Consider the following transformations:I. XeF | vedclass

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(A) All three transformations are chemically correct and balanced:$I.$ $XeF_6$ acts as a fluoride ion acceptor,reacting with $NaF$ to form the complex

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$I, II, III$

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(A) All three transformations are chemically correct and balanced:$I.$ $XeF_6$ acts as a fluoride ion acceptor,reacting with $NaF$ to form the complex salt $Na^+[XeF_7]^-$.$II.$ In the solid state,$PCl_5$ exists as an ionic lattice consisting of $[PCl_4]^+$ and $[PCl_6]^-$ ions.$III.$ The hydrated aluminum ion $[Al(H_2O)_6]^{3+}$ acts as a weak acid in water,donating a proton to form $[Al(H_2O)_5OH]^{2+}$ and $H_3O^+$.Therefore,all three transformations are correct.

Consider the following transformations:
$I. XeF_6 + NaF \to Na^+[XeF_7]^-$
$II. 2PCl_{5(s)} \to [PCl_4]^+[PCl_6]^-$
$III. [Al(H_2O)_6]^{3+} + H_2O \to [Al(H_2O)_5OH]^{2+} + H_3O^+$
Which of the above transformations are correct?

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Consider the following transformations:$I. XeF_6 + NaF \to Na^+[XeF_7]^-$$II. 2PCl_{5(s)} \to [PCl_4]^+[PCl_6]^-$$III. [Al(H_2O)_6]^{3+} + H_2O \to [Al(H_2O)_5OH]^{2+} + H_3O^+$Which of the above transformations are correct?