Chemistry Homework Help

24/7 Chemistry Homework Help

Get step-by-step solutions from expert tutors.

How it works?

Ask a question

Type, take a picture, or paste your question with all necessary details to ensure high-quality responses.

Get an answer in less than 24hrs

Once our tutors receive the question, they'll begin. You'll get an email once the solution is ready.

Get Notified

We will send you email and text notification to let you know when your question is answered.

Browse Homework Solutions

31 solutions

Weak Base Strong Acid Titrations

Q. (20pt.)50.00 mL of 0.100 M C5H5N is titrated with 0.050 M HCl.a.What is the initial pH before any HCl is added?b.What is the pH after the addition of 10.0 mL of HCl? c.What is the pH at the equivalence point?d.What is the pH 10.0 mL of HCl past the endpoin

Solved • Aug 12, 2019

Weak Base Strong Acid Titrations

Q. Calculate the pH for the titration of 50.0 mL of a 0.10 M methylamine solution with a0.20 M HCl solution: after 12.5 mL of HCl has been added, Kb CH3NH2 = 4.4 x 10–4. I understand how to do the problem, but CH3NH2 is a weak base and the equation given was CH3NH2(aq)+H+ (aq) ->>>>>>>. CH3NH3 I just dont understand how the equation would be written like that because I was doing more like HCl + CH3NH2 -> CH3NH2Cl + H (which is wrong but how come?)

Solved • Aug 4, 2019

Weak Base Strong Acid Titrations

Q. 50 ml of 0.10 M NH3 (aq) is titrated with 0.050 HCLO4 (aq) calculate when pH when the following total volume of HCLO4 are added kb (NH3) = 1.8 X 10^-5 0) 0ml a) 10 ml b) 100 ml c) 110 ml I am not allowed to use the henderson hasselbach equation

Solved • Aug 2, 2019

Weak Base Strong Acid Titrations

Q. Suppose that you completed a titration of 50.0 mL of 0.20 M NH3 with 0.40 M HI. After the addition of 20.0 mL of 0.40 M HI. What is the pH of the solution?

Solved • Aug 1, 2019

Weak Base Strong Acid Titrations

Q. 50 ml of 0.10 M NH3 (aq) is titrated with 0.050 HCLO4 (aq) calculate when pH when the following total volume of HCLO4 are added kb (NH3) = 1.8 X 10^-5 0) 0ml a) 10 ml b) 100 ml c) 110 ml

Solved • Jul 30, 2019

Weak Base Strong Acid Titrations

Q. A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HF is 3.5 × 10-4. 3.09 2.78 3.46 4.11 3.82

Solved • Jul 27, 2019

Weak Base Strong Acid Titrations

Q. 1. Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid C4H4N2O3 (Ka = 9.8× 10−5) with 0.100 M KOH. (a) no KOH added (b) 20 mL of KOH solution added (c) 39 mL of KOH solution added (d) 40 mL of KOH solution added (e) 41 mL of KOH solution added

Solved • Jul 26, 2019