
Select the INCORRECT relation.
Which of the following when dissolved in water results in neutral solution?
The least basic hydroxide from the following is:
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
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.
In which of the following solvents is silver chloride most soluble?
Define pH.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Derive a relationship between pH and pOH.
Define pOH.
Define pOH.
Define pH.
Define pOH.
Define the following term:
pH
