A powder contains FeSO4·7H2O (molar mass = 278.01 g/mol) among other components. A 2.750-g sample of the powder was dissolved in HNO3 and heated to convert all iron to Fe3+ . The addition of NH3 precipitated Fe2O3·xH2O which was subsequently ignited to produce 0.484 g of Fe2O3. What was the mass of FeSO4·7H2O in the 2.750-g sample

Q: A 21.25g mixture of the solid salts, sodium chloride and lead (11) nitrate , is added to distilled…

A:

Q: Iron(II) can be oxidized to iron(III) by dichromate ion, which is reduced to chromium(III) in acid…

A: From given  Initially with the data , the reaction is given and from the reaction number of moles of…

Q: The phosphorus in a 0.2222-g sample was precipitated as the slightly soluble (NH4)3PO4 • 12Mo O3.…

A: P2O5 = 2 (NH4)3PO4 • 12Mo O3 = 24 PbMoO4   Moles of PbMoO4 are, Moles = mass ÷ molar mass Moles =…

Q: The Burke Museum at the UW is analyzing a dinosaur bone sample for the amount of calcium it…

A: The solid

Q: A solution of 25 mL Na2CO3 is neutralized with 22.4 mL of 0.1065 M HCl. In the another analysis, 50…

A: Given that, Volume of 0.1065 M HCl = 22.4 mL  = 0.0224 L Moles of HCl in 0.0224 L = 0.1065 M×0.0224…

Q: 100.0 mL of an aqueous solution containing 0.250 M KOH(aq) is mixed with 100.0 mL of an aqueous…

A: First of all, we need to write down the balanced chemical.  The molar mass of Fe(OH)3 = 106.87g/mol

Q: A sample of 0.3207 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Number of moles is calculated by dividing given mass with molecular mass.

Q: A small iron pan was analyzed by dissolving a 11.1321 g sample in HCl. The resulting solution was…

A: Given, mass of Fe3O4 = 5.1231 g molar mass of Fe3O4 = 231.533 g/mol !! Calculate the moles of Fe3O4…

Q: In the laboratory you are given the task of separating Ca and Fe" ions in aqueous solution. For each…

A: We are authorized to answer one question at a time, since you have not mentioned which question you…

Q: A sample of 0.3233 g of an ionic compound containing the bromide ion (Br¯) is dissolved in water and…

A: Given information: Mass of sample = 0.3233 g Mass of AgBr = 0.7017 g

Q: How many milliliters of 2.00M HCl(aq) are required to react with 2.15g of an ore containing 36.0%…

A: Calculation for mass of zinc:

Q: In a neutralization reaction, 50.00 mL of 0.8500 M phosphoric acid reacts with 2.500 g of magnesium…

A: The answers to the first three questions can be given as - Given Data -

Q: A powder contains FeSO4 ·7H2O (molar mass = = 278.01 g/mol), among other components. A 2.825 g…

A: To find the mass of FeSO₄·7H₂O in the 2.825 g sample, we need to follow these steps: 1. Calculate…

Q: Sulfate samples are to be analyzed by BaSO4 (233.38 g/mol) precipitation. It was known that the SO4…

A:

Q: The N in a 0.4984-g sample of organic material is converted to NH4HSO4 by digestion with…

A: Solution: This question is based on mole concept. if we know the moles of Pt then by using…

Q: 5.587 grams of Pb(NO3)2 are reacted with 5.587 grams of Na2S, and the resulting precipitate is…

A: The given reaction is as follows. Pb(NO3)2aq+Na2Saq→2NaNO3aq+PbSs The precipitate formed in this…

Q: A 4.399 g sample containing Mg2+ is dissolved and treated with excess (NH4)2HPO4, resulting in the…

A: Given : Mass of Mg2+ sample = 4.399 g And mass of Mg2P2O7 precipitate produced = 1.42 g

Q: A solution of 300.0 mL of 0.150 M Nickel (II) sulfate is mixed with a solution of 100.0 mL of 0.200…

