You are working as a chemist and your boss asks you for 100 g of iron(III) hydroxide. Unfortunately, you do not have this chemical in store but you know you can prepare it from iron(III) chloride and potassium hydroxide. (At every step, explain your reasoning and calculations. a)Write the formulae of iron(III) hydroxide, iron(III) chloride and potassium hydroxide and calculate their molecular weight. Formula for below compounds Molecular weight (g.mol-1) for below compounds: Iron(III) chloride Iron(III) hydroxide Potassium hydroxide b)You only have iron(III) chloride as a solid and you need to dissolve it in water. You decide to prepare 500.00 mL of a 3.000 M iron(III) chloride solution in water, called solution A. What mass of solid will you weight? s c)Decribe the experimental steps you must follow to accurately perform the dissolution of the solid to obtain solution A.
1)You are working as a chemist and your boss asks you for 100 g of iron(III) hydroxide. Unfortunately, you do not have this chemical in store but you know you can prepare it from iron(III) chloride and potassium hydroxide. (At every step, explain your reasoning and calculations.
a)Write the formulae of iron(III) hydroxide, iron(III) chloride and potassium hydroxide and calculate their molecular weight.
Formula for below compounds
Molecular weight (g.mol-1) for below compounds:
Iron(III) chloride
Iron(III) hydroxide
Potassium hydroxide
b)You only have iron(III) chloride as a solid and you need to dissolve it in water. You decide to prepare 500.00 mL of a 3.000 M iron(III) chloride solution in water, called solution A. What mass of solid will you weight? s
c)Decribe the experimental steps you must follow to accurately perform the dissolution of the solid to obtain solution A.
d)You mix 450 mL of this new solution with 750 mL of 6.00 M potassium hydroxide solution you already have in the lab. You observe the formation of a light blue precipitate. Write all three forms of the balanced chemical equation for this reaction. Do not forget to indicate the physical state of each chemical species
Molecular equation:
Complete ionic equation:
Net ionic equation:
e)What is the limiting reagent in this reaction?
f)What is the expected mass of copper(II) hydroxide after the reaction is complete.
g)You collect the solid by filtration on paper. You transfer the wet solid to an evaporating dish and dry it overnight in the oven. The next morning, you weight the dry solid and find only 124.8g. YES! Your colleagues jump at your exclamation. You have enough to satisfy your boss!
What is the percent yield of your reaction?
2)Consider the reaction taking place between 20.0 mL of a 1.05 M aqueous solution of AgNO3 and 15.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed.
a)What is the nature of the precipitate? Write down its formula AND its name.
b)What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution.
c)Calculate the mass of solid obtained.
d)Calculate the concentration of all the remaining ions in solution.
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