Advertisements
Advertisements
प्रश्न
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
Advertisements
उत्तर
For 2g of TlOH dissolved in water to give 2 L of solution:
`["TlOH"_("aq")] = 2/2 "g/L"`
`= 2/2 xx 1/221 "M"`
`= 1/221` M
`"TlOH"_("aq") -> "Tl"_("aq")^+ + "OH"_("aq")^-`
`["TlOH"_("aq")^(-)] = ["TlOH"_("aq")] = 1/221 "M"`
`"K"_"M" = ["H"^+ ]["OH"^-]`
`10^(-14) = ["H"^+] (1/221)`
`221 xx 10^(-14) = ["H"^+]`
`=> "pH" = - log ["H"^+] = - log(221 xx 10^(-14))`
`= - log(2.21 xx 10^(-12))`
= 11.65
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:
0.002 M KOH
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
The pH of 10−8 M of HCl is ______.
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
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.
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
The pH of an aqueous solution is Zero. The solution is ____________.
Derive the relationship between pH and pOH.
Define pH.
Define pOH.
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Define pH.
Define pOH.
