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MentorMill Titration of a Strong Acid with a Strong Base

Name: MentorMill Titration of a Strong Acid with a Strong Base
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Titration of a Strong Acid with a Strong Base – A Precise Method for Determining Concentration

Titration is a laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. In the case of titrating a strong acid with a strong base, this method involves the neutralization reaction between a strong acid (such as hydrochloric acid, HCl) and a strong base (such as sodium hydroxide, NaOH).

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Preparation: The acid (strong acid) is placed in a burette, and the base (strong base) is placed in a conical flask along with a few drops of a suitable indicator, typically phenolphthalein or methyl orange, which will change color when the solution reaches the endpoint.
Neutralization Reaction: As the base is slowly added to the acid, a neutralization reaction occurs:
$HCl (aq)+NaOH (aq)→NaCl (aq)+H2O (l)\text{HCl (aq)} + \text{NaOH (aq)} \rightarrow \text{NaCl (aq)} + \text{H}_2\text{O (l)}$ $HCl (aq)$ $+$ $NaOH (aq)$ $\to$ $NaCl (aq)$ $+$ $H$ $2$ $$ $O (l)$
The reaction results in the formation of salt and water.
End Point: The titration continues until the indicator changes color, signaling the neutralization point. The volume of base added to the acid at this point is noted.
Calculation: Using the volume of the base solution added and its known concentration, the concentration of the acid solution can be calculated using the formula:
$M1×V1=M2×V2\text{M}_1 \times \text{V}_1 = \text{M}_2 \times \text{V}_2$ $M$ $1$ $$ $\times$ $V$ $1$ $$ $=$ $M$ $2$ $$ $\times$ $V$ $2$ $$