Home
Class 12
CHEMISTRY
Determine the solubilities of silver chr...

Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298 K form their solubility product constants given below. Determine also the molarities of individual ions.
`K_(SP(Ag_(2)CrO_(4)))=1.1xx10^(-12)`,
`K_(SP(BaCrO_(4)))=1.2xx10^(-10)`,
`K_(SP[Fe(OH)_(3)])=1.0xx10^(-38)`,
`K_(SP(PbCI_(2)))=1.6xx10^(-5)`,
`K_(SP(Hg_(2)I_(2)))=4.5xx10^(-29)`.

Text Solution

AI Generated Solution

To determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride, and mercurous iodide at 298 K from their solubility product constants (Ksp), we will follow these steps for each compound: ### 1. Silver Chromate (Ag2CrO4) - **Dissociation Equation**: \[ \text{Ag}_2\text{CrO}_4 \rightleftharpoons 2 \text{Ag}^+ + \text{CrO}_4^{2-} \] - **Let the solubility be \( S \)**: ...
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise LEVEL 1|75 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise LEVEL 2|50 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

Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298K from theor solubility product constants given in Table 7.9 . Determine also the molarities of individual ions.

Determine the solubility of silver chromate at 298 K given its K_(sp) value is 1.1xx10^(-12) ?

What is the molar solubility of AgCl(s) in 0.1 M NH_(3)(aq)?K_(sp)(AgCl)=1.8xx10^(-10), K_(f)[Ag(NH_(3))_(2)]^(+)=1.6xx10^(7).

Calculate the solubility og AgCN in a buffer solution of pH 3.00 K_(sp(AgCN)) = 1.2 xx10^(-18) and K_(a(HCN)) = 4.8 xx 10^(10) M^(2) .

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )

Freshly prepared aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing 0.25M of ammonium chloride and 0.05M of ammonium hydroxide. Calculate the concentration of aluminium and magesium ions in solution (K_(b) NH_(4)OH = 1.8 xx 10^(-5), K_(sp) Mg(OH)_(2) = 6 xx 10^(-10), K_(sp) Al(OH)_(3) = 6 xx 10^(-32) .

What is the molar solubility of Ag_(2)CO_(3)(K_(sp)=4xx10^(-13)) in 0.1M Na_(2)CO_(3) solution ?

The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))

What is the molarity of F^(-) ions in a saturated solution of BaF_(2) ? (K_(sp)=1.0xx10^(-6))

What is the molarity of Fe(CN)_(6)^(4-) in a saturated solution of Ag_(4)[Fe(CN)_(6)] ? (K_(sp)=1.6xx10^(-41))