Question

If you start with 30.0 mL of solution A and you add 2.0 mL of 0.50...

  1. If you start with 30.0 mL of solution A and you add 2.0 mL of 0.50 M HCl, calculate the pH of the final solution.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

HCl is a strong acid, hence will dissociate completely in the solution

                              

Initial                    0.03125M       0         0

Final                          0           0.03125 0.03125

0 0
Know the answer?
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
Similar Questions
If you start with 80.0 mL of solution B and you add 10.0 mL of 0.60...
If you start with 80.0 mL of solution B and you add 10.0 mL of 0.60 M NaOH, calculate the pH of the final solution.
Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of...
Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of 0.50 M HCl to 49 mL of the buffer. What is the new pH of the solution?
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of 0.50 M HCl to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of...
Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of 0.50 M HCl to 49 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M...
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution: (a) prior to the start of the titration pH = (b) after the addition of 25.1 mL of 0.350 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 71.9 mL of 0.350 M HCl. pH =
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 M...
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution: (a) prior to the start of the titration pH = (b) after the addition of 48.4 mL of 0.260 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 76.2 mL of 0.260 M HCl. pH =
Calculate the pH of solution by mixing 30.0 mL of 0.0182 M HNO3 with 21.0 mL...
Calculate the pH of solution by mixing 30.0 mL of 0.0182 M HNO3 with 21.0 mL of 0.0130 M Ca(ClO2)2
Calculate the pH of the solution resulting from the addition of 30.0 mL of 0.200 M...
Calculate the pH of the solution resulting from the addition of 30.0 mL of 0.200 M HClO4 to 60.0 mL of 0.150 M NaOH
a) 30.0 ml of an HCl solution of unknown molarity was titrated with .200 M NaOH....
a) 30.0 ml of an HCl solution of unknown molarity was titrated with .200 M NaOH. Phenolphthalien was used as the indicator. The titrated solution turned a very pale pink after 21.8 mL of NaOH was added. What was the initial molarity of the HCl? b)Consider the following three titrations: 100.0 mL of 0.100 M CH3NH2 (Kb = 4.4x10-4) titrated with 0.100 M HCl 100.0 mL of 0.100 M NH3 (Kb = 1.8x10-5) titrated with 0.100 M HCl 100.0 mL...
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 6.00×10−2 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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT