I got this question wrong. I *believe* I read the buret correctly. To get the la

Question

I got this question wrong. I *believe* I read the buret correctly. To get the last box I divided: 0.856/.00215

Any help in correcting this would be much appreciated!

The flask shown here contains 0.856 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.320 M NaOH. What volume of base is needed to reach the end point of the titration? What is the molar mass of the acid (assuming it is diprotic and that the end point corresponds to the second equivalaence point)? 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 drop by drop until the pink color persists in the flask.

Explanation / Answer

Hello!

I read 22 mL in the buret, remember the meniscus tells you the measure.

For box 2 remember: ConcNaOH x VNaOH = moles of NaOH and at the Equivalence Point = Moles of Acid therefore Moles of Acid= 0.32Mx0.022L=7.04E-3 mol

The molar mass = 0.856g/7.04E-3 mol = 122.87 g/mol

My Regards!!

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