QUESTION 1 Read off the volume in mL of NaOH at the equivalence point. QUESTION

Question

QUESTION 1

Read off the volume in mL of NaOH at the equivalence point.

QUESTION 2

Separately calculate the volume in mL of 0.20 M NaOH needed to react completely with 100 mL of 0.040 M HCl.

QUESTION 3

Calculate the volume in mL of 0.20M NaOH needed to react completely with 100.mL of 0.040M acetic acid.

QUESTION 4

Does the volume of NaOH needed to reach the equivalence point depend on whether the acid is strong or weak?

Yes
No

QUESTION 5

Compare the pH curves for HCl and acetic acid before the equivalence point. Does the acetic acid curve satisfy the definition of a buffer, i.e. a region with an intermediate value of pH, with a slow variation of pH as the NaOH is added

Yes
No

QUESTION 6

What is the pH of the solution acetic acid solution at the equivalence point?

QUESTION 7

How many equivalence points are in the titration of a diprotic acid?  123limitless

QUESTION 8

The other sheet shows titration curves for reaction of a diprotic acid with NaOH. On this sheet you need to enter the two Ka values of the acid manually, in cells E1 = 1.00 x 10-3

And E2 = 1.0 0x 10-8.

Enter the volume and concentration data in the pink cells G1, G2 and G4:

            Volume of acid: 100mL:                     Enter 100

            Concentration of acid: 0.040M           Enter 0.040

            Concentration of NaOH: 0.20M         Enter 0.20

What is the pH after 40 mL of NaOH has been added to the diprotic aicd?

Explanation / Answer

A graph is missing for question 1

Question 2

NaOH + HCl ==== NaCl + H2O

1 mole of NaOH requires 1 mole of HCl so if we have 0.1 Liters of 0.04 M of HCl then the available moles are

moles = molarity * volume

moles = 0.04 * 0.1 = 0.004 moles of HCl available so there are 0.004 moles of NaOH

We need to calculate the volume needed to get 0.004 moles of 0.2M of NaOH

volume = moles / molarity = 0.004 / 0.2 = 0.02 Liters of solution

Question 3

NaOH + CH3COOH = CH3COONa + H2O, 1 mole of NaOH requires 1 mole of acetic acid

since we have the same numbers as question 2 then we can say that we will require 0.02 liters of solution of 0.2 M NaOH

Question 4

The volume required to reach the equivalence point does not depend on wether the acid is strong or weak

Question 5

The titration curve of CH3COOH with NaOH sattisfies the deffinition of buffer, the region before the equivalence point has a low ph variation, the intermediate value of ph is known as pka

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