All AP Chemistry Resources
Example Questions
Example Question #1 : Yield And Error
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
Example Question #2 : Yield And Error
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
Example Question #1 : Drawing Conclusions From Observations
During lab you have a solution of 1M NaCl at room temperature. You accidentally add so much salt to the solution that you still see some at the bottom of the beaker no matter how vigorously you mix it. What conclusion can you arrive at based upon your knowledge of chemistry?
The saturation limit of the water for sodium chloride has been surpassed. This is a saturated solution.
The saturation limit of the water for sodium chloride has been surpassed. This is a unsaturated solution.
The large spill caused hydrophobic clusters of sodium chloride to form, preventing them from being dissolved.
The salt you spilled into the solution wasn't sodium chloride, but was magnesium chloride, which isn't soluble in water.
The sodium chloride that sank to the bottom is a special isotope that can't be solubilized.
The saturation limit of the water for sodium chloride has been surpassed. This is a saturated solution.
The addition of so much salt (NaCl) caused the water to reach its solubility limit for NaCl. This means that no matter how much more NaCl you add to that solution or how hard you stir, it will not dissolve, and will precipitate on the bottom of the beaker. This type of solution is saturated. If the solution were unsaturated, then more salt would still be able to dissolve.
There is no special isotope that makes NaCl insoluble in water. The vigorous mixing would have separated any clumps, and if the solution was unsaturated the salt would have eventually dissolved. Magnesium chloride, another salt, is very soluble in water and would not result in the scenario described.
Example Question #2 : Drawing Conclusions From Observations
There is a beaker full of a clear liquid on the counter. It was left unlabeled by your lab partner, and you are required to find out what it is. You perform a number of tests and observe the follwing results.
1. The liquid is miscible with water.
2. You add the liquid to 1M phosphoric acid. The beaker gets extremely warm.
3. You grab a piece of red litmus, and it turns blue upon exposure to the unknown liquid.
Which of the following could be the identity of the unknown liquid?
Each test gives us a different piece of information. The first test tells us that our compound is soluble in water. The second test tells us that heat is released when acid is added. The third test tells us that the solution turns red litmus paper blue, which means that the solution is basic. From these results, we can conclude that the compound is a water-soluble base. Now we can look at our answer options.
, , , and are all acids.
, however, will generate cyanide ions in solution. Cyanide is basic; thus, this is our correct answer.
Example Question #31 : Laboratory Techniques And Analysis
Using the target shown, determine whether the shots were accurate and/or precise.
Precise but not accurate
Precise and accurate
Accurate but not precise
Neither precise nor accurate
Precise but not accurate
The target is precise because the shots are closely grouped together. However, the shots are not accurate because they are not in the middle of the target.
Example Question #32 : Laboratory Techniques And Analysis
Using the target, determine whether the shots are accurate and/or precise.
Precise but not accurate
Accurate and precise
Neither accurate nor precise
Accurate but not precise
Accurate and precise
The target is accurate because the shots are all in the middle of the target. It is also precise because all the shots are grouped together.
Example Question #33 : Laboratory Techniques And Analysis
Using the target shown, determine whether the shots are accurate and/or precise.
Neither accurate nor precise
Accurate but not precise
Precise but not accurate
Accurate and precise
Accurate but not precise
The shots are not precise because they are not grouped together. However, one of the shots is in the center of the target, and thus is accurate.
Example Question #1 : Laboratory Equipment And Procedure
You have a stock solution of 12M HCl, but want to dilute it to 1M HCl. What is the safest way you could go about doing this?
Measure out the water first, then slowly add the correct amount of 12M HCl
Measure out the water first, then rapidly add the correct amount of 12M HCl
Measure out the 12M HCl first, then rapidly add the correct amount of water
Add the correct amount of water and 12M HCl to a common beaker at the same time
Measure out the 12M HCl first, then slowly add the correct amount of water
Measure out the water first, then slowly add the correct amount of 12M HCl
Always add acid to water. You should mix solutions slowly because you run the risk of solutions spilling, which may ruin your reaction entirely. Rapid mixing can also lead to inadvertently speeding up reactions and releasing energy or heat in a dangerous manner. During dilution of acids with, water heat is released; if a small amount of water is added to a concentrated acid it has the possibility of bubbling over the counter and onto you.
Example Question #2 : Laboratory Equipment And Procedure
Which procedure separates two substances using their different boiling points?
Dehydration
Fermentation
Filtration
Distillation
Hydration
Distillation
During the distillation process, the combined substances are heated until the first one boils. The substance that boils and becomes a gas is then separated from the still liquid or solid substance via condensation into a separate container. Filtration involves separating substances in solid and liquid phases through a filter paper, and is often facilitated by a vacuum. Dehydration and hydration are types of reactions where water is a product, and a reactant, respectively. Fermentation is a biochemical process that occurs under anaerobic conditions. Some organisms produce lactic acid as a byproduct of fermentation, (humans), others produce ethanol (yeast).
Example Question #1 : Laboratory Equipment
You are trying to create a new chemical structure. You need exactly 9mL of phenyllithium for your next reaction. Which measuring tool would be the most accurate to measure out that liquid?
100mL beaker
9mL watch glass
10mL syringe
9mL volumetric pipet
10mL graduated cylinder
9mL volumetric pipet
When measuring any liquid in the lab, a volumetric pipet or flask is always going to be the most accurate. This makes the 9mL volumetric pipet the best choice.
There is no such thing as a 9mL watch glass. Though a 10mL syringe and graduated cylinder would be quite accurate, the 9mL volumetric pipet is more accurate, and remember the question asked for the best out of the answer choices. A beaker is very inaccurate and should only be used to transfer solutions, not to measure them.