Advertisements
Advertisements
Question
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Advertisements
Solution
Given: Concentration of sulphuric acid = 0.01 M
To find: pH
Formula: pH = `-"log"_10["H"_3"O"^+]`
Calculation:
Sulphuric acid (H2SO4) is a strong acid. It dissociates almost completely in the water as:
\[\ce{H2SO4_{(aq)} + 2H2O_{(l)} -> 2H3O^+_{ (aq)} + SO^{2-}_{4(aq)}}\]
Hence, [H3O+] = 2 × c = 2 × 0.01 M = 2 × 10-2 M
From formula (i),
pH = -log10[H3O+] = -log10[2 × 10-2] = `-"log"_10"2" - "log"_10"10"^-2`
= `-"log"_10"2" + 2 = 2 - 0.3010`
pH = 1.699
The pH of 0.01 M sulphuric acid is 1.699.
APPEARS IN
RELATED QUESTIONS
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
The pH of 10−8 M of HCl is ______.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Define pOH.
Derive the equation pH + pOH = 14.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
The pH of a monoacidic weak base is 11.5. The concentration of OH− ions in this solution is ____________ M.
An aqueous solution of which of the following will have a pH greater than 7?
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 ____________.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Assertion (A): Increasing order of acidity of hydrogen halides is \[\ce{HF < HCl < HBr < HI}\]
Reason (R): While comparing acids formed by the elements belonging to the same group of periodic table, \[\ce{H - A}\] bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.
Derive the relationship between pH and pOH.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Define pOH.
The mole fraction of the solute molal aqueous solution is:
Derive relationship between pH and pOH.
Derive the relationship between pH and pOH.
Define pOH.
Derive a relationship between pH and pOH.
Derive relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define pOH.
Derive the relation pH + pOH = 14.
Define the following term:
pH
