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Mountain Kilimanjaro is very amazing one in East Africa did you know?

From Le Chatlier's Principle Equilibrium Lab

Fill a second cuvette about ¾ full with 0.10 M Co(NO3)2 .6H2O.

Prepare 100 mL of a 0.010 M Co(NO3)2 . 6H2O solution. Add exactly 10.0 mL of 0.10 M Co(NO3)2 .6H2O to a 100 mL volumetric flask and dilute with deionized water to the mark.

5. Use the 10.0 ml graduated cylinder to prepare a solution of [C oCl4]2-. To the 10 mL graduated cylinder add 1.0 mL of 0.010 M Co(NO3)2 * 6H2O (prepared in step 4). Carefully pipette 4.0 mL of 12 M HCl into the graduated cylinder so that the total volume is 5 mL.

With this information, I have to calculate the concentration of Co(NO3)2. 6 H2O and do not know how. Thank you.

I need the last three questions answered at bottom of page!!!

The Base Hydrolysis
of Ethyl Acetate

The reaction of ethyl acetate and hydroxide ions yields ethanol and acetate ions, as shown below.

CH₃COOC₂H₅ (aq) + OH^– (aq) → CH₃CH₂OH (aq) + CH₃COO^– (aq)

The progress of this reaction can be observed by monitoring the conductivity of the reaction mixture. Although the reactants and products each contain an ion, the OH^– ion has a higher ionic mobility than the CH₃COO^– ion. This results in a net decrease in the conductivity of the reaction mixture as the reaction proceeds.

Ethyl acetate is the major active ingredient in commercial acetone-free, nail-polish removers. The molar concentration of CH₃COOC₂H₅ in this product is 0.10 M. You can successfully use one of these over-the-counter products in this experiment. The primary objective of this experiment is to conduct a series of reactions from which you will determine the rate law expression for the base hydrolysis of ethyl acetate.

OBJECTIVES

In this experiment, you will

Conduct the base hydrolysis of ethyl acetate under various conditions.

Calculate the rate law constant, k, for the reaction.

Determine the rate law expression for the reaction.

Figure 1

MATERIALS

PROCEDURE

1. Obtain and wear goggles.

2. Connect a Conductivity Probe to Channel 1 of the Vernier computer interface. Connect the interface to the computer using the proper cable.

3. Set the toggle switch on the Conductivity Probe to the 0–2000 μS/cm range.

4. Start the Logger Pro program on your computer. Open the file “29 Ethyl Acetate” from the Advanced Chemistry with Vernier folder.

5. Obtain the materials you will need to conduct this experiment.

Two 50 mL graduated cylinders

One 10 mL graduated cylinder

100 mL beaker in which to conduct the reaction

Approximately 90–100 mL of 0.010 M NaOH solution in a 250 mL beaker

Approximately 10 mL of 0.10 M CH₃COOC₂H₅ solution in a second 100 mL beaker

Distilled water (75-80 mL)

6. During the experiment you will conduct three trials. This step describes the process for conducting Trial 1. When you repeat this process, use the correct volumes for each trial based on the table below.

Use a utility clamp to connect the Conductivity Probe to the post of a Stir Station or a ring stand as shown in Figure 1.

Measure 20.0 mL of NaOH solution and 28.0 mL of distilled water into a 100 mL beaker. Carefully place a stirring bar in the beaker of solution. Place the beaker on the platform of the Stir Station, or on the magnetic stirrer.

Position the Conductivity Probe in the 100 mL beaker so that the opening near the tip of the probe is completely immersed in the solution and the stirring bar will not strike the probe. Record the initial conductivity of the NaOH solution in your data table, but do not start the data collection.

Turn on the Stir Station to setting 5 or 6 (moderate stirring, small vortex).

Measure out 2.0 mL of CH₃COOC₂H₅ solution.

Click to begin data collection. Add the 2.0 mL of CH₃COOC₂H₅ solution to the beaker of NaOH solution. Data will be collected for five minutes.

7. When the data collection is complete, dispose of the contents of the beaker as directed. Rinse and clean the beaker and the Conductivity Probe for the second trial.

8. Examine the graph of your data. The graph will show a gradual, nonlinear, conductivity decrease. Click and drag the cursor across a linear section of the graph over 20–30 s during the first minute. Click on the Linear Regression button, , to calculate the best-fit line equation. Record the slope, in your data table, as the initial rate of the Trial 1.

9. Repeat Steps 6–8 to conduct Trials 2 and 3.

DATA TABLE

DATA ANALYSIS

1. What is the order of the reaction in sodium hydroxide and ethyl acetate? Explain how you determined order for each reactant.

2. Write the rate law expression for the reaction.

3. Convert conductivity to molar concentration by using the initial conductivity of the NaOH solution as a conversion factor. Convert each initial rate into the units: moles/L/s. For example, if the initial conductivity of the NaOH solution was 2000 μS/cm and initial rate was 5.0 μS /cm/s, you would convert the rate to moles/L/s by completing the following calculation: Rate = 5.0 μS/cm/s ´ [(0.005 mol/L)/(2000 μS/cm)] = 1.25 ´ 10^–5 mol/L/s. Use these new values to calculate the rate constant, k.

