Home
Class 12
CHEMISTRY
The solubility product of SrF(2) in wate...

The solubility product of `SrF_(2)` in water is `8xx10^(-10)`. Calculate its solubility in `0.1M` NaF aqueous solution.

Text Solution

AI Generated Solution

To calculate the solubility of `SrF2` in a `0.1 M` NaF aqueous solution, we will follow these steps: ### Step 1: Write the dissociation equation for `SrF2` `SrF2` dissociates in water according to the following reaction: \[ \text{SrF}_2 (s) \rightleftharpoons \text{Sr}^{2+} (aq) + 2 \text{F}^- (aq) \] ### Step 2: Define the solubility product (Ksp) The solubility product \( K_{sp} \) for the dissociation of `SrF2` can be expressed as: ...
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

The solubility product of SrF_(2) in water is 8 xx 10^(-10) Calculate its solubility in 0.1 M of aqueous NaF solution. If its solubility is expressed as y xx 10^(-8) then what is the value of 'y' ?

The solubility product of MgF_(2) is 7.4xx10^(-11) . Calculate the solubility of MgF_(2) in 0.1 M NaF solution

The solubility of Pb(OH)_(2) in water is 6.7xx10^(-6) M. Calculate the solubility of Pb(OH)_(2) in a buffer solution of pH=8 .

The solubility of Pb(OH)_(2) in water is 6.7xx10^(-6) M. Calculate the solubility of Pb(OH)_(2) in a buffer solution of pH=8 .

The solubility of Pb(OH)_(2) in water is 6.7xx10^(-6) M. Calculate the solubility of Pb(OH)_(2) in a buffer solution of pH=8 .

The solubility of Pb(OH)_(2) in water is 6.7xx10^(-6) M. Calculate the solubility of Pb(OH)_(2) in a buffer solution of pH=8 .

The solubility product of BaCl_(2) is 3.2xx10^(-9) . What will be solubility in mol L^(-1)

Solubility of Cd(OH)_(2) in pure water is 1.84xx10^(-5)"mole"//L Calculate its solubility in a buffer solution of pH=12 .

The solubility product of Ni(OH)_(2) is 2.0xx10^(-15) . The molar solubility of Ni(OH)_(2) in 0.1 M NaOH solution is

The solubility product of PbCl_(2) at 298K is 1.7 xx 10^(-5) . Calculate the solubility of PbCl_(2) in g L^(-1) at 298K