Question #47e74

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Question #47e74

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Answer 1 · 2017-09-25T06:08:32

$N i {(C l O_{4})}_{2} (s) H_{2} O - - \to N i^{2 +} + 2 C l O_{4}^{-}$ $Ni(ClO_4)_2(s)stackrel(H_2O)rarrNi^(2+) + 2ClO_4^(-)$

Explanation:

As with any chemical reaction, MASS and CHARGE are conserved absolutely. We started with a NEUTRAL material, and the TOTAL charge of the ions on the right hand side is neutral. We started with approx. $258 \cdot g$ $258*g$ of the perchlorate. There are precisely $258.8 \cdot g$ $258.8*g$ in solution.

Therefore we started with 4 moles of $N i {(C l O_{4})}_{2}$ $Ni(ClO_4)_2$ . I think that when this dissolves in solution, there will be FOUR MOLES of $N i^{2 +}$ $Ni^(2+)$ , and HOW MANY MOLES of perchlorate anion?

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