HARD
JEE Main/Advance
IMPORTANT
Earn 100

The solubility of CaCO3 is  7 mg/litre. Calculate the solubility of BaCO3 (in mol/L) from this information and from the fact that when Na2CO3 is added slowly to a solution containing equimolar concentration of Ca+2 and Ba+2, no precipitate of CaCO3 is formed until 90% of Ba+2 has been precipitated as BaCO3. (Assume no hydrolysis of CO32- ion)

50% studentsanswered this correctly

Important Questions on Equilibrium

HARD
JEE Main/Advance
IMPORTANT
To a solution formed by adding n mole of sparingly soluble salt MX in 1 L water, NaY solid (a readily soluble salt) is added until x% of MX is converted to MY(s) (another sparingly soluble salt). Then: (Assume no hydrolysis of any ion).
HARD
JEE Main/Advance
IMPORTANT

What maximum pH must be maintained in a saturated H2S solution (0.1 M) to avoid precipitation of both Mn2+ and Fe2+ from a solution, in which each ion is present at a concentration of 0.01 M?

Kaof H2S=9.6×10-21; Ksp of MnS=2.5×10-13; Ksp ofFeS=6.4×10-18

HARD
JEE Main/Advance
IMPORTANT

What minimum pH must be maintained in a saturated H2S solution (0.1 M) to avoid precipitation of both Mn2+ and Fe2+ from a solution, in which each ion is present at a concentration of 0.01 M?

Kaof H2S=9.6×10-21; Ksp of MnS=2.5×10-13; Ksp ofFeS=6.4×10-18

HARD
JEE Main/Advance
IMPORTANT
A decimolar solution of HCl is saturated with H2S gas. Calculate the minimum Cu2+ ion that will saturate the above solution with CuS. Given Ksp of CuS=6.4×10-36, Ka for H2S=9.6×10-21 and solubility of H2S=0.1 mole litre-1.
HARD
JEE Main/Advance
IMPORTANT
0.98 g H3PO4 is dissolved in 100 mL a buffer solution (pH=5). If the equilibrium concentrations of H2PO4-,HPO42-,PO43- and H3PO4 are C1,C2,C3 and C4 respectively. Find pC1+pC2+pC3+pC4pCi=-logCi; where i=1,2,3,4) Given: For H3PO4, Ka1=10-3, Ka2=10-8, Ka9=10-12.
HARD
JEE Main/Advance
IMPORTANT
On addition to V mL volume of 0.1M KOH, buffer capacity is found maximum at pHsolution =x>7 when it is titrated against 50 mL,0.2 M H2CO3. For H2CO3:Ka1=4.3×10-6,Ka2=5.6×10-11
Report your answer as (V+x)×0.4, rounding it off to the nearest whole number.
HARD
JEE Main/Advance
IMPORTANT

The solubility product of Ag2C2O4 at 25° C is 1.29×10-11mol3L-3. A solution of K2C2O4 containing
0.152 mole in 500 mL water.is shaken with an excess of Ag2CO3 till the following equilibrium is reached:

Ag2CO3(s)+K2C2O4(aq)Ag2C2O4(s)+K2CO3(aq).

At equilibrium, the solution contains 0.0358 mole of K2CO3. Assuming the degree of dissociation of K2C2O4 and K2CO3 to be equal, if the solubility product of Ag2CO3 is 3.794×10-x mol3L-3, find x.

HARD
JEE Main/Advance
IMPORTANT
0.1 millimole of CdSO4 are present in 10 mL acid solution of 0.08 M HCI. Now H2S is passed to precipitate all the Cd2+ ions. Find the pOH of the solution after filtering off precipitate, boiling off H2S and making the solution 100 mL by adding H2O.