Can you solve the last four questions?

Can you solve the last questions?

1. Concentrations of acetic acid and sodium acetate in the prepared buffer solutions in Part I as noted in the table in the lab handout

The acetic acid and sodium acetate solutions will have concentrations of 0.50 M.

2. Theoretical pH of prepared buffer solutions in Part I

There are 0.10 M aqueous solutions of HCl and NaOH available in the lab for this part of the experiment.

3. Theoretical pH of solutions and deionized water after the addition of strong acid and strong base in Part II of the experiment.

Measure 20 mL of buffer solution A using a graduated cylinder and pour the solution into a clean beaker labeled A1. Measure 20 mL of buffer solution B using a clean graduated cylinder and pour the solution into a clean beaker labeled B1. Measure 20 mL of the deionized water sample from part I and pour the solution into a clean beaker labeled W1.

3. Using a clean graduated cylinder, add 10 mL of 0.10 M HCl (aq) to each solution A1, B1 and W1. Mix the solutions well using a glass stir rod making sure to rinse the stir rod in between mixing each solution. Measure and record the pH of all 3 solutions in your notebook.

4. Measure 20 mL of buffer solution A using a graduated cylinder and pour the solution into a clean beaker labeled A2. Measure 20 mL of buffer solution C using a clean graduated cylinder and pour the solution into a clean beaker labeled C2. Measure 20 mL of the deionized water sample from part I and pour the solution into a clean beaker labeled W2.

5. Using a clean graduated cylinder, add 10 mL of 0.10 M NaOH (aq) to each solution A2, C2 and W2. Mix the solutions well using a glass stir rod making sure to rinse the stir rod in between mixing each solution. Measure and record the pH of all 3 solutions in your notebook.

For the buffer we prepared in the procedure, when the buffering effect fail? (Hint: This is equivalent to asking when will we exceed the buffer's capacity?)

Buffers:
A total of 100 mL of 1.0 M HCL Is added in 10 mL increments to 100 mL of the following solutions:
1. Pure water where pH=7 (unbuffered)
2. A solution containing 1.0 M HA, 1.0M A-. Where pKa=7.0.(buffered)
Determine pH for both solutions after each 10 mL addition of HCl.

Part A: Determine the initial pH of a 100mL buffered solution containing 0.1 M H2PO4^- and 0.063M HPO4 ^-2. (pKa=7.2)

(B) Calculate the pH of the buffered solution when 1.0 * 10^-3 mols of HCl are added.

C) what would be the change if the same amount of HCl were added to 100mL of pure water.

please show all steps.

Please answer the following questions regarding the nature of buffers:

Part 1: A few drops of 1.0 M HCl are added to pure water and to a buffered solution containing hydrogen phosphate (HPO42-) and dihydrogen phosphate (H2PO4-). You observed that the pH of the pure water drops significantly, while the pH of the buffered solution only decreases slightly. Which explains the result?

A) H2PO4- reacted with the HCl, changing to HPO42- and removing H+ from solution

B) HPO42- reacted with the HCl, changing to H2PO4- and removing H+ from solution

C) H2PO4- reacted with the HCl, changing to H3PO4 and removing H+ from solution

Part 2: A few drops of 1.0 M NaOHl are added to pure water and to a buffered solution containing hydrogen phosphate (HPO42-) and dihydrogen phosphate (H2PO4-). You observed that the pH of the pure water increases significantly, while the pH of the buffered solution only increases slightly. Which explains the result?

A) HPO42- reacted with the NaOH, changing to H2PO4- and removing OH- from solution

B) HPO42- reacted with the NaOH, changing to PO43- and removing OH- from solution

C) H2PO4- reacted with the NaOH, changing to HPO42- and removing OH- from solution

Part 3: You begin with 43 mL of the buffered solution. If the solution is 1.0 M H2PO4- and 0.5 M HPO42-, how many mL of the 1.0 M solution of HCl would be needed to 'overwhelm' and completely react with the buffer?

Part 4: You begin with 43 mL of the buffered solution. If the solution is 1.0 M H2PO4- and 0.5 M HPO42-, how many mL of the 1.0 M solution of NaOH would be needed to 'overwhelm' and completely react with the buffer?

Part 5: Buffers are solutions that can accept protons in the presence of a base and donate protons in the presence of an acid. Which of these would be able to function as a buffer?

A) Weak Acid + Weak Base

B) Weak Acid + Strong Acid

C) Weak Base + Strong Base

D) Strong Acid + Strong Base

Part 6: Buffers are defined as a solution containing one of the following:

1)A weak acid and that weak acid’s conjugate base

2)A weak base and that weak base’s conjugate acid Which of the following solutions would form a buffer? Select all that apply.

