The flask shown here contains 10.0 mL of HCL and a few drops of phenolphthalein

Question

The flask shown here contains 10.0 mL of HCL and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH.
What volume of NaOH is needed to reach the end point of the titration?
What was the initial concentration of HCl? Ma Sapling Learning macmillan learning The flask shown here contains 10.0 mL of HCI and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH. mL Res What volume of NaOH is needed to reach the end point of the titration? - 15 Number 25 12.38 mL NaOH 35 40 45 What was the initial concentration of HCI? Number 0.26 M HCI You may not have reached the end point of the titration yet, or you may be reading the volume in the buret incorrectly Once you see pink that fades away in the flask continue adding base d pink color persists in the flas drop until the O Previous Give Up & View Solution Try Again Next Exit

Explanation / Answer

Part 1:

This question is totally based on the readings shown by the burette.

We calculate volumes of titrant (which is NaOH here) needed to reach end point by,

= Final volume - initial volume

= 30 mL - 0 mL

= 30 mL

Note : I have considered initial volume as zero because i have assume you have started the experiment with 0 mL and this is your first result.

Part 2:

Using, M1V1 = M2V2

Where M1, M2 = molarity of HCl and NaOH respectively

V1, V2 = volumes of HCl and NaOH respectively

So, M1 = M2V2 / V1

= 0.210 M * 30 mL / 10 mL

= 0.63 M

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