ZuoTi.Pro
Question

Imagine that you are working at a lab station (at the Mountain Dew factory) with an...

Imagine that you are working at a lab station (at the Mountain Dew factory) with an ultra pure water sample. Unfortunately, your lab neighbor accidentally splashes a few small drops of HCl in your sample when you aren't looking. What is the new pH of your ultra pure water if the HCl concentration is 5.0×10−7M solution of HCl?

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

ultra pure water is neutral.

thus it has a pH of 7

but, accidentally there is HCl added ie 5.0 x 10^-7

since, HCl is a strong acid.. so dissociate completely to produce H+ ions.

thus H+ ions = 5.0 × 10^-7

and pure H2O has = 10^-7

thus total [H+] = 5× 10^-7. +. 10^-7

= 6 x 10^-7

pH = -log[H+]

= -log(6× 10^-7)

= 6.22

0 0
Add a comment
Know the answer?
Add Answer to:
Imagine that you are working at a lab station (at the Mountain Dew factory) with an...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 6.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 6.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2mol L−1 HCl, 100 mL of 5.00×10−2mol L−1 NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 6.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...

  • Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you...

    Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...

  • Constants Periodic Table Imagine that you are in chemistry lab and need to make 1.00 L...

    Constants Periodic Table Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. Part A You have in front of you 100 mL of 7.00x10-2 MHCI, 100 mL of 5.00x10-2 MNaOH, and plenty of distilled water. Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to achieve the desired pH? Express your answer to three significant figures and include the...

  • Mixing Strong Acids and Bases (< 1 of 13 > Constants Periodic Table Imagine that you...

    Mixing Strong Acids and Bases (< 1 of 13 > Constants Periodic Table Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you Part A • 100 mL of 7.00x10-2 MHCI, · 100 mL of 5.00x10-2 M NaOH, and • plenty of distilled water. Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to...

  • As part of Lab 11 you will make and standardize a solution of NaOH(aq). Suppose in the lab you measure the solid NaOH an...

    As part of Lab 11 you will make and standardize a solution of NaOH(aq). Suppose in the lab you measure the solid NaOH and dissolve it into 100.0 mL of water. You then measure 0.1993 g of KHP (204.22 g/mol) and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phenolphthalein indicator. You titrate this with your NaOH(aq) solution and find that the...

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
ADVERTISEMENT