If 500 mg of Fe 3 and 50 mg of OH areadded to 1L of pure water, wha...

If 500 mg of Fe3+ and 50 mg of OH- are added to 1L of pure...

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Chemistry

If 500 mg of Fe³⁺ and 50 mg of OH^- areadded to 1L of pure water, what will be the final equilibriumconcentration of Fe³⁺ and OH^-. Assume waterdoes not dissociate.
Fe(OH)₃ => Fe³⁺+3OH^-, pKs=38.57, MW_Fe = 55.85 g/mol, MW_OH = 17.01g/mol

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3.8 Ratings (606 Votes)

Fe3 moles mass of Fe3 in grams Mol weight of Fe3 05 5585 00089526 Oh mole mass Mola mass of OH 005 1701 00029395 OH moles required per Fe3 moles 3 See Answer

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If 500 mg of Fe3+ and 50 mg of OH- are added to 1L of pure...

70.2K

Verified Solution

Question

Chemistry

If 500 mg of Fe³⁺ and 50 mg of OH^- areadded to 1L of pure water, what will be the final equilibriumconcentration of Fe³⁺ and OH^-. Assume waterdoes not dissociate.
Fe(OH)₃ => Fe³⁺+3OH^-, pKs=38.57, MW_Fe = 55.85 g/mol, MW_OH = 17.01g/mol

Answer & Explanation Solved by verified expert

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If 500 mg of Fe3+ and 50 mg of OH- are added to 1L of pure...

70.2K

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Chemistry

If 500 mg of Fe3+ and 50 mg of OH- areadded to 1L of pure water, what will be the final equilibriumconcentration of Fe3+ and OH-. Assume waterdoes not dissociate.Fe(OH)3 => Fe3++3OH-, pKs=38.57, MWFe = 55.85 g/mol, MWOH = 17.01g/mol

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If 500 mg of Fe³⁺ and 50 mg of OH^- areadded to 1L of pure water, what will be the final equilibriumconcentration of Fe³⁺ and OH^-. Assume waterdoes not dissociate.
Fe(OH)₃ => Fe³⁺+3OH^-, pKs=38.57, MW_Fe = 55.85 g/mol, MW_OH = 17.01g/mol