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311.

Calculate the solubility of lead iodide in water at 298 K. (K_sp of PbI₂ = 7·1×10^–9).

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312. Calculate the concentration of Mg²⁺ ions and OH^- ions in a saturated solution of Mg(OH)₂, solubility product of Mg(OH)₂ is 9×10^–12

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313.

Determine the solubility of silver chromate at 298K. Given that K_sp for Ag₂CrO₄= 1·1 × 10^–12. Also determine the molarities of each ion.

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314. Determine the solubility of barium chromate at 298K. Given K for BaCrO₄ = 1·2 × 10^–10. Also, determine the molarities of each ion.

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315. Determine the solubility of ferric hydroxide at 298K. Given K_sp for Fe(OH)₃ = 1·0 × 10^–38. Also, determine the molarities of each ion.

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316. Determine the solubility of lead chloride at 298K. Given K_sp for PbCl₂ = 1·6 × 10^–5. Also, determine the molarity of each ion.

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Molar mass of Sr(OH)₂ = 87·6 + 32 + 2 = 121·6

The solubility equilibrium is

i.e. 1 mole of

in the solution gives 1 mole of

Hence in the solution,

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318. The solubility product of BaSO₄ is 1·5 × 10^–9. Find solubility in:
(i) pure water
(ii) 0·10 M BaCl₂.

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319.

How many moles of AgBr (K_sp = 5 × 10^–13 mol² L^–2) will dissolve in a 0·01 M NaBr solution (NaBr is completely dissociated into Na⁺ and Br^-ion).

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320. What is the minimum volume of water required to dissolve lg of calcium sulphate at 298 K? [For calcium sulphate, K_sp is 9·1 × 10^–6).

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