Category: Chemistry

Reflective Essay on Chapter 10 Acids and Bases and Chapter 11 Nuclear Chemistry

Posted on | by Kelvin

 

In a minimum of 200 words, reflect on the chapter content and answer the following questions:

Which concepts were easy to understand and why?
Which concepts were more difficult to grasp and why?
What did you do, specifically, to better understand those difficult concepts?
What, if anything, did you find helpful in the course that allowed you to understand those more difficult concepts?
Did you find any outside resources that helped you better understand the chapter material? Please share them.

https://docs.google.com/file/d/1q6Dgqb6v0cWLiCZ09CMYiA4CvVK2WZkD/edit?filetype=mspresentation
Chapter 10
https://docs.google.com/file/d/12_cZVuzSF43iMaHQnZi6O1GYxnK56reG/edit?usp=docslist_api&filetype=mspresentation
Chapter 11

 

The Importance of Safety in a Chemical Laboratory

Posted on | by Kelvin

Watch this video-“Safety Videos for Chemistry,” (
https://www.youtube.com/watch?v=SYpafHbYz0g&list=PLfSk-dHOm3SBv2Uhy8S1oEf6O04AGPSul) write a 1000-
word paper on the importance of safety in a chemical laboratory. Include a description of proper personal
protective equipment (PPE) that should be worn in the laboratory, the purpose of each PPE item, at least two
examples of potential hazards that students could face in a chemistry laboratory setting, and a brief description
on how a chemistry laboratory differs from biology or anatomy laboratory settings. Use APA format (1
additional source and youtube video).
What needs to be included?
-Discuss the importance of safety (provide a compelling argument on the importance of safety in a chemical
laboratory, including examples of dangers and what we do to mitigate them.)
-Full description of all PPE that should be worn in the laboratory is given, and purpose of each item is
thoroughly and correctly explained. Proper attire is addressed and integrated into the idea of PPE.
-Thorough explanation of two examples of potential hazards that students could face in a chemistry laboratory
setting are given.
-Lab differences – Thorough description given of differences between chemistry lab and an anatomy or biology
lab

The Role of Acids and Bases in Kitchen Foods

Posted on | by Kelvin

 

Acids and bases can be found in many places, including the kitchen. Acids like lemon juice can make foods taste sour. Basic or alkaline foods such as peas or almonds may have more of a bland taste. As we’ve learned this week, an acid donates a proton, and a base will accept a proton.
Choose three foods that you can find in your kitchen.
Describe how the food tastes, smells, and looks.
Using this week’s resource, what is the pH of the food you’ve consumed, and how do they contribute to the acidity or alkalinity of the body? Specifically, discuss an organ or system in the body. You should include outside resources and cite them according to APA.
Are there specific conditions that might benefit from consuming more acidic foods or alkaline foods?
Please be sure to validate your opinions and ideas with citations and references in APA format.

 

 

 

Basic atomic structure

Posted on | by Kelvin

Explain basic atomic structure.
Interpret the Periodic Table of Elements.
Analyze the principles of chemical reactions.
Apply the scientific method to experimental data.
Apply principles of measurement.
Questions
For each learning objective, provide an analysis of how the course supported each objective.
Explain how the material learned in this course, based on the objectives, will apply to your professional career.
Reflections
Reflect back on your journey through this course and answer the following:

What topic in the course did you find most interesting and applicable?
What are your thoughts on your learning in the course?
Please be sure to validate your opinions and ideas with citations and references

 

Acid, base, strong electrolyte, weak electrolyte, and nonelectrolyte

Posted on | by Kelvin

Question 1

Define and list an example of each of the following: acid, base, strong electrolyte, weak electrolyte, and nonelectrolyte. Explain why each of your examples matches the definition.

Question 2

In your own words, define and compare fission and fusion (be specific). Provide an example of each in your response.

Question 3

Scientific Method.
a. List the steps of the Scientific Method.
b. Create an example of a scientific study that could be done in terms of the steps of the scientific method. Be creative and describe the study in terms of the steps of the scientific method.

Question 4

What is the mass of sodium chloride used to create a 100 mL solution at a concentration of 1.5 M? Your solution must include a step-by-step solution with units included throughout to support your final answer.

Question 5

For the nitrite ion (NO2- ), identify:
a. How many total lone pairs are in the ion?
b. What is the VSEPR molecular shape of the ion?
c. How many resonance structures can be drawn from the ion?

Question 6

The density of table salt is 2.16 g/cm3. Detail the conversion into units of pounds per liter, and provide the density in lb/L. Your solution must include a step-by-step solution with units included throughout.

