Melodyharmony
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If 0.1mol of the isomer reacts with 0.2mol of AgNO3, that means the ratio is 1:2, and there would be 2Cl involved, so shouldn't the answer be C?
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Toscana
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this some big brain stuff
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Melodyharmony
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(Original post by Toscana)
this some big brain stuff
I was hoping you were the one with the big brains
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Pigster
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(Original post by Melodyharmony)
If 0.1mol of the isomer reacts with 0.2mol of AgNO3, that means the ratio is 1:2, and there would be 2Cl involved, so shouldn't the answer be C?
The two Cl in the complex are dative covalently bonded to the Cr.

You may note that there are three Cl in the formula and the complex ion has a charge of 2+.

Therefore, in B, the other two Cl are in the form of Cl- (to balance out the charge). These two Cl- ions are available to ppt out with the Ag+.

The two NO3- that were with the Ag+ now perform the task of balancing out the charge on the complex ion.
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Melodyharmony
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(Original post by Pigster)
The two Cl in the complex are dative covalently bonded to the Cr.

You may note that there are three Cl in the formula and the complex ion has a charge of 2+.

Therefore, in B, the other two Cl are in the form of Cl- (to balance out the charge). These two Cl- ions are available to ppt out with the Ag+.

The two NO3- that were with the Ag+ now perform the task of balancing out the charge on the complex ion.
Oh I see. So B actually stands for [CrCl(H2O)5]2+2Cl-? So does the Cl in CrCl not react with Ag+? Why not?
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Pigster
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(Original post by Melodyharmony)
Oh I see. So B actually stands for [CrCl(H2O)5]2+2Cl-? So does the Cl in CrCl not react with Ag+? Why not?
Like I said... the Cl in the complex is covalently bonded to the Cr. It is not a Cl- ion. Ag requires free Cl- ions to ppt.
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Melodyharmony
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(Original post by Pigster)
Like I said... the Cl in the complex is covalently bonded to the Cr. It is not a Cl- ion. Ag requires free Cl- ions to ppt.
Oh sorry about that 😅😅
Thank you so much!!!
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