a sample aqueous solution of iron(iii) sulfate has a mass of 200g, a density of 1.05...

a sample aqueous solution of iron(iii) sulfate has a mass of 200g, a density of 1.05 g/cm^3 and 8.35 x10^21 atoms of sulfur. What is the molarity of the solution?

Expert Solution

Fe2(SO4)3

1mole of Fe2(SO4)3 contains 3 moles of S

6.023*10^23 molecules of Fe2(SO4)3 contains 3* 6.023*10^23 of S

3 * 6.023*10^23 molecules of S present in 6.023*10^23 molecules of Fe2(SO4)3

8.35*10^21 molecules of S present in 6.023*10^23*8.35*10^21/3*6.023*10^23 = 2.78*10^21 molecules of Fe2(So4)3

6.023*10^23 molecules of Fe2(SO4)3 = 400g

2.78*10^21 molecules of Fe2(SO4)3 = 400*2.78*10^21/6.023*10^23 = 1.85g of Fe2(SO4)3

volume of solution = mass of solution /density

= 200g/1.05g/cm^3 = 190.5cm^3

molarity = W*1000/G.M.Wt* volume of solution in ml

= 1.85*1000/400*190.5 = 0.0243M >>>>answer

queen_honey_blossom answered 9 months ago

What mass of a solid hydrate of iron (III) sulfate that is 76.3% by mass iron...

What mass of a solid hydrate of iron (III) sulfate that is 76.3% by mass iron (III) sulfate is needed to supply 1.00 g of iron (III) ion? How many moles of carbon atoms are present in 2.41 x 1022 molecules of acetic acid? How many chloride ions are supplied by 1.00 g of chromium (III) chloride hexahydrate? What mass in grams of cobalt(II) nitrate hexahydrate supplies 0.200 g of cobalt (II) nitrate? What mass in grams of oxalic acid...

What is the pH ans the concentration of bisulfate and sulfate in 0.15M solution of iron(III)...

What is the pH ans the concentration of bisulfate and sulfate in 0.15M solution of iron(III) bisulfate? What about in a solution of 2.1M sodium bisulfate?

An aqueous solution is 12.0 % by mass silver nitrate, AgNO3, and has a density of...

An aqueous solution is 12.0 % by mass silver nitrate, AgNO3, and has a density of 1.11 g/mL. The mole fraction of silver nitrate in the solution is ________ . .

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of...

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of 1.02 g/mL. The molality of hydrochloric acid in the solution is ____ m. B) An aqueous solution of iron(III) sulfate has a concentration of 0.192 molal. The percent by mass of iron(III) sulfate in the solution is ____ %.

Consider the reaction of iron (III) sulfate (aq) and sodium phosphate (aq) to form iron (III)...

Consider the reaction of iron (III) sulfate (aq) and sodium phosphate (aq) to form iron (III) phosphate (s) and sodium sulfate (aq). c. If 2.16 g of iron (III) phosphate are obtained when a student performed this reaction, what is the percent yield? d. Is the answer from part C reasonable? Assuming no calculation errors were made, give a possible explanation for the answer in part C. e. If you perform this reaction with 20.00 mL of the 0.250 M...

a. An aqueous solution is made by dissolving 18.4 grams of iron(III) bromide in 314 grams...

a. An aqueous solution is made by dissolving 18.4 grams of iron(III) bromide in 314 grams of water. The molality of iron(III) bromide in the solution is ________m. b.In the laboratory you are asked to make a 0.473 m chromium(II) acetate solution using 425 grams of water. How many grams of chromium(II) acetate should you add? _________ grams. c. The boiling point of diethyl ether CH3CH2OCH2CH3 is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is...

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate,...

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate, a precipitation reaction occurs. Write the balanced net ionic equation of the reaction.

a) The molar solubility of iron(III) sulfide in a 0.249 M iron(III) nitrate solution is __________ M.

a) The molar solubility of iron(III) sulfide in a 0.249 M iron(III) nitrate solution is __________ M. b) The maximum amount of iron(II) sulfide that will dissolve in a 0.164 M sodium sulfide solution is ___________ M. c) The molar solubility of lead iodide in a 0.170 M sodium iodide solution is ______________ M.

The density of an aqueous solution containing 15.0% ethanol (C2H5OH) by mass is 0.974 g/mL. A)...

The density of an aqueous solution containing 15.0% ethanol (C2H5OH) by mass is 0.974 g/mL. A) calculate the molality of this solution. B) calculate the solutions molarity. C) what volume of the solution would contain 0.108 mole of ethanol?

A 228 mL sample of an aqueous solution contains 2.00 %MgCl2 by mass (molar mass of...

A 228 mL sample of an aqueous solution contains 2.00 %MgCl2 by mass (molar mass of MgCl2 is 96.9 g/mol). Exactly one-half of the magnesium ions are Mg−28, a beta emitter with a half-life of 21 hours. What is the decay rate of Mg−28 in the solution after 4.00 days? (Assume a density of 1.02 g/mL for the solution.) Express your answer using two significant figures(atoms/day)

Question