Advertisements
Advertisements
प्रश्न
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
Advertisements
उत्तर
Given: [OH–] = `2.87 xx 10^-4` M
To find: pH of the solution
Formulae:
i. pOH = –log10[OH–]
ii. pH + pOH = 14
Calculation:
From formula (i),
pOH = –log10[OH–]
∴ pOH = –log10[2.87 × 10–4]
= –log102.87 – log1010–4
∴ –log102.87 + 4 = 4 – 0.4579
pOH = 3.5421
From formula (ii),
pH + pOH = 14
pH = 14 – pOH
= 14 – 3.5421
= 10.4579
pH of the solution is 10.4579
संबंधित प्रश्न
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
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 ________.
Derive the relation pH + pOH = 14.
Which of the following is INCORRECT statement?
Which of the following when dissolved in water results in neutral solution?
The pH of 0.001 M HCl solution is ______.
An aqueous solution of which of the following will have a pH greater than 7?
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
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.
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.
Neutral solutions have the pH of ______.
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?
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
If pH of a solution is 3.12, what would be the concentration of H+ ion?
Define pOH.
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relation pH + pOH = 14.
Define the following term:
pH
