How Much HCl Is Needed to Neutralize NaOH?

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Discussion Overview

The discussion revolves around the stoichiometry involved in neutralizing sodium hydroxide (NaOH) with hydrochloric acid (HCl). Participants explore the conditions under which limiting reagents need to be considered in acid-base reactions, particularly focusing on a specific problem involving the volumes and molarities of the reactants.

Discussion Character

  • Technical explanation, Conceptual clarification, Homework-related

Main Points Raised

  • One participant questions why the reaction does not require determining a limiting reagent, noting that the problem specifies adding just enough hydrogen ions to react with the hydroxide ions present.
  • Another participant realizes that since the volume of NaOH is fixed, the exact amount of HCl needed can be calculated without considering limiting reagents, unless the volumes were different.
  • A third participant suggests a straightforward approach to the problem by calculating the moles of NaOH first and then determining the corresponding volume of HCl required.
  • One participant asks if the calculation led to the correct answer of 87.5 mL of HCl.

Areas of Agreement / Disagreement

Participants generally agree on the approach to solving the problem and the reasoning behind not needing to consider limiting reagents in this specific case. However, there is no consensus on the final answer, as one participant asks for confirmation of the calculated volume.

Contextual Notes

The discussion does not resolve the broader question of when limiting reagents should be considered in other contexts, leaving some assumptions and conditions unaddressed.

Who May Find This Useful

Students and individuals interested in acid-base chemistry, particularly those learning about stoichiometry and neutralization reactions.

Integral0
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What volume of a .100 M HCl is needed to neutralize 25.0 mL of a .350 Molarity Sodium Hydroxide?

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I don't understand why this reaction doesn't require you to determine the limiting reagent (there is none).

The book explicitly says "This problem requires the addition of just enough Hydrogen ions to react exactly with the OH- ions present."

Even with this description my mind is still a little fuzzy on how I can determine when a problem needs a limiting reagent to be found and when a problem doesn't need a limiting reagent found.

Please shed some light on this issue.
 
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oops, I know why now.


Since 25 mL is the only exact volume (excluding the molarities). You are finding the exact amount of H that will react with the exact amount of Hydroxides. If HCl had an amount of mL different than NaOH . . . then you would determine the LR.

:D
 
Looks like you got it. Do you still need help?

It's pretty easy. Just figure out how many moles of NaOH you have. Then figure out how many mL's HCl that would be.
 
Did you come to the right answer? 87.5 ml
 

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