yohollyyo
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#1
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In the following ionic equation, there is 1 mole of AgCl, but 2 moles of Cl^-, despite the molar ratio being 1:1. I don't understand this; can somebody explain why please!
Ag^+ + Cl^- --> AgCl

(from F321 June '12 paper)
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7253567
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Where does it say their are 2 moles of silver+


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7253567
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Chloride


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Borek
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If possible, please quote entire question.
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yohollyyo
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Deduce the amount, in moles, of the Group 2 chloride that the student dissolves.
Hence deduce the relative atomic mass and the identity of the Group 2 metal

From a previous questions, we know that the ionic equation for the reaction is
Ag^+ + Cl^- --> AgCl
And that there are 0.06 moles of AgCl

But in the mark scheme, it says: amount of Group 2 chloride = 1⁄2 × 0.0600 OR = 0.0300mol

I understand the rest of how you work it out, but not this first part
Sorry if I'm not making myself clear!
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Borek
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What are group 2 metals? Can you list them? Is silver between them?
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yohollyyo
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It was AgNo^3 and the question was asking you to work out what was bonded to the chloride in the first part; I think the correct answer was Magnesium.
The reaction was the silver nitrate test for identifying halides.


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