Advertisements
Advertisements
प्रश्न
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
Advertisements
उत्तर
For 1mL of 13.6 M HCl diluted with water to give 1 L of solution:
13.6 × 1 mL = M2 × 1000 mL
(Before dilution) (After dilution)
13.6 × 10–3 = M2 × 1L
M2 = 1.36 × 10–2
[H+] = 1.36 × 10–2
pH = – log (1.36 × 10–2)
= (– 0.1335 + 2)
= 1.866 ∼ 1.87
संबंधित प्रश्न
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 ______.
Define pH.
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.
Calculate the pH and pOH of 0.0001 M HCl solution.
Define pOH.
The CORRECT match between transition metal ion and its colour in aqueous solution.
Select the INCORRECT relation.
Among the following, the CORRECT increasing order of acidity:
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
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 ____________.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
The mole fraction of the solute molal aqueous solution is:
Define pOH.
Derive the relation pH + pOH = 14.
Define pH.
Define pOH.
