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13 Dec 2019

1. Determine the volume of 0.097 M NaOH required to titrate a 325mg aspirin tablet if the aspirin was pure acetylsalicylicacid?
Answer with units and to 3 significant figures.

2. Suppose you get the same data that you recorded in your lab butyou mistakenly thought the mol ratio of acetylsalicylic acid:NaOHwas 2:1 respectively. How would your percent acid in aspirincompare?
a) You would get the percent acetylsalicylic acid in aspirin thatis lower than that of your current answer.
b) You would get the percent acetylsalicylic acid in aspirin thatis the same as your current answer.
c) You would get the percent acetylsalicylic acid in aspirin thatis higher than that of your current answer. .

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

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3.Convert the numerical value of the density in question 2 from units of grams per cubic centimeter (g / cm3) to milligrams per milliliter (mg / mL). Note:

-there are 1000 milligrams in a gram.

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Keep the new density to the same significant figures as you reported in question 2

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6.A brand of aspirin claims to contain 325 mg (1 g = 1000 mg) of aspirin per tablet. In addition to pure aspirin, a tablet also contains a non-active filler. We assume that the tablet contains only these two components: aspirin and filler. If a single tablet weighs 1.17 g, calculate the percent filler. Hint: calculate percent aspirin FIRST using the formula

% aspirin = [ (mass aspirin รƒยท mass tablet) x 100], the find % filler. When using this formula, make sure the masses of aspirin and tablet have the same units.

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Give a possible value for the density of nylon, including the correct units. Explain your answer briefly.

9.A procedure similar to that used in Lab 3 was performed to find the density of cyclohexane, which has an actual density of 0.779 g/mL, Due to poor lab technique, an experimental density of only 0.663 g/mL is found. Calculate the percent error for the density. Give your answer to the correct number of significant figures.

10.Two white powders are given to you. One is pure sodium bicarbonate, and the other is baking powder (a mixture of sodium bicarbonate and a weak acid like citric acid). Which single test (NOT counting the visual examination with a hand lens) used in Lab 3 allows you to distinguish sodium bicarbonate from baking powder? Explain your answers completely.

11.Gold has a specific heat of 0.129 J/goC. If a piece of gold (initially at 10.0oC) is dropped into hot water, the final temperature of both the gold and the water is measured as 70.9oC. If it is known that 4560 J of heat transferred from the hot water to the gold, what is the mass of the piece of gold in grams? Give your answer to the correct number of significant figures.

12.It is stated in the Introduction to Lab 4 that qwater = -qmetal. This equation means that if a hot piece of metal is placed in water, the amount of heat given off by the metal is exactly equal to the amount of heat absorbed by the water. However, this equation is not always accurate, because not all of the heat from the metal necessarily goes to the water. Where else can some of the heat go if it is not absorbed by the water?

13.A certain brand of breakfast cereal claims to have 100 Calories per 28 gram serving. 150.0 grams of cereal are burned using a procedure similar to that used in Lab 4. How many calories of heat are released? Note 1 food Calorie (capital C) = 1000 heat calories (lower case c)

14.The oxalate anion C2O42- is found in many dark green vegetables, including spinach, swiss chard, and collard greens. When cations react with oxalate, the resulting ionic compounds are insoluble in water except Group I A oxalates (e.g. compounds of lithium, sodium, potassium, etc. and oxalate) and ammonium oxalate (NH4)2C2O4. These exceptions are soluble in water.

15.Spinach leaves are cut into small pieces, mashed with small amounts of boiling water, and filtered through filter paper to remove the insoluble spinach material. The resulting aqueous extract contains the oxalate anion.if a small amount of the spinach extract is mixed with a small amount of a calcium acetate solution, Ca(C2H3O2)2(aq), what do you expect will be observed?

16.If a small amount of the spinach extract from question 16 is mixed with a small amount of a potassium acetate solution, KC2H3O2(aq), what do you expect will be observed?

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The standardized NaOH solution was used to titrate vinegar samples. The vinegar was delivered from a 5.00 mL transfer pipet and diluted with water. The results of three titrations are given in the table below:

RUN 1 RUN 2 RUN 3
Volume of Vinegar (mL) 5.00 5.00 5.00
Volume of Water added (mL) 45.0 45.0 45.0
Initial NaOH Buret reading (mL) 2.98 0.89 1.17
Final NaOH Buret reading (mL) 22.81 20.91 21.13

Pay close attention to the significant figures in the calculations involving the vinegar analysis!

Question 7

What is the concentration of acetic acid determined in Run 1?

Enter Your Answer:

Question 8

What is the concentration of acetic acid determined in Run 2?

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Question 9

What is the concentration of acetic acid determined in Run 3?

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Question 10

What is the average concentration of acetic acid for the three runs ?

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Question 11

What is the average deviation of the concentration of acetic acid?

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Question 12

What is the percent deviation of the concentration of acetic acid?

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Question 13

Would changing the volume of distilled water added to the vinegar samples before titrating have changed the concentrations of acid that you determined?

A. Yes

B. No

C. It is not possible to tell from the data given

Enter Your Answer: A B C

Question 14

If the actual concentration of acetic acid was 0.419, what is the percent deviation of the average result from the actual concentration?

Enter Your Answer:

Question 15

The pH of a sample of the undiluted unknown vinegar solution is measured to be 2.53. What is the pKa of the acetic acid?

Enter Your Answer:


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