Home
Class 12
CHEMISTRY
If K("sp") of calcium iodate Ca(IO(3))(...

If `K_("sp") ` of calcium iodate `Ca(IO_(3))_(2) = 6.3 xx 10^(-7) " at " 18^(@)C`, find the solubility of salt (in gm/L) in water at `18^(@) C` .

Text Solution

AI Generated Solution

To find the solubility of calcium iodate \( \text{Ca(IO}_3\text{)}_2 \) in water at \( 18^\circ C \) given that the solubility product constant \( K_{sp} = 6.3 \times 10^{-7} \), we can follow these steps: ### Step 1: Write the dissociation equation Calcium iodate dissociates in water as follows: \[ \text{Ca(IO}_3\text{)}_2 (s) \rightleftharpoons \text{Ca}^{2+} (aq) + 2 \text{IO}_3^{-} (aq) \] ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 17|1 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 18|1 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 15|1 Videos

  • INTRODUCTION TO ORGANIC CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE ADVANCED ARCHIVE|81 Videos

  • JEE MAIN - 5

    VMC MODULES ENGLISH|Exercise PART II : CHEMISTRY (SECTION - 2)|5 Videos

Similar Questions

Explore conceptually related problems

The K_(sp) of AgC1 at 25^(@)C is 1.6 xx 10^(-9) , find the solubility of salt in gL^(-1) in water.

K_(sp) for lead iodate [Pb(IO_(3))_(2) is 3.2 xx 10^(-14) at a given temperature. The solubility in molL^(-1) will be

The solubility product of barium sulphate is 1.5 xx 10^(-9) at 18^(@)C . Its solubility in water at 18^(@)C is

If the solubility product K_("sp") of a sparingly soluble salt MX_(2)" at "25^(@) C " is " 1.0 xx 10^(-11) , then the solubility of the salt in mole "litre"^(-1) at this temperature will be

The K_(SP) for Cr(OH)_(3) is 1.6xx10^(-30) . The molar solubility of this compound in water is

The K_(SP) for Cr(OH)_(3) is 1.6xx10^(-30) . The molar solubility of this compound in water is

K_(sp) of PbBr_(2) is 8 xx 10^(-5) . If the salt is 80% dissociated in solution, calculate the solubility of salt in gL^(-1) .

If K_(sp) for HgSO_(4) is 6.4xx10^(-5) , then solubility of this substance in mole per m^(3) is

K_(sp) of AgCl is 2.8 xx 10^(-10) at 25^(@)C . Calculate solubility of AgCl in. a. Pure water b. 0.1M AgNO_(3) c. 0.1M KCl or 0.1M NaCl

At 25^(@) C, the solubility product of Hg_(2)CI_(2) in water is 3.2xx10^(-17)mol^(3)dm^(-9) what is the solubility of Hg_(2)CI_(2) in water at 25^(@) C ?

Home
Profile