What is the Molarity of an Acid Sample Neutralized by NaOH?

In summary, standardizing an acid is the process of determining its exact concentration, which is crucial in scientific experiments. This is done by titrating the acid with a known concentration of base and using the equation M1V1 = M2V2 to calculate its concentration. The most commonly used indicators for acid standardization are phenolphthalein and methyl orange, depending on the strength of the acid and base. It is important to use a standardized acid in experiments to ensure accuracy and reproducibility of results. Potential sources of error in acid standardization include measurement errors, mishandling of indicators, and inaccuracies in the concentration of the base used for titration.
  • #1
kara
54
0
It requires 46.5 mL of 0.215M NaOH to neutralize 15.0 mL of aqueous H2SO4. What was the molarity (M) of the acid sample?

I'm not quite sure how to approach this quesiton, if anyone has and starter tips please let me know.
 
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  • #2
So for a I know that M (molarity) = moles of solute/liters of sol'n
 
  • #3
Don't worry about it, I figured it out :D
 

1. What is the purpose of standardizing an acid?

The purpose of standardizing an acid is to determine its exact concentration or molarity. This is important in many scientific experiments, as the concentration of an acid can greatly affect the outcome of a reaction.

2. How is an acid standardized?

An acid is standardized by titrating it with a base of known concentration. The volume of the base required to neutralize the acid is used to calculate the acid's concentration using the equation M1V1 = M2V2, where M1 is the concentration of the base, V1 is the volume of base used, M2 is the concentration of the acid, and V2 is the volume of acid used.

3. What are the common indicators used in acid standardization?

The most commonly used indicators in acid standardization are phenolphthalein and methyl orange. Phenolphthalein is used for strong acids and bases, while methyl orange is used for weak acids and bases.

4. Why is it important to use a standardized acid in experiments?

Using a standardized acid ensures accuracy and reproducibility of experimental results. If the acid used is not accurately standardized, it can lead to incorrect conclusions and unreliable data.

5. What are the potential sources of error in acid standardization?

The potential sources of error in acid standardization include incorrect measurement of volumes, improper handling of the indicator, contamination of the acid or base, and inaccuracies in the concentration of the base used for titration.

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