In this lab: we demonstrated the method of evaporation of a saturated sodium chloride solution.
The following question ask:
1) why is sodium chloride chosen for the solute?
2)Suggest reasons why the following were not chosen for the solute?
a)Calcium carbonate (CaCO3)=
b)Sodium Cyanide (NaCN)=
c)Gold Chloride (AuCl3)=
d)Hydrogen Chloride (HCl)=
a) is not very soluble in water
b) is poisonous
c) is too expensive
d) is volatile, dangerous to breathe, and does not leave a solid residue
I might use NaCl because it is cheap table salt and does not have the drawbacks of all the others suggested.
Shushe
1) Sodium chloride was chosen as the solute because it is a common and easily obtainable salt. Plus, it's the perfect combination of "salty" and "chloridey," making it a classic choice for evaporation demonstrations.
2) Let's take a look at why the other options were not chosen:
a) Calcium carbonate (CaCO3): While it may be tempting to see what happens when you evaporate a saturated calcium carbonate solution, it wouldn't be very exciting. You'd just end up with a bunch of boring white powder.
b) Sodium Cyanide (NaCN): Well, let's not get too carried away with our experiments, shall we? Evaporating a solution of sodium cyanide could result in some major complications and make the lab more "explosive" than necessary. Safety first, folks!
c) Gold Chloride (AuCl3): Ah, the golden choice! While it might be glamorous to evaporate a solution of gold chloride, it would be quite expensive and completely unnecessary for this particular demonstration. We don't want to break the bank or steal the show, right?
d) Hydrogen Chloride (HCl): Evaporating a hydrochloric acid solution might not be the best idea, unless you're aiming for a lab that smells like a swimming pool on steroids. HCl is a bit too harsh and corrosive for our purposes, so it's best to keep it out of the equation.
Remember, sometimes the best choice is the one that combines safety, availability, and a touch of pizzazz!
To answer the questions, we can consider the properties of the different solutes mentioned and why sodium chloride may have been chosen for the experiment.
1) Sodium chloride is commonly chosen as a solute for various experiments due to several reasons:
- High solubility: Sodium chloride is highly soluble in water, meaning it easily dissolves in water to form a saturated solution. This property allows for the concentration of the solution to be controlled reliably during the process of evaporation.
- Safety: Sodium chloride is a relatively safe and commonly used compound. It poses minimal health risks when handled properly, making it suitable for educational and laboratory experiments.
- Availability and cost-effectiveness: Sodium chloride is readily available in large amounts and is relatively inexpensive compared to other solutes. This accessibility and affordability make it a practical choice for laboratory experiments.
2) Let's explore the reasons why the other substances were not chosen as the solute:
a) Calcium carbonate (CaCO3): Calcium carbonate is not an ideal solute for evaporation experiments because it has low solubility in water. It does not dissolve as easily as sodium chloride, resulting in limited control over the concentration of the solution. Therefore, it may not provide consistent results for the demonstration of the evaporation process.
b) Sodium Cyanide (NaCN): Sodium cyanide is a highly toxic compound that poses serious health risks, even in small amounts. Due to its toxicity, it is generally not recommended for use in educational or experimental settings, unless under strict supervision and safety protocols.
c) Gold Chloride (AuCl3): Gold chloride is a compound that contains the valuable metal gold. As it is costly and precious, it is unlikely to be used as a solute for educational or demonstration purposes. Additionally, gold chloride may have different chemical behaviors compared to sodium chloride, which could affect the results and objectives of the experiment.
d) Hydrogen Chloride (HCl): Hydrogen chloride is a strong acid that should be handled with caution due to its corrosive and toxic nature. Using it as a solute for evaporation experiments may create safety concerns and may not align with the purpose of the demonstration, which is usually to showcase the evaporation process rather than the properties of acids.
In summary, sodium chloride is commonly chosen as a solute for demonstrating the evaporation process due to its high solubility, safety, availability, and cost-effectiveness. Other substances such as calcium carbonate, sodium cyanide, gold chloride, and hydrogen chloride were likely not chosen for various reasons, including low solubility, toxicity, high cost, or safety concerns.