Question

In: Chemistry

A 0.3999g sample of reagent grade Al2(SO4)3.xH2O was dissolved and analyzed for its aluminum content gravimetrically...

A 0.3999g sample of reagent grade Al2(SO4)3.xH2O was dissolved and analyzed for its aluminum content gravimetrically by precipitation as the aluminum oxinate complex, AL(C9H6NO)3, the precipitate weighing 0.4185g. Calculate the number of molecules of water of crystallization.

Solutions

Expert Solution

Ans. Moles of Aluminum oxinate, Al(C9H6NO)3 produced = Mass / Molar mass

                                                            = 0.4185 g / (459.439879 g/ mol)

                                                            = 0.000910892 mol

Note that 1 mol aluminum oxinate contains 1 mol Al-atom whereas 1 mol aluminum sulfate, Al2(SO4)3.xH2O contains 2 mol Al-atom. That is, 2 mol aluminum sulfate produces 2 mol aluminum oxinate.

So,

            Moles of Al2(SO4)3.xH2O in sample = (1/2) x moles of Al(C9H6NO)3 produced

                                                            = (1/2) x 0.000910892 mol

                                                            = 0.000455446 mol

1 mol Al2(SO4)3.xH2O consists of 1 mol Al2(SO4)3.

So,

Mass of Al2(SO4)3 in sample = Moles x Molar mass

                                                            = 0.000455446 mol x (342.153878 g/ mol)

                                                            = 0.155832574 g

Now,

            Mass of H2O in sample = (Mass of Al2(SO4)3.xH2O – Mass of Al2(SO4)3) in sample

                                                = 0.3999 g – 0.155832574 g

                                                = 0.244067426 g

            Moles of water in sample = Mass / Molar mass

                                                = 0.244067426 g / (18.01528 g /mol)

                                                = 0.013547801 mol

# Calculate stoichiometry:

Molar stoichiometry in Al2(SO4)3.xH2O = Moles of H2O / Moles of Al2(SO4)3.xH2O

                                                = 0.013547801 mol / 0.000455446 mol

                                                = 29.746 : 1

                                                = 30 : 1                      (nearest whole number)

That is, there are 30 moles of H2O every mol of Al2(SO4)3.xH2O

Hence,

            Molecules of water of crystallization, X = 30

            And, the compound is - Al2(SO4)3.30H2O


Related Solutions

How many moles of Al2(SO4)3 are there in 10.26 g of Al2(SO4)3?
How many moles of Al2(SO4)3 are there in 10.26 g of Al2(SO4)3?
(a) The reaction of Al2(SO4)3 solution with NaOH forms a precipitate according to the equation: Al2(SO4)3...
(a) The reaction of Al2(SO4)3 solution with NaOH forms a precipitate according to the equation: Al2(SO4)3 (aq) + 6NAOH (aq) >>> 3Na2SO4 + 2Al(OH)3. (i) Which species is the precipitate? (b) The addition of more NaOH causes the precipitate in the initial reaction to redissolve: Al(OH)3 + NaOH >>> NaAl(OH)4 (aq) (ii) Write the formula of the complex ion. (iii) Write the net ionic equation for this reaction. (c) Finally, addition of an acid HCl to the solution in (b)...
17.11 g of Al2(SO4)3 is dissolved in water to make 500 mL solution. What is the...
17.11 g of Al2(SO4)3 is dissolved in water to make 500 mL solution. What is the concentration of aluminum ion and sulfate ion in the resulting solution
Determine the mass of oxygen in a 3.6 g sample of Al2(SO4)3. m(O) =
Determine the mass of oxygen in a 3.6 g sample of Al2(SO4)3. m(O) =
A water sample obtained from the neigborhood pond was analyzed for dissolved oxygen content. A volume...
A water sample obtained from the neigborhood pond was analyzed for dissolved oxygen content. A volume of 300 mL, with temperature 21 degrees Celsius, was analyzed using the Wrinkler method shown in the simulated lab material. It took 15.0 mL of 0.01 mol/L Na2S2O3 solution to reach titration end point. *Note: Na2S2O3 solution is the source of S2O32- ions for the titration reaction. In the succeeding questions, provide the following values required. Take note of the units a.What is the...
What is the TOTAL number of atoms in 10.26 g of Al2(SO4)3?
What is the TOTAL number of atoms in 10.26 g of Al2(SO4)3?
9) for the reaction [ 2Al + 3H2SO4 → Al2(SO4)3 + 3 H2SO4] 6.0 g of...
9) for the reaction [ 2Al + 3H2SO4 → Al2(SO4)3 + 3 H2SO4] 6.0 g of Al (MW=26.98 g/mol) are added to 12.0 mL of 0.20 M of H2SO4 A) what is the limiting reagent in the above reaction? b) how many miles of H2SO4 will be formed? c) how many grams of Al2(SO4)3 (MW=342.15 g/mol) are produced in the reaction?
A stainless steel alloy is to be analyzed for its chromium content. A 3.00 g sample...
A stainless steel alloy is to be analyzed for its chromium content. A 3.00 g sample of the steel is used to produce 250.0 mL of a solution containing Cr2O72−. A 10.0-mL portion of this solution is added to BaCl2(aq). When the pH of the solution is properly adjusted, 0.145 g BaCrO4(s)precipitates. What is the percent Cr, by mass, in the steel sample?​
Consider the following unbalanced equation for the reaction of aluminum with sulfuric acid. Al(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2(g). How many...
Consider the following unbalanced equation for the reaction of aluminum with sulfuric acid. Al(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2(g). How many moles of H2 are formed by the complete reaction of 0.384 mol of Al? Express your answer using three significant figures. Chemical Equation -> 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) Calculate the mass of water produced when 2.66 g of butane reacts with excess oxygen. Express your answer to three significant figures and include the appropriate units. Calculate the mass of butane needed to produce 62.7 g of carbon...
A solid hydrate of Ca(NO3)2 is to be analyzed (Ca(NO3)2 •XH2O). A sample of the hydrate...
A solid hydrate of Ca(NO3)2 is to be analyzed (Ca(NO3)2 •XH2O). A sample of the hydrate is weighed in a clean, dry and covered crucible. When empty, the crucible and cover are heated to a constant weight of 30.2016 g. The mass of the crucible and sample is 33.2255 g. The crucible with sample is heated (to drive off the water of hydration) to a final constant weight of 32.2995 g Table 1: Mass Data for the Analysis of a...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT