Question

Sodium hydroxide used to make standard \(\mathrm{NaOH}(\mathrm{aq})\) solutions for acid-base titrations is invariably contaminated with some sodium carbonate. (a) Explain why, except in the most precise work, the presence of this sodium carbonate generally does not seriously affect the results obtained, for example, when \(\mathrm{NaOH}(\mathrm{aq})\) is used to titrate HCl(aq). (b) Conversely, show that if \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) comprises more than \(1 \%\) to \(2 \%\) of the solute in NaOH(aq), the titration results are affected.

Short answer

The presence of a small amount of Sodium Carbonate doesn't affect the titration results as sodium hydroxide, the strong base, reacts first with the acid. Sodium carbonate, being a weak base, only starts to react after all the sodium hydroxide has reacted. On the other hand, when sodium carbonate's composition goes beyond 1-2%, it starts reacting with the acid before all the sodium hydroxide is consumed, which leads to incorrect results.

Step-by-step solution

Explain why a small amount of sodium carbonate does not affect titration results

Sodium hydroxide is a strong base and sodium carbonate will act as a source of weak base. When a solution of sodium hydroxide is titrated against an acid (\(HCl\) in this case), the strong base will react first. Any sodium carbonate contamination will begin reacting only after all the sodium hydroxide has reacted. Therefore, even if there is a slight contamination of sodium carbonate, it will not significantly affect the results of the titration due to its weak basicity.

Show that if Na2CO3 is 1-2% of the solute in NaOH, titration results are affected

If the percentage of sodium carbonate rises to 1-2%, it means it is no longer negligible. The increased concentration of sodium carbonate can result in its reaction with the acid before all the sodium hydroxide is consumed. This would cause an earlier than expected end point in the titration, leading to higher values of acid concentration.

Key concepts

Sodium Hydroxide

Sodium hydroxide, also known as lye or caustic soda, is a highly soluble white solid that is commonly used in chemical laboratories. It is known for being a strong base, meaning it can easily dissociate in water to release hydroxide ions (\(OH^-\)). This property makes it an essential component in acid-base titrations, where its primary role is to neutralize acids.
Sodium hydroxide solutions are widely used because they provide a reliable measure of strength, allowing for accurate comparison in titration processes. Despite its usefulness, sodium hydroxide solutions are prone to contamination by sodium carbonate due to exposure to air, as sodium hydroxide reacts with atmospheric carbon dioxide (\(CO_2\)) to form sodium carbonate (\(Na_2CO_3\)). Understanding this common yet manageable contamination is crucial for accurate titration results.

Sodium Carbonate Contamination

Sodium carbonate contamination in sodium hydroxide solutions occurs naturally when sodium hydroxide absorbs carbon dioxide from the air. This forms sodium carbonate, which is a weaker base compared to sodium hydroxide. Typically, sodium carbonate contamination is negligible in small amounts and does not drastically alter the outcome of a titration.
However, if the contamination exceeds 1-2%, it can lead to significant errors in titration results. Sodium carbonate, being a weak base, will begin to react with the acid used in the titration after all the sodium hydroxide has already reacted. This premature reaction shifts the titration endpoint and can result in miscalculations of the acid concentration. To minimize these issues, ensure proper storage and handling of sodium hydroxide to reduce exposure to air.

Titration Endpoint

The titration endpoint is the stage in a titration when the reaction between the titrant and the analyte is complete. At this point, any further addition of titrant stops producing a noticeable reaction, typically indicated by a color change if an indicator is used. The endpoint is critical for determining the exact point of neutralization.
In cases where sodium hydroxide is contaminated with sodium carbonate, achieving a precise endpoint can be problematic. If the sodium carbonate contamination is significant, it can lead to an earlier endpoint. This early endpoint is misleading because it suggests that all the sodium hydroxide has reacted when, in fact, part of the titrant is unreacted. To recognize contamination's impact on the endpoint, it's essential to account for any potential interference from sodium carbonate.

Acid Concentration

Acid concentration in a titration process refers to the molarity or strength of the acid being analyzed. By reaching the titration endpoint accurately, one can compute the acid concentration using the known concentration and volume of the titrant, such as sodium hydroxide.
When sodium carbonate contamination is present in sodium hydroxide, your calculated acid concentration may be higher than it actually is. This happens if the carbonate reacts early with the acid, falsely indicating that more acid has been required to reach the endpoint. Consequently, understanding the degree of contamination allows chemists to make necessary adjustments in calculations to ensure accurate results. To get trustworthy acid concentration readings, regularly check the purity of your sodium hydroxide solutions.

Chemical Reactions in Titration

Chemical reactions in titration involve a titrant reacting with the analyte in a highly controlled chemical process. Typically, an acid-base titration involves a base, such as sodium hydroxide, reacting with an acid to form water and salt. The reaction proceeds until the titration endpoint is reached.
For example, in a titration of hydrochloric acid (\(HCl\)) with sodium hydroxide, the reaction can be represented by:\(\mathrm{NaOH} + \mathrm{HCl} \rightarrow \mathrm{NaCl} + \mathrm{H_2O}\).If sodium carbonate is present, another reaction can occur early in the titration:\(\mathrm{Na_2CO_3} + 2\mathrm{HCl} \rightarrow \mathrm{2NaCl} + \mathrm{H_2O} + \mathrm{CO_2}\).
This additional reaction from carbonate contamination must be accounted for to avoid misjudging the endpoint and miscalculating results, emphasizing the importance of knowing the chemical nuances within the reaction.