Advertisements
Advertisements
Question
Calculate the pH and pOH of 0.0001 M HCl solution.
Advertisements
Solution
Given: Concentration of HCl solution = 0.0001 M
To find: pH and pOH
Formulae:
- pH = – log10[H3O+]
- pH + pOH = 14
Calculation: HCl is a strong acid. It dissociates almost completely in water as:
\[\ce{HCl_{ (aq)} + H2O_{ (l)} -> H3O^+_{ (aq)} + Cl^-_{ (aq)}}\]
Hence, [H3O+] = c = 0.0001 M = 1 × 10-4 M
From formula (i),
pH = - log10[H3O+] = - log10[1 × 10-4] = 4
From formula (ii),
pH + pOH = 14
∴ pOH = 14 − pH = 14 – 4 = 10
The pH and pOH of 0.0001 M HCl solution are 4 and 10 respectively.
APPEARS IN
RELATED QUESTIONS
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pKa.
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Which of the following solution will have a pH value equal to 1.0?
Define pH.
Define pOH.
Derive the equation pH + pOH = 14.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
The least basic hydroxide from the following is:
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
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 ______.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Derive relationship between pH and pOH.
Define pOH.
Define pOH.
Define pH.
Define pH.
Derive relationship between pH and pOH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Define pH.
Derive the relation pH + pOH = 14.
Define the following term:
pH
