We needed to let the sample dry before we checked purity. How would we be able to use the melting point to determine if there was still solvent in the sample? O Melting point won't tell us there's still solvent there. O If the melting point is much higher than the literature value, then we know there's still solvent in it. O If the melting point of the product is lower and wider than expected, it may still be wet. O If the crystals are too small to fit in the melting point capillary, then they are not fully dry.

We needed to let the sample dry before we checked purity. How would we be able to use the melting point to determine if there was still solvent in the sample? O Melting point won't tell us there's still solvent there. O If the melting point is much higher than the literature value, then we know there's still solvent in it. O If the melting point of the product is lower and wider than expected, it may still be wet. O If the crystals are too small to fit in the melting point capillary, then they are not fully dry.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

CuSO A solution consists of 35.00 g of 4 dissolved in 250.0 mL of water. The molar mass of Cu is 63.55 %/mol, the molar mass of S is 32.07 %/mol, and the molar mass of O is 16.00 %/mol. What is the molarity of the solution? Show your work.
Question 6 a,b,c
What is the theory behind recrystallization purifying a solid?
a) What is the purpose of performing a distillation? p) How is a distillation performed? c) What factors would cause you to choose to do a fractional distillation instead of a simple distillation?
Given a solid sample that contains impurities, how would you determine which solvent to use for recrystallization? Describe how you would do this in the laboratory.
Saved Normal BIIIU fxl Ix Actual mass used in solution prep (g) Volume solution prepared Measured conductivity (uS/cm) Substance 0.1 g Naci 0.1003 100 mL 1149 0.1 g Nal 0.10 100 ml 419 Calculate the mass of Nal that would be necessary to yield the same conductivity as the NaCl solution. Clearly show these calculations in your lab notebook. Saved T BII U X X + fr Normal
My experiment was to have eight drops of liquid in each well. For a one I had five drops of Na2S2O3 and three drops of hydrochloric acid. For well A2 I had four drops of Na2S2O3, One drop of distilled water, and three drops of hydrochloric acid. For well a three I had three drops of Na2S2O3, two drops of distilled water, and three drops of hydrochloric acid. Four well a four I had two drops of Na2S2O3, three drops of distilled water, and three drops of hydrochloric acid. Use the table for information to answer the questions below. Additional information: hydrochloric acid = 0.1M and the sodium Thiosulfate (Na2S2O3) = 0.1M.
To prepare the solution you would place the solute in a 50.0 ml volumetric flask, and then fill to the mark with water while mixing. This would give a total solution volume of 50.0 ml. The 5.0 solution needs to be diluted to make 10.0 ml of a 2.0% solution. What volume of 5.0% solution should be used? Please answer fast i give you upvote.