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At 298 K, calculate the solubility of metal sulfide, MS(s), in a saturated solution of H2S where the concentration of H2S and pH are maintained at 0.1 M and 3.0, respectively Given at 298 K,K = 10–7K = 5 × 10–19Correct answer is 'Therefore, solubility of metal sulphide = 5 × 10–14 M.'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared
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At 298 K, calculate the solubility of metal sulfide, MS(s), in a saturated solution of H2S where the concentration of H2S and pH are maintained at 0.1 M and 3.0, respectively Given at 298 K,K = 10–7K = 5 × 10–19Correct answer is 'Therefore, solubility of metal sulphide = 5 × 10–14 M.'. Can you explain this answer?, a detailed solution for At 298 K, calculate the solubility of metal sulfide, MS(s), in a saturated solution of H2S where the concentration of H2S and pH are maintained at 0.1 M and 3.0, respectively Given at 298 K,K = 10–7K = 5 × 10–19Correct answer is 'Therefore, solubility of metal sulphide = 5 × 10–14 M.'. Can you explain this answer? has been provided alongside types of At 298 K, calculate the solubility of metal sulfide, MS(s), in a saturated solution of H2S where the concentration of H2S and pH are maintained at 0.1 M and 3.0, respectively Given at 298 K,K = 10–7K = 5 × 10–19Correct answer is 'Therefore, solubility of metal sulphide = 5 × 10–14 M.'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice At 298 K, calculate the solubility of metal sulfide, MS(s), in a saturated solution of H2S where the concentration of H2S and pH are maintained at 0.1 M and 3.0, respectively Given at 298 K,K = 10–7K = 5 × 10–19Correct answer is 'Therefore, solubility of metal sulphide = 5 × 10–14 M.'. Can you explain this answer? tests, examples and also practice IIT JAM tests.