Advertisements
Advertisements
प्रश्न
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
Advertisements
उत्तर
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
संबंधित प्रश्न
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Which of the following is INCORRECT statement?
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
The pH of 0.001 M NaOH(aq) solution will be:
The CORRECT match between transition metal ion and its colour in aqueous solution.
The pH of a monoacidic weak base is 11.5. The concentration of OH− ions in this solution is ____________ M.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
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 ____________.
The pH of an aqueous solution is Zero. The solution is ____________.
A lab assistant prepared a solution by adding a calculated quantity of HCl gas at 25°C to get a solution with [H3O+]= 4 × 10−5 M. Is the solution neutral (or) acidic (or) basic.
Calculate the pH of 0.04 M HNO3 solution.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
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?
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.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Define pH.
Derive relationship between pH and pOH.
Define pH.
Define pH.
Derive the relation pH + pOH = 14.
Define the following term:
pOH
