Advertisements
Advertisements
Question
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
Solution
\[\ce{HBr + H_2O ↔ H_3O+ + Br-}\]
`["H"_3"O"^+] = ["HBr"]`
`=> ["H"_3"O"^+] = 0.002`
`therefore "pH" = - log ["H"_3"O"^+]`
= - log (0.002)
= 2.69
APPEARS IN
RELATED QUESTIONS
Choose the most correct answer:
Which of the following solution will have a pH value equal to 1.0?
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H⊕ ion concentration.
Derive the relation pH + pOH = 14.
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.
Select the INCORRECT relation.
The pH of 0.001 M HCl solution is ______.
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Neutral solutions have the pH of ______.
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.
Define pOH.
Define pH.
Define pH.
Derive the relation pH + pOH = 14.
Define pH.
Define pOH.
