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I am looking for a solution for problem number 13 in chapter 15 inthis book
General Chemistry Principles and Modern Applications(9th)


I have found the solution but it was not completed. So, can someone help me and sove it

you can see it from this link that the solution for the problemis incomplete

http://www.cramster.com/solution/solution/899755

I took a picture for the problem from my book and this is it

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Related questions

I am having trouble with absorbance and conentration. can someone help me with this homework question? if you could explain each step so that I conuld do it again on my own that would be fantastic. THANKS!

4. You make the following 5 CuSO4 * 5H2O solutions using a 100.00 mL volumetric flask and the data given in the table below.

a. calculate the molarity of each solution

b. using the equation, calculate the absorbance for each solution A=-log(%T/100)

c. use excel to create a calibration curve (a graph of absorbance vs concentration), for this data set. Keep in kind the concentration is the independent variable and the absorbance is the dependant. include the equation for the linea nd R2 value on the graph as well as all exes labels and graph title. attach graph to assignment

d. write your equation for your linear regression and R2 value from your graph in the previous problem.

e. using your calibration curve, calculate the number of grams used to make a 1000.0 ml solution of CuSO4 * 5H2O if the absorbance of this solution was found to be 0.0643.

f. could this calibration curve be used to determine the absorbance of 6.45 x10^3M CuSO4 * 5H2O. Why or why not?

Please see the information I’ve provided in bold, then fill in the blanks below #11 (A-G and the following questions). This is not a long question - I only need a few things answered, and all the information you need is here. I am just struggling with what is the "strong acid" and what numbers to put in for pH. Thanks!

Select 4 250-mL Erlenmeyer Flasks from the pictorial or equipment menu. Keep track of which one is which.

Click on the first flask and add 100 mL of distilled water to it. Click on the second flask and add 100 mL of distilled water to it.

Click on the third flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the third flask. Finally add 26.0 mL of distilled water to the third flask. Stir the solution.

Click on the fourth flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the fourth flask. Finally add 26.0 mL of distilled water to the fourth flask. Stir the solution.

Right click on each of the flasks and choose pH meter. The pH of each solution should appear in blue below the flask.

Record the pH of each solution on a separate WORD document.

My recordings: pH = 7. 2) pH = 7. 3) pH = 5.0127. 4) pH = 5.0127

Add 5.0 mL of HCl to the first flask. Record the pH on the Report sheet. pH 2.3222

Add 5.0 mL of NaOH to the second flask. Record the pH on the Report sheet. pH 11.6778

Add 5.0 mL of HCl to the third flask. Record the pH on the Report sheet. pH 4.9679

Add 5.0 mL of NaOH to the fourth flask. Record the pH on the Report sheet. pH 5.0590

A. Preparation the buffer solution:

initial pH of buffer solution: ____

B. Titration of a weak acid with a strong base:

initial pH of weak acid: ____

final pH of weak acid: ____

Amount of NaOH added: ____

C. Titration Curve for Weak Acid with a Strong Base

(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)

D. Titration of buffer with a strong base:

pH of buffer solution: ____

Amount of NaOH added: ____

E. Titration Curve for Buffer with a Strong Base

(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)

F. Titration of the buffer with a strong acid:

pH of buffer solution: ____

Amount of HCl added: ____

G. Titration Curve for Buffer with a Strong Acid

(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)

Questions:

What conclusions can you draw from looking at the titration curve of the weak acid with a strong base and comparing it to the titration curve for the buffer with a strong base?

What conclusions can you draw from looking at the titration curve of the buffer with a strong base and comparing it to the titration curve for the buffer with a strong acid?

Could someone please help me with this chemistry problem? Thank you!

After performing a titration using 20 mL of unknown weak acid with 0.3830M NaOH, I obtained the following results:

0 mL added NaOH = pH 3.80

Final amount of added NaOH = 8.59 mL = pH 12.20

At Equivalence Point: Volume of NaOH = 4.835 mL; pH = approx 8.40

At the Halfway Point; Volume of NaOH = 2.418 mL: pH = 5.15

Ka = 7.08 x 10^-6

Initial [HA] = 0.0926M (determined by M1V1=M2V2 at the equivalence point)

Molar Mass = 1079.8 g/mol (determined by using original mass 1.9977 g/1.85 x 10^-3 moles

-----------------------------------------------------------------------------------------------------------------------------------------------

Now I am asked the following questions in order to check my results for consistency;

Using your experimental Ka value, the concentration of your unknown acid solution and the concentration of the standardized NaOH solution, CALCULATE the pH of the following points on your titration curve:

1) The beginning of the titration before any any NaOH was added

2) 25% of the way to the equivalence point (25% of 4.835 mL is 1.21 mL)

3) 75% of the way to the equivalence point

4) The equivalence point (remember, this is found using Ka and concentrations of acid and base)

5) 20% of the way to the equivalence point (1.20 x 4.835= 5.80 mL)

I've found some info on the internet that says when in the buffer region, the moles of A- = moles of base added and that moles of HA = original moles of HA - moles of base added. Where I got confused was when the equilibrium expression was written as Ka = [H+] [mols Base Added/Volume] ÷ [mols Acid Left/Volume]. I don't know what volumes to use because I always think it makes more sense to use total volume of acid plus base mL's. But maybe you are supposed to use only the volume of each (acid/base) separately, in which case I think the volume of acid would be 20 mL. Maybe this is a totally wrong way to do it- I don't know! Please Help!!!!

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