Question 7
Given the reaction between ammonia and oxygen as 4NH3 + 5O2 4NO + 6H2O:
a. Calculate the amount of nitrogen monoxide (in grams) produced if 0.5 g of ammonia is reacted.
b. Calculate the amount of nitrogen monoxide (in grams) produced if 0.5 g of oxygen is reacted.
c. In comparing (a) and (b), indicate what the limiting reactant is. Explain.
Your solution must include a step-by-step solution with units included throughout to support your answers.

Question 8

In using the following table, note which intermolecular attractive interactions are present for each of the following substances. For each interaction, explain why you selected it or why you did not. Be specific.

Substance Dispersion Dipole-dipole Hydrogen bonding Ion-dipole
CO2 (g)
NaCl(aq)
OF2 (g)

Question 9

As a birthday balloon is filled with helium, the amount of helium increases from 1.5 moles of helium to 9.5 moles of helium. If the initial volume of the balloon is 50.5 mL, what is the final volume? Your solution must include a step-by-step solution with units included throughout.

Question 10

The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 °C. The specific heat of this compound in the liquid state is 0.91 J/g-K and in the gas state is 0.67 J/g-K. The heat of vaporization is 27.5 kJ/mol. What is the amount of heat required to convert 5.6 g of the compound from a liquid at 30.0 °C to a gas at 60.5 °C? Your solution must include a step-by-step solution with units included throughout.

 

Percent error

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1. The vinegar bottle normally has a 5% concentration, which is the equivalent of 0.83 M. Find your percent error using the average experimental value that you calculated for vinegar. Comment on your results. (Less than 10% error is acceptable, more than that requires additional discussion.)

%error=|”actual value – experimental value” |/”actual value” ×100%

2. Using the Ka value for HC2H3O2 from the pre-lab, find the Kb value for this anion.
3. If you reverse the equilibrium reaction described in the pre-lab, you can set up an ICE table and solve for x = [OH-], and use that to determine the pH. Using the concentration you found in this lab as the initial concentration of C2H3O2-, calculate the hydroxide concentration and the pH at the equivalence point.
C_2 H_3 O_2^-+H_2 O↔〖HC〗_2 H_3 O_2+OH^-
4. How does this value compare to the pH value on your graph at the equivalence point?

 

 

 

Acid-Base titration

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1. Provide definitions for the following terms:
Acid-Base titration curve
Equivalence point
Weak acid
2. What is the name and formula for the acid titrated in this experiment? What is the Ka value for the weak acid from Appendix H in your textbook?
3. Use the calculation instructions in the introduction to solve the following titration example: A 5.0 mL sample of aqueous HNO3 requires 18.5 mL of 0.11 M NaOH to reach the equivalence point. What is the molar concentration of HNO3? The equation for the reaction is:
HNO_3+NaOH→NaNO_3+H_2 O
4. What safety rules must be observed during this experiment?

 

 

The different colors

Posted on | by Brian Leakey
  1. Use Le Chatelier’s principle to explain the different colors found in the following equilibria. (This means your explanation will say either reactant added, reactant removed, product added, product removed.)
  2. Show all chemical reactions.
    a.
    i. Which way does it shift when Fe3+ is added?
    ii. Explain why in terms of LeChatelier’s Principle.
    iii. Which way does it shift when SCN- is added?
    iv. Explain why in terms of LeChatelier’s Principle.
    b.
    i. Which way does it shift when NH3 is added?
    ii. Explain why in terms of LeChatelier’s Principle.
    iii. Which way does it shift when vinegar is added?
    iv. Explain why in terms of LeChatelier’s Principle.
    c.
    The formation of CoCl42- from Co2+ and Cl- is endothermic.
    i. Which way does it shift when HCl is added?
    ii. Explain why in terms of LeChatelier’s Principle.
    iii. Which way does it shift when Ag+ is added?
    iv. Explain why in terms of LeChatelier’s Principle.
    v. Which way does it shift when it is heated?
    vi. Explain why in terms of LeChatelier’s Principle.
    vii. Which way does it shift when it is cooled?
    viii. Explain why in terms of LeChatelier’s Principle.

Le Chatelier’s Principle

Posted on | by Brian Leakey
  1. Define the following terms:
    a. Chemical equilibrium
    b. Le Chatelier’s principle
  2. Write chemical equations that describe the three equilibria that you will observe during this experiment.
  3. Consider the hypothetical exothermic equilibrium reaction:
    A + B ↔ C + D + heat
    Which direction will the equilibrium shift under each of the following conditions:
    a. Either A or B is added to the equilibrium system: _
    b. Either A or B is removed from the equilibrium system: _
    c. Either C or D is added to the equilibrium system: _
    d. The equilibrium system is heated: _
    e. The equilibrium system is cooled: __
  4. What safety precautions need to be observed during this experiment?