3) If a 35.75 mL sample of 0.175 M HCI (aq) solution is neutralized with 0.125 M Mg(OH)2, how much Mg(OH)2 will be needed? 2 HCI (aq) + Mg(OH), (aq) → MgCl2(aq) + 2 HOH (I)

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### Chemistry Problem: Neutralization Reaction

**Problem Statement:**

If a 35.75 mL sample of 0.175 M HCl (\(aq\)) solution is neutralized with 0.125 M Mg(OH)\(_2\), how much Mg(OH)\(_2\) will be needed?

**Chemical Equation:**

\[ 2 \, \text{HCl} \, (aq) + \text{Mg(OH)}_2 \, (aq) \rightarrow \text{MgCl}_2 \, (aq) + 2 \, \text{HOH} \, (l) \]

**Explanation:**

This problem involves a neutralization reaction, where hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)\(_2\)) to form magnesium chloride (MgCl\(_2\)) and water (H\(_2\)O), represented as HOH here. The balanced equation shows that two moles of HCl react with one mole of Mg(OH)\(_2\).

To find the amount of Mg(OH)\(_2\) needed:

1. Calculate the moles of HCl present in the sample using the volume and molarity.
2. Use the stoichiometry of the reaction (2:1 ratio) to find the moles of Mg(OH)\(_2\) needed.
3. Convert the moles of Mg(OH)\(_2\) to the required volume using its molarity.

This exercise demonstrates stoichiometry concepts in chemistry, focusing on balancing reactions and using molarity in calculations.
Transcribed Image Text:### Chemistry Problem: Neutralization Reaction **Problem Statement:** If a 35.75 mL sample of 0.175 M HCl (\(aq\)) solution is neutralized with 0.125 M Mg(OH)\(_2\), how much Mg(OH)\(_2\) will be needed? **Chemical Equation:** \[ 2 \, \text{HCl} \, (aq) + \text{Mg(OH)}_2 \, (aq) \rightarrow \text{MgCl}_2 \, (aq) + 2 \, \text{HOH} \, (l) \] **Explanation:** This problem involves a neutralization reaction, where hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)\(_2\)) to form magnesium chloride (MgCl\(_2\)) and water (H\(_2\)O), represented as HOH here. The balanced equation shows that two moles of HCl react with one mole of Mg(OH)\(_2\). To find the amount of Mg(OH)\(_2\) needed: 1. Calculate the moles of HCl present in the sample using the volume and molarity. 2. Use the stoichiometry of the reaction (2:1 ratio) to find the moles of Mg(OH)\(_2\) needed. 3. Convert the moles of Mg(OH)\(_2\) to the required volume using its molarity. This exercise demonstrates stoichiometry concepts in chemistry, focusing on balancing reactions and using molarity in calculations.
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