Home
Class 12
CHEMISTRY
The dissociation constants of H(2)O, H(2...

The dissociation constants of `H_(2)O, H_(2)S, H_(2)Se` are `1.8xx10^(-6),1.4xx10^(-16), 1.3xx10^(-7) and 2.2xx10^(-5)`, respectively. What do these values denote? 

Text Solution

Verified by Experts

Dissociation of hydride is given as,
`H_(2)MhArrH^(+)+MH^(-)`
  For this dissociation equilibrium, a lower value of `K_(a)` denotes that the acid is weak.
As the `K_(a)` values increase from `H_(2)O` to `H_(2)Te`, their acidic strength also increases. `H_(2)Te` is retalively a stronger acid.
Promotional Banner

Topper's Solved these Questions

  • VIA GROUP ELEMENTS

    AAKASH SERIES|Exercise SUBJECTIVE EXERCISE - 1(LONG ANSWER QUESTIONS)|1 Videos

  • VIA GROUP ELEMENTS

    AAKASH SERIES|Exercise SUBJECTIVE EXERCISE - 1(SHORT ANSWER QUESTIONS)|5 Videos

  • VA GROUP ELEMENTS

    AAKASH SERIES|Exercise PRACTICE EXERCISE|51 Videos

  • VII GROUP ELEMENTS

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE -4|55 Videos

Similar Questions

Explore conceptually related problems

The dissociation coustant of H_(2)O, H _(2)Se and H_(2) Te are 1.8 xx 10 ^(-16) , 1.4 xx 10 ^(-7) , 1.3 xx 10 ^(-4)and 2.2 xx 10 ^(-3), respectively. What do these values denote ?

The ionization constants of HF, H COOH and HCN at 298 K are 6.8x10^(-4), 1.8xx10^(-4) and 4.7xx10^(-9) respectively. Calculate the ionization constants of the corresponding conjugate base.

For the formation of NH_(3) from N_(2) and H_(2) at 500 K, the concentration of N_(2), H_(2) and NH_(3) at equilibrium are 1. 5xx10^(-2) M and 1.2xx10^(-2)M, respectively. The equilibrium constant for the reverse reaction is

For the formation of NH_3 from H_2 at 500 K, The concentration of N_2, H_2 and NH_3 at equilibrium are 1.5xx10^(-2) M , 3.0 x 10^(-2) M and 1.2 xx 10^(-2) M , respectively. The equilibrium constant for the reverse reaction is

The first and second dissociation constants of an acid H_(2)A are 10^(-5) and 5 xx 10^(-10) respectively . Then overall dissociation constant of the acid is

The Ksp values of MA , MB , MC , MD are 1.8 xx 10^(-10) , 4 xx 10^(-3) , 4 xx 10^(-8) & 6 xx 10^(-5) respectively . If a 0.01 M solution of MX is added dropwise to a mixture containing A , B , C , D solution the one to be precipitated first will be :

Dissociation constants of CH_3 COOH and NH_4 OH are respectively 1.8 xx 10^(-5) and 2 xx 10^(-5) . What is the nature of aqueous ammonium acetate solution ? Explain.

The equilibrium constants of a reaction at 27^(@)C and aet 127^(@)C are 1.6xx10^(-3) and 7.6xx10^(-2) respectively. Is the reaction exothermic or endothermic?