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Answer :
The concentrations are [OH⁻] = 3.0 M and [H₃O⁺] = 3.33 × 10⁻¹⁵ M
Let's approach this problem step-by-step:
1. Understand the given information:
- We have a Sr(OH)₂ solution
- The concentration is 1.5 M
2. Write the dissociation equation for Sr(OH)₂:
Sr(OH)₂ → Sr²⁺ + 2OH⁻
3. Calculate the concentration of OH⁻:
- Each mole of Sr(OH)₂ produces 2 moles of OH⁻
- So, [OH⁻] = 2 × [Sr(OH)₂] = 2 × 1.5 M = 3.0 M
4. Use the ion product of water (Kw) to find [H₃O⁺]:
Kw = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25°C
5. Rearrange to solve for [H₃O⁺]:
[H₃O⁺] = Kw / [OH⁻] = (1.0 × 10⁻¹⁴) / (3.0)
6. Calculate [H₃O⁺]:
[H₃O⁺] = 3.33 × 10⁻¹⁵ M
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