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:
0.003 M HCl
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
The CORRECT match between transition metal ion and its colour in aqueous solution.
Which of the following when dissolved in water results in neutral solution?
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.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
Derive relationship between pH and pOH.
The mole fraction of the solute molal aqueous solution is:
Define pOH.
Define pOH.
Derive relationship between pH and pOH.
Derive the relation pH + pOH = 14.
Define pH.
