Hi! I am doing this chemistry lab of solubility curve of a solid investigation and this is for KCl.

The purpose of this lab is to investigate the relationship between the solubility of potassium chloride and the temperature of its solution and to create a solubility curve for an ionic solid.

There is two questions I do not understand...

1) What property of the solution is illustrated at the moment the crystals start forming explain briefly?

and for both of these questions I found a link:

h t t p : / / a w e s o m e n e s s . c a / h i g h s c h o o l / b i n / 1 1 % 2 0 C h e m i s t r y / S o l u b i l i t y % 2 0 C u r v e % 2 0 o f % 2 0 a % 2 0 S o l i d % 2 0 L a b % 2 0 R e p o r t . p d f

Both my questions are under analysis... # 4 and 5

Question 5 is )
According to your graph, which of the following mixtures is a saturated solution and which is an unsaturated solution;
1)100g of KCl in 100mL of H2O at 40°C
2)50g of KCl in 100mL of H2O at 70°C
3) 120g of KCl in 100mL of H2O at 60°C

The website I gave you is another person with the same assignment except it is of KNO3 whereas mine is KCl...I just want to know what I should write for question 4 and for question 5 how do I basically find out if it is saturated or unsaturated...

Please help my lab is due tmw and I am completely clueless about these 2 questions..

I appreciate your time to my heart please help me:)

Thankyou!

Hello! I'll be happy to help you with your chemistry lab questions.

For question 4, "What property of the solution is illustrated at the moment the crystals start forming?", the property being illustrated is the saturation point of the solution. At the moment the crystals start forming, it indicates that the solution has reached its maximum solubility at that temperature. This means that any additional solute (KCl) added to the solution will not dissolve and will instead form solid crystals.

As for question 5, to determine whether a solution is saturated or unsaturated based on the given mixtures, you will need to compare the amount of solute (KCl) dissolved in each solution to its maximum solubility at the corresponding temperature.

To do this, you need to refer to the solubility curve for potassium chloride (KCl) at the given temperature range. Unfortunately, I cannot access the specific link you provided, but you can search for a solubility curve of KCl or refer to your textbook or class materials to find the information.

Once you have the solubility curve, you can compare the amount of KCl in each mixture to the maximum solubility of KCl at the respective temperature. If the amount of KCl in the mixture is less than the maximum solubility, then the solution is unsaturated because more solute can dissolve. If the amount of KCl in the mixture is equal to or greater than the maximum solubility, then the solution is saturated because no more solute can dissolve and any additional KCl will precipitate as crystals.

So, for each mixture:

1) Calculate the maximum solubility of KCl at 40°C and compare it to the amount of KCl (100g). If 100g is less than the maximum solubility, then the solution is unsaturated. If 100g is equal to or greater than the maximum solubility, then the solution is saturated.

2) Apply the same procedure for the mixture at 70°C, comparing the amount of KCl (50g) to the maximum solubility at 70°C.

3) Repeat the process for the mixture at 60°C, comparing the amount of KCl (120g) to the maximum solubility at 60°C.

Remember to consult the solubility curve to determine the maximum solubility of KCl at each temperature. Once you have compared the amount of KCl in each mixture to its maximum solubility, you can identify whether each mixture is saturated or unsaturated.

I hope this helps! If you have any more questions, feel free to ask. Good luck with your lab!