Be sure to answer all parts. Ammonia has a Kp of 1.8 × 105. Find [H3O+], [OH¯ ], pH, and pOH for a 0.550 M ammonia solution. [H₂O+]: × 10 M [OH]: pH: POH: M (Enter your answer in scientific notation.)
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![**Chemistry: Calculating Ionic Concentrations and pH**
**Problem Statement**
Be sure to answer all parts.
**Ammonia (NH₃) has a base dissociation constant (Kb) of 1.8 × 10⁻⁵. Find the hydronium ion concentration \([H₃O⁺]\), hydroxide ion concentration \([OH⁻]\), pH, and pOH for a 0.550 M ammonia solution.**
---
**Given:**
- \( K_b = 1.8 \times 10^{-5} \)
- Ammonia concentration \([NH₃] = 0.550 M\)
**Solution:**
1. **Hydronium ion concentration, [H₃O⁺]:**
\[
[H₃O⁺] = \quad \times 10^{\quad} M \quad \text{(Enter your answer in scientific notation.)}
\]
2. **Hydroxide ion concentration, [OH⁻]:**
\[
[OH⁻] = \quad M
\]
3. **pH:**
\[
pH = \quad
\]
4. **pOH:**
\[
pOH = \quad
\]
**Hints:**
- Decide which method or formula to use.
- Pay attention to unit conversions and significant figures.
**Guided Solution:**
- Click on "Guided Solution" for detailed step-by-step instructions on solving this problem.
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**Note:**
- Ensure you understand the relationship between pH, pOH, and ion concentrations.
- Verify your answers as you proceed with the calculations.
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