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
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:
0.003 M HCl
Assuming complete dissociation, calculate the pH of the following solution:
0.005 M NaOH
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 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
The pH of milk, black coffee, tomato juice, lemon juice and egg white are 6.8, 5.0, 4.2, 2.2 and 7.8 respectively. Calculate corresponding hydrogen ion concentration in each.
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.
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 ________.
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Calculate the pOH of 10-8 M of HCl.
Define pOH.
The pH of 0.001 M NaOH(aq) solution will be:
The CORRECT match between transition metal ion and its colour in aqueous solution.
Which of the following when dissolved in water results in neutral solution?
The least basic hydroxide from the following is:
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
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.
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of \[\ce{NH^+_4}\] is 0.20 M. If the equilibrium constant, Kb tor NH3 equals 1.8 × 10-5, what is the pH of the solution?
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Define pOH.
Derive the relationship between pH and pOH.
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Define pH.
