Question

In lab you are asked to titrate 50.00 mL of 1.000 M HCl with 1.000 M...

In lab you are asked to titrate 50.00 mL of 1.000 M HCl with 1.000 M NaOH. Predict what the pH will be after adding 60.00 mL of NaOH.

Homework Answers

Answer #1

Given:

M(HCl) = 1 M

V(HCl) = 50 mL

M(NaOH) = 1 M

V(NaOH) = 60 mL

mol(HCl) = M(HCl) * V(HCl)

mol(HCl) = 1 M * 50 mL = 50 mmol

mol(NaOH) = M(NaOH) * V(NaOH)

mol(NaOH) = 1 M * 60 mL = 60 mmol

We have:

mol(HCl) = 50 mmol

mol(NaOH) = 60 mmol

50 mmol of both will react

remaining mol of NaOH = 10 mmol

Total volume = 110.0 mL

[OH-]= mol of base remaining / volume

[OH-] = 10 mmol/110.0 mL

= 9.091*10^-2 M

use:

pOH = -log [OH-]

= -log (9.091*10^-2)

= 1.0414

use:

PH = 14 - pOH

= 14 - 1.0414

= 12.9586

Answer: 12.96

Know the answer?
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
Similar Questions
You titrate 25.0 mL of 0.15 M HCl with 0.10 M sodium hydroxide. a. What is...
You titrate 25.0 mL of 0.15 M HCl with 0.10 M sodium hydroxide. a. What is the pH after 20.0 mL NaOH have been added? b. How many mL of NaOH are required to reach the equivalence point?
a. You titrate 25.0 mL of 0.60 M NH3 with 0.60 M HCl. Calculate the pH...
a. You titrate 25.0 mL of 0.60 M NH3 with 0.60 M HCl. Calculate the pH of the solution after adding 5.00, 15.0, 22.0, and 30.0 mL of the acid. Ka = 5.6×10-10 pH(5.00 mL added) ------------------------------ pH(15.0 mL added)------------------------------ pH(22.0 mL added) ---------------------------- pH(30.0 mL added)---------------------------- b. itration of 27.9 mL of a solution of the weak base aniline, C6H5NH2, requires 28.64 mL of 0.160 M HCl to reach the equivalence point. C6H5NH2(aq) + H3O+(aq) ⇆ C6H5NH3+(aq) + H2O(ℓ)...
The titration of 50.00 mL of 0.160-M HCL with 0.160-M NaOH (the titrant) is carried out...
The titration of 50.00 mL of 0.160-M HCL with 0.160-M NaOH (the titrant) is carried out in a chemistry laboratory. Calculate the pH of the solution after these volumes of the titrant have been added: i. 0.0 mL ii. 25.0 mL iii. 49.9 ml
Generate the hypothetical titration curve for the titration of 50.00 mL of 0.0500 M HCl with...
Generate the hypothetical titration curve for the titration of 50.00 mL of 0.0500 M HCl with 0.1000 M NaOH at 25 degrees Celsius. Hint: For this type of problem, first calculate the volume of the titrant you need to add to reach equivalence point (VOH-=Veq), and then calculaett the pH at: 1. Initial point (before adding the titrant VOH-=0) 2. Before equivalence point (0<VOH-<Veq) ex. V=10.00 mL 3. At equivalence point (VOH-=Veq) 4. After equivalence point (VOH->Veq) ex. V= 25.10...
A buret is filled with a 0.100M HCl and its used to titrate 35.0 mL of...
A buret is filled with a 0.100M HCl and its used to titrate 35.0 mL of an unknown strong base. The titration requires 44.57 mL of HCl to reach the equivalence point. The pH after adding 40 mL of HCl will be ? The pH at the equivalence point will be? - Please explain how you got the answer, thank you
Do the calculations for the titration of 50.00 mL of a 0.1000 M solution of H2SO3...
Do the calculations for the titration of 50.00 mL of a 0.1000 M solution of H2SO3 with a 0.2000 M solution of NaOH. Calculate the pH after the addition of 0.00, 12.50, 25.00, 37.50, 50.00, and 60.00 mL of NaOH. Ka1(H2SO3)=1.23×10-2; Ka2(HSO3-)=6.60×10-8. Please show all of your work.Thanks!
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
What is the pH of the solution that results from adding 50.00 mL of 0.1000 M...
What is the pH of the solution that results from adding 50.00 mL of 0.1000 M Acetic Acid with 10.00 mL of 0.1000 M NaOH
You titrate 10.0 mL of 0.30 M acetic acid with 0.10 M sodium hydroxide. a. What...
You titrate 10.0 mL of 0.30 M acetic acid with 0.10 M sodium hydroxide. a. What is the pH of the solution after you have added 10.00 mL of NaOH? b.   What is the pH of the solution at the equivalence point?
A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M...
A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M HCl and 0.0500 M HOAc. Please determine the pH of the solution after 27.00 mL of NaOH is added. Ka, HOAc = 1.75*10-5 . Answer. 4.04 Just want to see how they got that.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT