140 Prentice Hall Laboratory Manual for Introductory Chemistry 5. An alum hydrat

Question

140 Prentice Hall Laboratory Manual for Introductory Chemistry 5. An alum hydrate sample was analyzed by decomposition and gave the following data: mass of beaker and watchglass+ alum hydrate mass of beaker and watchglass mass of beaker and watchglass + anhydrous compound 96.818 g 95.886 g 96.398 g e theoreti Calculate the experimental percentage of water. Do the experimental results agree wit value shown in Example Exercise 1? hth An unknown hydrate (AC·XH,O) was analyzed and found to contain 13.7% water of the anhydrous compound (AC) is 345 g/mol, what is the water of crystallization? the molar n 6. 7. What are the major sources of error in this experiment? 8. What safety precautions must be observed in this experiment?

Explanation / Answer

5)

mass of hydrated alum = 96.818 g - 95.886 g

= 0.932 g

mass of anhydrous alum = 96.398 g - 95.886 g

= 0.512 g

mass of H2O = mass of hydrated alum - mass of anhydrous alum

= 0.932 g - 0.512 g

= 0.420 g

mass % of H2O = mass of H2O * 100 /mass of hydrated alum

= 0.420*100/0.932

= 45.1 %

Answer: 45.1 %

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