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28 Nov 2019

Calculate the solubility of each of the following compounds in moles per liter and grams per liter. (Ignore any acid-base properties.) (a) Cr(OH)3, Ksp = 6.7 ✕ 10−31 (b) BaCO3, Ksp = 1.6 ✕ 10−9 (c) Hg2Br2, Ksp = 1.3 ✕ 10−22 (Hg22+ is the cation in solution.)

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Hubert Koch
Hubert KochLv2
31 Oct 2019

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Related questions

C) Calculate the pOH at which Cr(OH)3 (s) will begin to precipitate from an aqueous solution that is 1.8 × 10–3 M in Cr3+ (aq) at 25°C. Ksp = 6.3 × 10–31 M4 for Cr(OH)3 (s). Select one: a. 2 × 10–20 M b. 5 × 10–6 M c. 8 × 10–7 M d. 3 × 10–25 M

D) Calculate the solubility of AgCl (s) in moles per liter in 0.20 M NH3 (aq) at 25°C. The two relevant chemical equations are as follows: AgCl (s) Ag+ (aq) + Cl– (aq) Ksp = 1.8 × 10–10 M2 Ag+ (aq) + 2NH3 (aq) [Ag(NH3)2]+ (aq) Kf = 2.0 × 107 M–2 Select one: a. 0.020 M b. 0.20 M c. 0.033 M d. 0.011 M

E) Calculate the solubility of Al(OH)3 (s) in moles per liter in an aqueous solution buffered at pH = 8.50 at 25°C. Ksp = 1.3 × 10–33 M4 for Al(OH)3 (s). Select one: a. 4.1 × 10–17 M b. 6.0 × 10–9 M c. 3.3 × 10–19 M d. 2.6 × 10–9 M

**Answer in Sig Figs**

Calculate the solubility of each of the following compounds inmoles per liter. Ignore any acid-base properties.

(c) PbI2, Ksp = 1.4x10^-8


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