Questions: BaCl2 + K2CrO4

BaCl2 + K2CrO4
Transcript text: $\mathrm{BaCl}_{2}+\mathrm{K}_{2} \mathrm{CrO}_{4}$
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Solution

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Solution Steps

Step 1: Identify the Reactants and Products

The given chemical reaction involves barium chloride (\(\mathrm{BaCl}_{2}\)) and potassium chromate (\(\mathrm{K}_{2} \mathrm{CrO}_{4}\)).

Step 2: Write the Balanced Chemical Equation

To determine the products, we need to consider the possible double displacement reaction. The barium ion (\(\mathrm{Ba}^{2+}\)) will pair with the chromate ion (\(\mathrm{CrO}_{4}^{2-}\)), and the potassium ion (\(\mathrm{K}^{+}\)) will pair with the chloride ion (\(\mathrm{Cl}^{-}\)).

The balanced chemical equation is: \[ \mathrm{BaCl}_{2} + \mathrm{K}_{2} \mathrm{CrO}_{4} \rightarrow \mathrm{BaCrO}_{4} + 2\mathrm{KCl} \]

Step 3: Verify the Balanced Equation

Ensure that the number of atoms of each element is the same on both sides of the equation:

  • Barium (Ba): 1 on both sides
  • Chlorine (Cl): 2 on both sides
  • Potassium (K): 2 on both sides
  • Chromium (Cr): 1 on both sides
  • Oxygen (O): 4 on both sides

The equation is balanced.

Final Answer

\[ \boxed{\mathrm{BaCl}_{2} + \mathrm{K}_{2} \mathrm{CrO}_{4} \rightarrow \mathrm{BaCrO}_{4} + 2\mathrm{KCl}} \]

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