Order ID | 53563633773 |
Type | Essay |
Writer Level | Masters |
Style | APA |
Sources/References | 4 |
Perfect Number of Pages to Order | 5-10 Pages |
Acidity of Common Household Products Experiment
Lab 4: Acids & Bases
Experiment: Acidity of Common Household Products
In this experiment, we will observe the neutraliza on of acids and bases using grape juice as an indicator. We will also test common household products for their acidity or alkalinity.
Procedure
Part 1: Acid‐Base Neutraliza on
Label three test tubes 1, 2, and Standard.
Prepare 50 mL of a 10% grape juice solu on by first pouring 5 mL of grape Juice into a 100 mL graduated cylinder. Add dis lled water un l the total volume of liquid is 50 mL. Mix well by s rring the solu on with a s rring rod.
Pour 10 mL of the dilute grape juice solu on into each test tube.
Note the color of the juice in the test tube labeled Standard in Table 2.
Using a pipe e, add 15 drops of saturated citric acid solu on into test tube 1. Record your observa ons concerning the color change in Ta‐ ble 2 of the Data sec on. Use the juice in the test tube labeled Standard for comparison.
Using a pipe e, add 15 drops of saturated sodium bicarbonate solu on into test tube 2. Record your observa ons concerning the color change in Table 2 of the Data sec on. Use the juice in the test tube labeled Standard for comparison.
Use pH paper to determine the pH of the solu on in each of the 3 test tubes. Record the pH val‐ ues in Table 2.
Using a pipe e, add drops of saturated sodium bicarbonate solu on to test tube 1 un l it re‐ turns to its original color. Record your observa ons in Table 3.
Materials Safety Equipment: Safety goggles, gloves Vinegar Household ammonia **Grape Juice 3 test tubes pH strips Saturated citric acid solu on (60% Test tube rack Neutral litmus paper
Saturated sodium bicarbonate solu‐ on (15%)
(2) 50 mL beakers Tomato juice Sodium bicarbonate 12‐well plate Powdered milk Lemon juice 10 Droppers (pipe es) Baking soda Dishwashing liquid
S rring rod 100 mL Graduated cylinder *Dis lled water
*You must provide **Used in the next lab— refrigerate a er opening
HINT: If the grape juice
is not dilute enough or
the base is not as
strong as needed, you
may con nue adding
drops of base.
55
Lab 4: Acids & Bases
Using a pipe e, add drops of saturated citric acid solu on to test tube 2 un l it returns to its original col‐ or. Record your observa ons in Table 3.
Use pH paper to test the pH of the three solu ons. Record the pH values in Table 3.
Part 2: Tes ng acidity and basicity of common household products
Use the pipe es to place into different wells of your 12‐well plate a couple of drops of each of the fol‐ lowing items: tomato juice, household ammonia, milk (mix powdered milk with 50mL water un l dis‐ solved), vinegar, lemon juice, and diluted dishwashing liquid (mix 1mL dishwashing liquid with 5mL wa‐ ter). Be sure to label or write down where each item is located in the 12‐well plate. CAUTION: Do not contaminate the items being tested. Be sure to use only a clean pipe e for each item.
Guess the pH of each of the items before you find the experimental value and record your guess in Table 4.
Test each item with litmus paper and pH paper. Record your results in Table 4.
To clean up rinse all chemicals into a waste beaker. Neutralize the waste to a pH between 4 and 8 using either baking soda or vinegar. Wash the waste solu on down the drain.
Data
Please submit your table data and answers for this experiment on the Word document provided to you.
Table 2: Acid‐Base Neutraliza on for Part 1, Steps 5 & 6 Table 3: Acid‐Base Neutraliza on for Part 1, Steps 8 & 9
Test tube 1 Test tube 2 Standard
Step 1 Add acid Add base Neutral
Color
pH value
Test tube 1 Test tube 2 Standard
Step 1 Add base Add acid Neutral
Color
pH value
Table 4: Acidity and basicity tes ng for household products data
Product Hypothesized pH Color of Litmus
Paper Color of pH Paper Actual pH
56
Lab 4: Acids & Bases
Ques ons
Why did the grape juice change color when an acid or base was added?
You added a base, sodium bicarbonate, to test tube 1 that contained citric acid and an acid to test tube 2 that contained base. Why did the grape juice return to its original color?
Name two acids and two bases you o en use.
Lab 5: Chemical Processes
59
Lab 5: Chemical Processes
Introduc on
Have you ever needed to place a cold pack on a sprained muscle?
It’s the final seconds of the community league champion‐ ship basketball game, and your team is behind by one point. One of your team’s players takes a shot and scores. The game is over, and your team won! But something is wrong: the player is si ng on the floor, and appears to be in a lot of pain. The coach quickly brings a cold pack to the player, squeezes it, and places it on the swelling ankle. The bag immediately becomes cold—but how?
Though we o en use them interchangeably, heat and tem‐ perature have different defini ons—though they are close‐ ly related in the study of thermodynamics. Heat is the transfer of energy from one object to another due to a difference in temperature. Temperature, on the other hand, describes how much energy the atoms and molecules in a sub‐ stance have. This energy, o en called internal energy, describes how quickly the atoms or molecules in a substance move or vibrate around. When an object gains heat its molecules vibrate with more energy, which we can sense or measure as an increase in temperature. When you touch a hot object, it feels hot because a heat moves from the hot object (higher energy) to your skin (lower energy). Similarly, an object feels cold when heat is lost by your hand and gained by the cold object. Heat always transfers in the direc on of high temperature to low temperature—high energy to low energy.
Both physical processes and chemical reac ons can release or absorb energy in the form of heat. When a reac on or phys‐ ical change gives off energy it is called an exothermic process. To remember exothermic, think of ‘exi ng’ as in leaving or going out. An endothermic process does just the opposite—it takes in energy from its surroundings. The generalized chemical equa ons for exothermic and endothermic reac ons are:
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