Upon mixming `100.0 mL` to `0.1 M` potassium solphate solution and `100.0 mL` of `0.05 M` barium chloride solution, precipitation of barium sulphate takes place. How many moles of barium sulphate are formed? Also, calculate the molar concentration of species left behind in the solution. Which is the limiting reagent?

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between potassium sulfate (K₂SO₄) and barium chloride (BaCl₂) can be represented as follows:

\[ K_2SO_4 + BaCl_2 \rightarrow BaSO_4 \downarrow + 2KCl \]

### Step 2: Calculate the number of moles of each reactant
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