`0.200g` of iodine is stirred in `100mL` of water at `298K` till equilibrium is reached:
`[I_2(aq.)]_("Equilibrium")=0.0011 mol L^(-1)` at `298K`
What will be the mass of iodine found in solution?

The solubility of iodine in water is 1.1 xx 10^(-3) "mol L"^(-1) at 288 K. When 0.200 g of iodine is stirred in 100 of water till equilibrium is reached, what will be the mass of iodine found in solution and the mass that is left undissolved. After equilibrium is reached with 0.200 g of iodine and 100 of water, we add 150 of water to the system. How much iodine will be dissolved and how much will be left undissolved and what will be the concentration of iodine in solution ?

100 g of NaCl is stirred in 100 mL of water at 20^(@)C till the equilibrium is attained: ( a ) How much NaCl goes into the solution and how much of it is left undissolved at equilibrium? The solubility of NaCl at 20^(@)C is 6.15 mol//litre . ( b ) What will be the amount of NaCl left undissolved, if the solution is diluted to 200 mL ?

Solubility of iodine of water is 1.1 times 10^-3 mol L^-1 at 290K. When 0.1g of iodine is stirred in 200ml water till the equilibrium is reached at 290K, calculate the mass of undissolved iodine.

For a reversible reactionn at 298 K the equilibrium constant K is 200. What is value of DeltaG^(@) at 298 K ?

For a reversible reaction at 298 K the equilibrium constant K is 200. What is value of DeltaG^(@) at 298 K ?

The solubility of Sb_(2)S_(3) in water is 1.0 xx 10^(-5) mol/letre at 298K. What will be its solubility product ?

The solubility of Sb_(2)S_(3) in water is 1.0 xx 10^(-5) mol/letre at 298K. What will be its solubility product ?

The dissociation of N_(2)O_(4) to NO_(2) was carried out at 298 K in chloroform medium. When equilibrium was reached, 0.2 mol of N_(2)O_(4) and 0.02 mol of NO_(2) were found to be present in a 2L solution. The K_(c) of the reaction at this temperature is

A solution of sucrose (molecular mass 342 u) is prepared by dissolving 0.84 g in 100g of water at 298K. Calculate the boiling point of water in the solution (K_b for water = 0.52 K kg mol^-1)