Calculating the Number of Moles of BaCl2

Oct 13, 2025 by magicalceylontours.com 73 views

Understanding the Chemical Reaction

The given chemical reaction is: $$BaCl_2(aq) + Na_2SO_4(aq) \rightarrow BaSO_4(s) + 2 NaCl(aq)$$

This is a double displacement reaction where barium chloride reacts with sodium sulfate to form barium sulfate and sodium chloride. The reaction is a classic example of a precipitation reaction, where the product, barium sulfate, is insoluble in water and precipitates out of the solution.

Calculating the Number of Moles of BaCl2

To calculate the number of moles of BaCl2, we need to multiply the volume of the solution (in liters) by the molarity of the solution.

First, we need to convert the volume from milliliters to liters:

25.34 \, \text{mL} = 0.02534 \, \text{L}

Now, we can calculate the number of moles of BaCl2:

n_{BaCl_2} = M_{BaCl_2} \times V_{BaCl_2}

n_{BaCl_2} = 0.113 \, \text{M} \times 0.02534 \, \text{L}

n_{BaCl_2} = 0.00287 \, \text{mol}

Calculating the Number of Moles of Na2SO4 Required

From the balanced chemical equation, we can see that 1 mole of BaCl2 reacts with 1 mole of Na2SO4. Therefore, the number of moles of Na2SO4 required is equal to the number of moles of BaCl2:

n_{Na_2SO_4} = n_{BaCl_2}

n_{Na_2SO_4} = 0.00287 \, \text{mol}

Calculating the Volume of Na2SO4 Required

To calculate the volume of Na2SO4 required, we need to divide the number of moles of Na2SO4 by the molarity of the Na2SO4 solution:

V_{Na_2SO_4} = \frac{n_{Na_2SO_4}}{M_{Na_2SO_4}}

V_{Na_2SO_4} = \frac{0.00287 \, \text{mol}}{0.218 \, \text{M}}

V_{Na_2SO_4} = 0.0131 \, \text{L}

Converting the Volume from Liters to Milliliters

To convert the volume from liters to milliliters, we can multiply by 1000:

V_{Na_2SO_4} = 0.0131 \, \text{L} \times 1000 \, \frac{\text{mL}}{\text{L}}

V_{Na_2SO_4} = 13.1 \, \text{mL}

The final answer is $\boxed{13.1}$

Q: What is the chemical reaction between BaCl2 and Na2SO4?

A: The chemical reaction between BaCl2 and Na2SO4 is: $$BaCl_2(aq) + Na_2SO_4(aq) \rightarrow BaSO_4(s) + 2 NaCl(aq)$$

Q: What is the product of the reaction?

A: The product of the reaction is barium sulfate (BaSO4) and sodium chloride (NaCl).

Q: Is the product of the reaction soluble in water?

A: No, the product of the reaction, barium sulfate, is insoluble in water and precipitates out of the solution.

Q: How many moles of BaCl2 are present in 25.34 mL of 0.113 M BaCl2?

A: To calculate the number of moles of BaCl2, we need to multiply the volume of the solution (in liters) by the molarity of the solution:

n_{BaCl_2} = M_{BaCl_2} \times V_{BaCl_2}

n_{BaCl_2} = 0.113 \, \text{M} \times 0.02534 \, \text{L}

n_{BaCl_2} = 0.00287 \, \text{mol}

Q: How many moles of Na2SO4 are required to react with 0.00287 mol of BaCl2?

A: From the balanced chemical equation, we can see that 1 mole of BaCl2 reacts with 1 mole of Na2SO4. Therefore, the number of moles of Na2SO4 required is equal to the number of moles of BaCl2:

n_{Na_2SO_4} = n_{BaCl_2}

n_{Na_2SO_4} = 0.00287 \, \text{mol}

Q: How many mL of 0.218 M Na2SO4 are required to react with 0.00287 mol of BaCl2?

A: To calculate the volume of Na2SO4 required, we need to divide the number of moles of Na2SO4 by the molarity of the Na2SO4 solution:

V_{Na_2SO_4} = \frac{n_{Na_2SO_4}}{M_{Na_2SO_4}}

V_{Na_2SO_4} = \frac{0.00287 \, \text{mol}}{0.218 \, \text{M}}

V_{Na_2SO_4} = 0.0131 \, \text{L}

Q: What is the final answer?

A: The final answer is $\boxed{13.1}$ mL of 0.218 M Na2SO4.

Q: What is the purpose of the reaction?

A: The purpose of the reaction is to determine the amount of Na2SO4 required to react with a given amount of BaCl2.

Q: What are the limitations of the reaction?

A: The limitations of the reaction are that it assumes that the reaction is a simple double displacement reaction and that the products are insoluble in water.

Q: What are the applications of the reaction?

A: The applications of the reaction are in the field of chemistry, where it is used to determine the amount of a substance required to react with another substance.

Q: What are the safety precautions for the reaction?

A: The safety precautions for the reaction are to handle the chemicals with care, wear protective gear, and perform the reaction in a well-ventilated area.

Q: What are the environmental concerns for the reaction?

A: The environmental concerns for the reaction are the potential for the products to contaminate the environment and the potential for the chemicals to be hazardous to human health.