Advertisements
Advertisements
Question
Calculate the pH of the following solution:
2 g of TlOH dissolved in water to give 2 litre of solution.
Advertisements
Solution
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
RELATED QUESTIONS
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
The pH of 0.001 M NaOH(aq) solution will be:
The CORRECT match between transition metal ion and its colour in aqueous solution.
Select the INCORRECT relation.
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 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 ____________.
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
Derive the relationship between pH and pOH.
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?
Define pH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Which from the following compound in aqueous medium having minimum pH?
