Question

reaction 10d: previous products with additional hydrochloric acid copper ions react with excess chloride to form cucl42- balanced net ionic equation (complex equation)

Explanation:

Step1: Identify reactants and product

Reactants: Copper ions ($\text{Cu}^{2+}$) and excess chloride ions ($\text{Cl}^-$ from HCl or other chloride sources). Product: Tetrachlorocuprate(II) ion ($\text{[CuCl}_4\text{]}^{2-}$).

Step2: Write unbalanced ionic equation

$\text{Cu}^{2+}(aq) + \text{Cl}^-(aq)
ightarrow \text{[CuCl}_4\text{]}^{2-}(aq)$

Step3: Balance the equation

Balance Cl atoms: There are 4 Cl in the product, so add 4 to $\text{Cl}^-$ on the left.
$\text{Cu}^{2+}(aq) + 4\text{Cl}^-(aq)
ightarrow \text{[CuCl}_4\text{]}^{2-}(aq)$

Check charge balance: Left side: $+2 + 4(-1) = -2$. Right side: $-2$. Charge is balanced. Also, Cu is balanced (1 on each side).

Answer:

$\boldsymbol{\text{Cu}^{2+}(aq) + 4\text{Cl}^-(aq) = \text{[CuCl}_4\text{]}^{2-}(aq)}$