Advertisements
Advertisements
प्रश्न
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Advertisements
उत्तर
Given: pH of solution = 6.06
To find: H+ ion concentration
Formula: pH = –log10[H3O+]
Calculation: From the formula,
pH = –log10[H3O+]
∴ log10[H3O+] = –pH
= –6.06
= –6 – 0.06 + 1 – 1
= (–6 – 1) + 1 – 0.06
= –7 + 0.94
= `bar (7).94`
Thus, [H3O+] = Antilog10`[bar (7).94]`
= 8.710 × 10–7 M
The H+ ion concentration of the solution is 8.710 × 10–7 M.
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:
0.005 M NaOH
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre 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 10−8 M of HCl is ______.
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Define pOH.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Among the following, the CORRECT increasing order of acidity:
Aqueous solution of ____________ will turn red litmus blue.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
An aqueous solution of which of the following will have a pH greater than 7?
The least basic hydroxide from the following is:
The number of ions given by Na3[Fe(CN)6] in aqueous solution is ____________.
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
The pH of 10−5 M KOH solution will be ____________.
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.
A sample of air turns lime water milky and also turns acidified potassium dichromate green in aqueous solution has low pH. This is due to the presence of pollutants.
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
Define pOH.
The mole fraction of the solute molal aqueous solution is:
Derive the relationship between pH and pOH.
Define pH.
Define pOH.
