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Naturally occurring boron consists of ...

Naturally occurring boron consists of two isotopes whese atomic weights are `10.01` and `11.01`. The atomic weight of natural boron is `10.81`. Calculate the percentage of each isotope in natural boron.

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To solve the problem of finding the percentage of each isotope in naturally occurring boron, we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Isotopes and Their Weights**: - Isotope 1 (Boron-10): Atomic weight = 10.01 - Isotope 2 (Boron-11): Atomic weight = 11.01 - Average atomic weight of natural boron = 10.81 2. **Define the Variables**: - Let the percentage (relative abundance) of Isotope 1 (Boron-10) be \( \alpha \). - Therefore, the percentage of Isotope 2 (Boron-11) will be \( 100 - \alpha \). 3. **Set Up the Equation for Average Atomic Weight**: The average atomic weight can be expressed as: \[ \text{Average Atomic Weight} = \frac{(10.01 \times \alpha) + (11.01 \times (100 - \alpha))}{100} \] Given that the average atomic weight is 10.81, we can set up the equation: \[ 10.81 = \frac{(10.01 \times \alpha) + (11.01 \times (100 - \alpha))}{100} \] 4. **Clear the Denominator**: Multiply both sides of the equation by 100 to eliminate the fraction: \[ 10.81 \times 100 = 10.01 \times \alpha + 11.01 \times (100 - \alpha) \] This simplifies to: \[ 1081 = 10.01 \alpha + 1101 - 11.01 \alpha \] 5. **Combine Like Terms**: Rearranging the equation gives: \[ 1081 = 1101 - 0.99 \alpha \] Now, isolate \( \alpha \): \[ 0.99 \alpha = 1101 - 1081 \] \[ 0.99 \alpha = 20 \] 6. **Solve for \( \alpha \)**: Divide both sides by 0.99: \[ \alpha = \frac{20}{0.99} \approx 20.20 \] 7. **Calculate the Percentage of Isotope 2**: Since \( \alpha \) represents the percentage of Isotope 1: \[ \text{Percentage of Isotope 2} = 100 - \alpha \approx 100 - 20.20 \approx 79.80 \] 8. **Final Results**: - Percentage of Isotope 1 (Boron-10) ≈ 20.20% - Percentage of Isotope 2 (Boron-11) ≈ 79.80% ### Summary: - The percentage of Boron-10 is approximately **20.20%**. - The percentage of Boron-11 is approximately **79.80%**.

To solve the problem of finding the percentage of each isotope in naturally occurring boron, we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Isotopes and Their Weights**: - Isotope 1 (Boron-10): Atomic weight = 10.01 - Isotope 2 (Boron-11): Atomic weight = 11.01 - Average atomic weight of natural boron = 10.81 ...
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