Question

what is the [H+] (and its error) of a solution of HCl that is prepared by...

what is the [H+] (and its error) of a solution of HCl that is prepared by using a 2mL volumetric pipet (tolerance +/0.01mL) of standardized HCl(0.02050+-0.00005 mol/L) and diluting to the mark with ddH2O in a 10mL volumetric flask (Tolerance +/0.02mL)

0 0
Add a comment Improve this question Transcribed image text
Answer #1

Solution of HCl :

Molarity : 2 mL*0.02050 M / 10 mL = 0.0041 M

[H+] = 0.0041 M

Uncertainty /error :

1 .    2mL volumetric pipet (tolerance +/0.01mL)   :

       % error = 0.01 mL /2 mL *100 = 0.5 %

2.   standardized HCl (0.02050+-0.00005 mol/L)

     % error = 0.00005 M / 0.02050 M *100 = 0.24 %

3.     10mL volumetric flask (Tolerance +/0.02mL) :

      % error = 0.02 mL/ 10 mL *100 = 0.2 %

Combined error = ( 0.52 + 0.242 + 0.22) = 0.6 %

thus, [H+] = 0.0041 M +- 0.6 %

or    [H+] = 0.0041 M +- 0.00003 M

Add a comment
Know the answer?
Add Answer to:
what is the [H+] (and its error) of a solution of HCl that is prepared by...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • A stock solution was prepared by dissolving 0.593 g of pure ASA (molar mass = 180.2...

    A stock solution was prepared by dissolving 0.593 g of pure ASA (molar mass = 180.2 g/mol) with NaOH solution and diluting with water in a 1000 mL volumetric flask. This was followed by pipetting 4.00 mL of the stock solution into flask A and 5.0 mL of the stock into flask B. Flasks A and B were each diluted to 20 mL mark of the volumetric flask. What are the concentrations, in molarity, of ASA in flasks A and...

  • What is the final concentration of a solution prepared by pipetting 10.00 mL of a 0.1284...

    What is the final concentration of a solution prepared by pipetting 10.00 mL of a 0.1284 M NaOH into a 25.00 mL volumetric flask and diluting with water to the mark?

  • A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in...

    A stock solution of Cu2+(aq) was prepared by placing 0.9157 g of solid Cu(NO3)2∙2.5 H2O in a 100.0-mL volumetric flask and diluting to the mark with water. A standard solution was then prepared by transferring 2.00 mL of the stock solution to a second 25.00-mL volumetric flask and diluting to the mark. What is the concentration (in M) of Cu2+(aq)in the stock solution? What is the concentration (in M) of Cu2+(aq)in the standard solution?

  • c. Calculate the molarity of the solution made by pipetting 5 mL of 2.00 + 0.02...

    c. Calculate the molarity of the solution made by pipetting 5 mL of 2.00 + 0.02 M NaOH with a volumetric pipet and transferring this to a 100 mL volumetric flask and diluting to the mark. Show the equation used to calculate error

  • Calculate the concentration of the standard HCl solution you prepared. Determine this concentration for each trial...

    Calculate the concentration of the standard HCl solution you prepared. Determine this concentration for each trial and the average and standard deviation for all three trials. Part B-Preparation and standardization of an HCl Solution 1. Before you can titrate your saturated Ca(oH)a solutions, you must prepare and standardize a dilute solution of Hcl. With a graduated cylinder measure at least 6 mL of the stock Hcl lution, transfer it to a 125 mL Erlenmeyer, and dilute to approximately 100 mL...

  • Calculate the [H+], the [OH-], the pH and the pOH for a solution prepared by diluting...

    Calculate the [H+], the [OH-], the pH and the pOH for a solution prepared by diluting 50.0 ml of 0.035 M HNO3 to 250 ml in a volumetric flask

  • 3. a) A standard ZnCl2 solution is prepared by dissolving 0.6483 g of Zn in an...

    3. a) A standard ZnCl2 solution is prepared by dissolving 0.6483 g of Zn in an HCl solution and diluting to volume in a 1.00 L volumetric flask. An EDTA solution is standardized by titrating a 15.00 mL aliquot of the ZnCl2 solution, which requires 16.12 mL of EDTA solution to reach the end point. Determine the concentration of the EDTA solution. (2 pts)      b) A 1.5146 g sample of powdered milk is dissolved and the solution titrated with...

  • You have 659.3 mL of a stock solution 4.660 M HCl. For a particular experiment, your...

    You have 659.3 mL of a stock solution 4.660 M HCl. For a particular experiment, your lab partner prepared a diluted solution for you to use. In her notes, you read: " Using a volumetric pipet, took 246.54 mL of stock solution and diluted it to 739.21 ml in a volumetric flask. Then, took 100.00 mL of that solution and diluted it to 194.63 mL in a second volumetric flask. " What is the concentration that you should report for...

  • the concentration of FAS is 50.00mg/L and it is diluted to the 50.00mL mark on a...

    the concentration of FAS is 50.00mg/L and it is diluted to the 50.00mL mark on a volumetric flask what is the concentration of Fe(+2) in standard solution in mg/L? and what is the concentration for solutions with 2mL, 5mL, and 10mL (all using a 50.00mL flask)? -The original concentration for 50 mg/L is 50.00mL as indicated in bold above

  • a dilute solution is prepared by transferring 40.00mL of a .3433 M stock solution to a...

    a dilute solution is prepared by transferring 40.00mL of a .3433 M stock solution to a 750mL volumetric flask and diluting to mark. What is the molarity of this dilute solution 0.01838876 M 0.03661 M 0.06436 M 0.004577 M 0.1716 M

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT