Why is it important to keep the NaOH solution (being used during titration) stoppered at all times when it is not in use? And why is it all right to use a wet flask for a titration experiment?
NaOH absorbs CO2 from the air.
Why not have a little water in the flask? as long as it contains none of the solutions being used you will have no extra moles of those materials. My students always told me, "but you're diluting the titrant" or "you're diluting the material in the flask." My answer was always, "true, we are diluting the material in the flask BUT we also dilute the material being added from the buret by exactly the same amount."
Ah, the mysteries of chemistry! Well, my curious friend, let me sprinkle some humor on your questions.
Firstly, keeping the NaOH solution stoppered is important because NaOH is like a mischievous escape artist. It's so slippery, it may decide to sneak out and play hide-and-seek with your experiment, leaving you with inaccurate results. And you don't want your titration turning into a game of Where's Waldo, do you?
Now, onto the wet flask! You know, using a wet flask is perfectly fine in titration experiments. It's like giving your glassware a refreshing shower before the main event. You want that flask nice and wet because, let's face it, water is clingy. It likes to stick around and form a thin film on the glass surface, making it easier for us chemists to spot any color changes. It's like having a guardian angel guiding you through your titration adventure, ensuring you get precise results every time.
Remember, my friend, in the world of chemistry, even the smallest details can make a big difference. So keep that NaOH solution stoppered and embrace the wonders of a wet flask!
It is important to keep the NaOH solution stoppered at all times when it is not in use for several reasons:
1. Protection from air: NaOH is hygroscopic, which means it easily absorbs moisture from the air. This moisture can change the concentration of the solution, affecting the accuracy of the titration results.
2. Protection from carbon dioxide: Carbon dioxide from the atmosphere can dissolve in NaOH solution, forming carbonate ions. The presence of carbonate ions can lead to errors in the titration, as they can react with the acid being titrated.
3. Safety: NaOH is a corrosive substance and can cause injury if it comes into contact with skin or eyes. Keeping the solution stoppered reduces the risk of accidental spills and exposure.
Regarding the use of a wet flask for a titration experiment, it is generally acceptable as long as certain precautions are taken:
1. Thorough rinsing: The flask should be thoroughly rinsed with distilled water before pouring the NaOH solution into it. This removes any impurities that could affect the accuracy of the titration.
2. Controlled moisture: Excessive moisture in the flask should be avoided. After rinsing, any excess water should be removed from the flask before starting the titration. This can be done by draining the excess water or by drying the flask using a gentle stream of air.
3. Calibration: If using a wet flask, it is important to calibrate it by determining the volume of water retained in the flask when it is "wet." This volume should be taken into account during calculations to ensure accurate titration results.
It is important to keep the NaOH solution stoppered at all times when it is not in use during a titration experiment for a few reasons:
1. Protection from atmospheric moisture: NaOH is a hygroscopic substance, meaning it readily absorbs moisture from the surrounding air. Keeping the solution stoppered helps prevent water vapor from entering the container and reacting with the NaOH. If water vapor comes in contact with NaOH, it can cause the solution to become diluted, affecting its concentration and accuracy during titration.
2. Minimizing the risk of contamination: By stoppering the NaOH solution, you can prevent any foreign particles or impurities from entering the solution. Contaminants can affect the purity and composition of the NaOH, leading to inaccurate results during titration.
On the other hand, using a wet flask for a titration experiment is generally acceptable for a few reasons:
1. Thorough rinsing: Prior to conducting a titration, it is customary to rinse the flask with some distilled water. This rinsing ensures that any residual substances in the flask are removed, minimizing their potential impact on the titration results.
2. Negligible impact on concentration: In most cases, a small amount of water left in the flask after rinsing will not significantly affect the concentration of the titrant. As long as the residual water is minimal, it is generally considered acceptable and will not substantially alter the accuracy of the titration.
It is important to note that these guidelines may vary depending on the specific experiment or protocol being followed. Consulting the specific instructions or guidelines provided by your teacher or lab manual is always recommended to ensure the best practices are followed.