Which describes the final laboratory observation when $0.40$ moles of $N a O H_{(s)}$ is added to $0.50$ liters of $0.60 M C u C l_{2}$ solution?

A precipitate forms; excess copper ions are found.

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A precipitate forms; excess hydroxide ions are found.

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A nearly colorless solution forms; excess copper ions are found.

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A nearly colorless solution forms; excess hydroxide ions are found.

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Solution

The correct option is B A precipitate forms; excess copper ions are found.
Balanced reaction is:
$2 N a O H      0.4 m o l e s + C u C l_{2}      0.3 m o l e s ⟶ 2 N a C l + C u (O H)_{2} ↓    p p t$
$x =$ No. of moles $=$ Molarity $\times$ Volume $= 0.5 \times 0.6 = 0.3$
$1$ $m o l e$ of $C u C l_{2}$ react with $2$ $m o l e s$ of $N a O H$
$0.4$ $m o l e$ of $N a O H$ react with $0.2$ $m o l e s$ of $C u C l_{2}$
$0.1$ $m o l e$ of $C u C l_{2}$ will be left.
So, percipitate is formed $(C u (O H)_{2})$ and excess copper ions are left.

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Which describes the final laboratory observation when 0.40 moles of NaOH(s) is added to 0.50 liters of 0.60 M CuCl2 solution?

Which describes the final laboratory observation when $0.40$ moles of $N a O H_{(s)}$ is added to $0.50$ liters of $0.60 M C u C l_{2}$ solution?