A) NH3 + NH4+

B) HF + F-

C) NH3 + NaOH

D) HF + HCl

E) OH- + H+

pH Shift

Unbuffered Buffered

Acid added to acidicsolutions: Solution 2: -2 Solution 5: 0

Base added to acidicsolutions Solution 2: 0 Solution 5: 0

Acid added to basicsolutions Solution 3: 0 Solution 6: 0

Base added to basicsolutions Solution 3: +2 Solution 6: 0

Acid added to nearly neutral solutions Solution1: -1 Solution 4: 0

Base added to nearly neutral solutions Solution 1: +1 Solution 4: 0

1. Which of the unbuffered solutions, 1,2 or 3, was the mostsubject to pH change? Explain why.

2. What concluding statement can you make, on the basis of yourobservations regarding the fluctuations in pH for buffered andunbuffered solutions when small amounts of acid and base areadded?

We have learned about 8 different factors that influence our food choices in our class (ex. Nutritional, Family/Social, etc.). Answer the following questions:

What is your most influential factor? 

Why is it the most influential factor for you?

Explain using details and examples. 

Critique the Gender based sexual harassment under RA11313 in 100 words

What kind of an argument does Reagan pose in the following excerpt from Sec. 11 of "A Time for Choosing"?'

"Now, we have no better example of this than government's involvement in the farm economy over the last 30 years. Since 1955, the cost of this program has nearly doubled. One-fourth of farming in America is responsible for 85 percent of the farm surplus. Three-fourths of farming is out on the free market and has known a 21 percent increase in the per capita consumption of all its produce."

A.  Reagan uses opinion: "3/4ths of farming is out on the free market." B.  Reagan uses opinion: "Since 1955, the cost of this program has doubled." C.  Reagan uses opinion: "1/4th of farming in America is responsible for 85% of the farm surplus." D.  Reagan uses fact: "1/4th of farming in America is responsible for 85% of the farm surplus."

What is 5 + 5?

Critique the Gender based sexual harassment under RA11313 in 100 words.

The Devon Motor Company produces automobiles. On April 1, the company had no beginning inventories, and it purchased 6,730 batteries at a cost of $115 per battery. It withdrew 6,200 batteries from the storeroom during the month. Of these, 100 were used to replace batteries in cars being used by the company’s traveling sales staff. The remaining 6,100 batteries withdrawn from the storeroom were placed in cars being produced by the company. Of the cars in production during April, 90 percent were completed and transferred from work in process to finished goods. Of the cars completed during the month, 30 percent were unsold at April 30.

Required:

1. and 2. Determine the cost of batteries that would appear in each of the following accounts on April 30 and select whether each of the accounts would appear on the balance sheet or on the income statement.

What you know about RA 11313?

What you want to know about RA 11313?

What you have learned about RA 11313?

In 2001, Fund Company purchased three pieces of equipment. The equipment is used for different purposes and hence different methods of amortization have been selected. Information concerning the equipment is summarized below: For the declining balance method, Fund Company uses the double-declining rate. For the units-of-activity method, total machine hours are expected to be 30,000 hours. Actual hours of use in the first three yoars were: 2001,1,500;2002,4,800; and 2003,6,000. Instructions (a) Calculate the amount of accumulated amortization on each machine at December 31, 2003. (Round your answer to the nearest dollar.) (b) Early in 2003, the company reviews the remaining useful life and residual values for the machines. The useful life for Machine 1 is now expected to be a total of eight years. The residual value of machine 2 is revised to $20,000 and the total machine hours for Machine 3 is revised to 40,000 . What would be the amortization expense for the machines in 2003 ? (Hint: you have to calculate the balance left to be amortized and the remaining useful life; e.g., for machine 3 the number of hours expected excluding the first two years.) (Round your answer to the nearest dollar.)

Cite 5 ways how NORSU can promote . REPUBLIC ACT No. 11313. Use 200 words

Cite 5 ways how NORSU can promote.

REPUBLIC ACT No. 11313 or The Safe Spaces Act (Bawal Bastos Law) Use 200 words

What is a good estimate for the mass of a goat?

A company borrows $130000, which will be paid back to the lender in one payment at the end of 5 years. The company agrees to pay monthly interest payments at the nominal annual rate of 12% compounded monthly. At the same time the company sets up a sinking fund in order to repay the loan at the end of 5 years. The sinking fund pays interest at an annual nominal interest rate of 4% compounded monthly. Find the total amount of the monthly payments, that is, the sum of the interest payment and the sinking fund payment.
Total monthly payment

A company borrows $150000, which will be paid back to the lender in one payment at the end of 5 years. The company agrees to pay yearly interest payments at the nominal annual rate of 6% compounded yearly. At the same time the company sets up a sinking fund in order to repay the loan at the end of 5 years. The sinking fund pays interest at an annual nominal interest rate of 1% compounded yearly. Find the total amount of the yearly payments, that is, the sum of the interest payment and the sinking fund payment. Total yearly payment = $