Calculate the total concentration, in molarity, of hydroxide ions when 1,949.5 milligrams of magnesium hydroxide are completely dissolved into 0.112 L of 7.71 x10-¹ M NaOH. Assume the added solute does not contribute significantly to the total volume. Report your answer to three significant digits. 4

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**Problem Statement:**

Calculate the total concentration, in molarity, of hydroxide ions when 1,949.5 milligrams of magnesium hydroxide are completely dissolved into 0.112 L of 7.71 x 10^-1 M NaOH. Assume the added solute does not contribute significantly to the total volume. Report your answer to three significant digits.

**Instructions for Students:**

1. **Understand the Chemical Context:** Recognize that the problem involves the dissolution of magnesium hydroxide (Mg(OH)₂) in a sodium hydroxide (NaOH) solution.

2. **Calculate the Moles of Mg(OH)₂:**
   - Convert 1,949.5 mg of magnesium hydroxide to grams.
   - Use the molar mass of Mg(OH)₂ to find the moles present.

3. **Compute Moles of Hydroxide Ions from Mg(OH)₂:**
   - Determine the number of moles of hydroxide ions contributed by the dissolved magnesium hydroxide. (Remember that each mole of Mg(OH)₂ provides two moles of OH⁻ ions.)

4. **Calculate Hydroxide Ion Contribution from NaOH:**
   - Use the molarity of the NaOH solution to determine moles of OH⁻ ions present in 0.112 L.

5. **Determine Total Hydroxide Ion Concentration:**
   - Add the moles of OH⁻ ions from both sources.
   - Divide by the total volume to find the molarity of hydroxide ions, considering the assumption that volume addition is negligible.

6. **Express Final Answer:**
   - Report the concentration in molarity to three significant digits.

**Additional Notes:**
- **Equations to Use:**
  - Molarity (M) = moles of solute / liters of solution
  - Moles = mass (g) / molar mass (g/mol)

Ensure precision and use consistent units throughout calculations.
Transcribed Image Text:**Problem Statement:** Calculate the total concentration, in molarity, of hydroxide ions when 1,949.5 milligrams of magnesium hydroxide are completely dissolved into 0.112 L of 7.71 x 10^-1 M NaOH. Assume the added solute does not contribute significantly to the total volume. Report your answer to three significant digits. **Instructions for Students:** 1. **Understand the Chemical Context:** Recognize that the problem involves the dissolution of magnesium hydroxide (Mg(OH)₂) in a sodium hydroxide (NaOH) solution. 2. **Calculate the Moles of Mg(OH)₂:** - Convert 1,949.5 mg of magnesium hydroxide to grams. - Use the molar mass of Mg(OH)₂ to find the moles present. 3. **Compute Moles of Hydroxide Ions from Mg(OH)₂:** - Determine the number of moles of hydroxide ions contributed by the dissolved magnesium hydroxide. (Remember that each mole of Mg(OH)₂ provides two moles of OH⁻ ions.) 4. **Calculate Hydroxide Ion Contribution from NaOH:** - Use the molarity of the NaOH solution to determine moles of OH⁻ ions present in 0.112 L. 5. **Determine Total Hydroxide Ion Concentration:** - Add the moles of OH⁻ ions from both sources. - Divide by the total volume to find the molarity of hydroxide ions, considering the assumption that volume addition is negligible. 6. **Express Final Answer:** - Report the concentration in molarity to three significant digits. **Additional Notes:** - **Equations to Use:** - Molarity (M) = moles of solute / liters of solution - Moles = mass (g) / molar mass (g/mol) Ensure precision and use consistent units throughout calculations.
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