# View the step-by-step solution to: A. How does the saturation point for salt you discovered in the

A. How does the saturation point for salt you discovered in the lab compare to the solubility of salt in the chart? Is it the same or different? What is the difference?
B. What would the concentration of the solution be, using 100g of sugar and 200 ml of water at 0 degrees Celsius?
C. Would a solution of 138 g of ammonia in 150 ml of water be saturated, unsaturated or super saturated?

Guiding Question: What factors may affect the rate that a solute dissolves?
Hypothesis: I think that how quickly a substance dissolves in a solvent is unknown. A teaspoon
of table sugar will dissolve rapidly in a hot drink. The same amount of sugar will take much
more time to dissolve in a glass of ice water. Similarly, table salt dissolves rapidly in water at
room temperature. Large pieces of salt, like those used in home water softeners, dissolve much
more slowly, which makes this type of salt ideal for use over long periods. The rate of dissolving
is affected by three main factors:
1. Stirring
2. Temperature
3. Particle Size
Guiding Question: Is there limit where a solution can’t dissolve any more solute?
Hypothesis: No, there is no limit of solute in the solvent.
Guiding Question: Will the same amount of solute dissolve in different types of solvents?
Hypothesis: Yes I think so, for example sugar can dissolve in warm milk.
Materials: Graduated Cylinder, Balance Beam, tsp. measurers, Fine Salt, Small Beakers, Large
Beakers, Stir Sticks
Procedure:
1. Use the balance to determine the mass of an empty glass dish. Measure 1 tsp of salt into
the dish. Record the new mass. Subtract the two values to determine the mass of 1 tsp of
salt.
2. Use the graduated cylinder to measure 100 ml of water. Pour the water into your beaker.
3. Pour 1 tsp of salt into your beaker of water. Stir with the stir stick until the salt dissolves.
Put a second tsp of salt into the water. Stir until it dissolves. Continue to add salt into the
beaker until it is impossible to dissolve any more salt. Make sure that each spoonful is
fully dissolved before you add the next one.
Caution: Make sure that you keep count of how many tsp of salt you put in the solution.
Make sure that each spoonful is holds the same amount. Your goal is to calculate the mass
of salt that 100 ml of water can dissolve.
4. Multiply the mass of salt by the number of spoonfuls you dissolved to determine the total
mass of salt dissolved. If your final spoon was not completely used, make an estimation
Questions:
1. What does “Agitation” mean?
2. What does Saturation mean? What was the conception of your solution at its saturation
point?
Saturation: The state of a physical system, such as a solution, containing as much of
another substance, such as a solute, as is possible at a given temperature or pressure.

3. Should the saturation point always be the same for the same solute and solvent, or should
4. Should the saturation point be the same if you changed the solvent? Again, think about
the Particle Theory.
5. What combination of factors would make a solute dissolve the fastest?
6. Using the solubility chart, answer the following questions:
A. How does the saturation point for salt you discovered in the lab compare to the
solubility of salt in the chart? Is it the same or different? What is the difference?
B. What would the concentration of the solution be, using 100g of sugar and 200 ml of
water at 0 degrees Celsius?
C. Would a solution of 138 g of ammonia in 150 ml of water be saturated, unsaturated or
super saturated?

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