Advertisements
Advertisements
Question
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Advertisements
Solution
\[\ce{H_2O + HCl ↔ H_3O+ + Cl-}\]
Since HCl is completely ionized,
`["H"_3"O"^+] = ["HCl"]`
`=>["H"_3"O"^+] = 0.003`
Now
`"pH" = - log["H"_3"O"^+] = - log(0.003)`
= 2.52
Hence, the pH of the solution is 2.52.
RELATED QUESTIONS
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 solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
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.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Define pOH.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Select the INCORRECT relation.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
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 ____________.
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
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.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Derive relationship between pH and pOH.
Derive the relation pH + pOH = 14.
Define pOH.
Define the following term:
pOH
