6.00 g of a compound, MC13 was dissolved in water. Excess aqueous silver nitrate was added to precipitate out all the chloride ions as silver chloride. The mass of AgCl obtained was 16.30 g. (a) Calculate the number of moles of silver chloride precipitated. (b) Write an ionic equation for the reaction of silver nitrate with MC13(aq). Calculate the relative atomic mass of M in the compound MC13.
6.00 g of a compound, MC13 was dissolved in water. Excess aqueous silver nitrate was added to precipitate out all the chloride ions as silver chloride. The mass of AgCl obtained was 16.30 g. (a) Calculate the number of moles of silver chloride precipitated. (b) Write an ionic equation for the reaction of silver nitrate with MC13(aq). Calculate the relative atomic mass of M in the compound MC13.
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Problem 4.84QP: A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to...
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![6.00 g of a compound, MCI, was dissolved in water. Excess aqueous silver nitrate was added
to precipitate out all the chloride ions as silver chloride. The mass of AgCl obtained was
16.30 g.
(a) Calculate the number of moles of silver chloride precipitated.
(b) Write an ionic equation for the reaction of silver nitrate with MC13(aq).
(c) Calculate the relative atomic mass of M in the compound MC13.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fafd8b140-7d32-4fb0-83f2-2671e45edad6%2Fed9f6c01-0554-4503-ae43-f74ad18cf8c4%2Fgnrfmv_processed.png&w=3840&q=75)
Transcribed Image Text:6.00 g of a compound, MCI, was dissolved in water. Excess aqueous silver nitrate was added
to precipitate out all the chloride ions as silver chloride. The mass of AgCl obtained was
16.30 g.
(a) Calculate the number of moles of silver chloride precipitated.
(b) Write an ionic equation for the reaction of silver nitrate with MC13(aq).
(c) Calculate the relative atomic mass of M in the compound MC13.
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