Home
Class 12
CHEMISTRY
A solution contains 0.1MH(2)S and 0.3MHC...

A solution contains `0.1MH_(2)S` and `0.3MHCl` .Calculate the conc.of `S^(2-)` and `HS^(-)` ions is solutions.Given `K_(a_(1))` and `K_(a_(2))` are `10^(-7)`and `1.3xx10^(-13)` respectively.

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the concentrations of the sulfide ion \( S^{2-} \) and the bisulfide ion \( HS^{-} \) in a solution containing \( 0.1 \, M \, H_2S \) and \( 0.3 \, M \, HCl \). Given the dissociation constants \( K_{a1} \) and \( K_{a2} \) for \( H_2S \) are \( 10^{-7} \) and \( 1.3 \times 10^{-13} \) respectively, we can follow these steps: ### Step 1: Determine the concentration of \( H^+ \) ions Since \( HCl \) is a strong acid, it will completely dissociate in solution: \[ [H^+] = [HCl] = 0.3 \, M \] ...
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Board Level Exercise|27 Videos

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Exercise -1|28 Videos

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise partIII one or more than one options correct type|10 Videos

  • HYDROCARBON

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Hydrocarbon)|50 Videos

  • IUPAC NOMENCLATURE & STRUCTURAL ISOMERISM

    RESONANCE ENGLISH|Exercise Advanced Level Problems Part-5|2 Videos

Similar Questions

Explore conceptually related problems

A solution contains 0.10 M H_2S and 0.3 HCl Calculate the concentration of S^(2-) and HS^(-) ions in the solution . For H_2S , K_(a_1) = 1 xx 10^(-7) and K_(a_2) = 1.3 xx 10^(-13)

If K_(a_(1))gtK_(a_(2)) of H_(2)SO_(4) are 10^(-2) and 10^(-6) respectively then:

Approximate p.H,0.1M aqueous H_(2)S solution when K_(1) and K_(2) for H_(2)S at 25^(@)C are 1xx10^(-7) and 1.3xx10^(-13) respectively:-

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. K_(b) =2xx10^(-5) .

10mL of 0.3M Na_(2)SO_(4) are mixed with 20mL solution having initially 0.1M Ca^(2+) and 0.1M Sr^(2+) in it. Calculate the final [Ca^(2+)], [Sr^(2+)] and [SO_(4)^(2-)] in solution? Given K_(sp) SrSO_(4) = 7.6 xx 10^(-7) and K_(sp) CaSO_(4) = 2.4 xx 10^(-5) .

An aqueous solution contains 0.10 M H_(2)S and 0.20 M HCl. If the equilibrium constants for the formation of HS^(–) from H_(2)S is 1.0xx10^(–7) and that of S^(2-) from HS^(–) ions is 1.2xx10^(–13) then the concentration of S^(2-) ions in aqueous solution is

For a 0.072 M NaSO_(4) solution,select the correct option(s): (K_(a_(1)) and K_(a_(2)) of H_(2)SO_(4)=oo & 1.2xx10^(-2))

Calculate solubility of MnS in a buffer solution of given pH.K_(sp) of MnS and K_(a_(1))&K_(a_(2)) for H_(2)S are given .

A solution contains 0.09 HC1, 0.09 M CHC1_(2)COOH , and 0.1M CH_(3)COOH . The pH of this solution is one. Calculate K_(a) for CHC1_(2)COOH . (Given K_(a)CH_(3)COOH = 10^(-5))

Determine the concentration of NH_(3) solution whose one litre can dissolve 0.10 mole AgCl. K_(sp) of AgCl and K_(f) of Ag(NH_(3))_(2)^(+) are 1.0xx10^(-10)M^(2) and 1.6xx10^(7)M^(-2) respectively.