A: Balanced chemical equation is necessary so as to abide by the law of conservation of mass and to…

Q: A mixture is prepared by adding 25.5 mL of 0.200 M Na3PO4 to 37.7 mL of 0.126 M Ca(NO3)2. (a) What…

A: Given: The volume of Na3PO4 (V1)= 25..5 mL = 0.0255 L The volume of Ca(NO3)2 (V2)= 37.7 mL = 0.0377…

Q: A 4.23 g sample of a mixture of BaCl2 and Ba(NO3)2 is treated with excess AgNO3(aq). The precipitate…

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Q: How many grams of Ag2CO3 will precipitate when excess Na2CO3 solution is added to 45.0 mL of 0.538M…

A:

Q: In a reaction between copper metal and aqueous iron (III) chloride, Fe3+(aq) is reduced to Fe2+(aq),…

A: First, we need to calculate the number of moles of FeCl3 in the solution. The molarity (M) of a…

Q: What mass of solid potassium oxalate (K2C2O4), when dissolved in an acidic solution, would be…

A:

Q: An aqueous solution of Pb(NO3)2 is mixed with an aqueous solution of AlCl3. Which is the net ionic…

A:

Q: A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 4.30 mL sample. About…

A:

Q: The total mass of 20 iron-containing tablets used in nutritional disorders is 22.131 g, and they are…

A: The question is based on the concept of quantitative estimation. we have to quantitatively estimate…

Q: 0.8838-g sample of an ionic compound containing bromide ions and an unknown metal cation is…

A: Weight of ionic compound = 0.8838 gm Weight of precipitate (AgBr) = 1.573 gm

Q: A piece of chalk (mainly calcium carbonate) is placed in 250. mL of 0.337 M HCl. All the CaCO3…

A:

Q: A 0.7785 g sample containing hydrazine (N2H4, rocket fuel) was dissolved and diluted to 250.0 mL in…

A: Answer: This question is based on stoichiometric calculation where we have to convert the moles of…

Q: 3-5.00 grams of potassium carbonate and 5.00 grams sodium carbonate were treated separately with…

A: Given data isMass of potassium carbonate = 5.00 grams mass of potassium carbonate = 5.00 grams

Q: A 0.9157 g mixture of CaBr2 and NaBr is dissolved in water, and AgNO3 is added to the solution to…

A: Given, Amount of  is 0.9157 g.Mass of the precipitate is 1.6390 g. Two reactions are taking place:

Q: A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no…

A: To calculate the molarity of the Ba2+ ions, first of all, we calculate the moles of barium sulfate.

Q: Zinc and magnesium react with hydrochloric acid to produce the metal chlorides and hydrogen gas. A…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: . Barium-contaminated soil can be remediated by immobilization of the barium as alforsite,…

A: A) To calculate the weight percent of alforsite in the soil sample, you need to find the mass of the…

Q: When a sample (0.6271 g) of impure magnesium chloride (MgCl2, MM = 95.211) was dissolved in water…

A: The reaction in which a precipitate is formed in the product is known as precipitation reaction.

Q: A 6.586-g sample containing magnesium chloride and sodium chloride was dissolved in sufficient water…

A: Mass of sample = 6.586 g Mass of sample solution = 500 mL Mass of AgCl formed from 50 mL solution =…

Q: 1. H2SO4. The resulting solution contained excess acid and required 15.85 mL of 0.09850 M NaOH for…

A: The balanced equations are   CaCO3 + H2SO4 ----------> CaSO4 + CO2 + H2O    H2SO4 + 2 NaOH…

Q: Write the balanced NET ionic equation for the reaction when aqueous Cs₃PO₄ and aqueous AgNO₃ are…

A:

Q: A supplement was tested for iron content in a laboratory. First, a random sample of 10 tablets…

A: #(a): Given the mass of the iron tablet taken to obtain Fe2O3(s) = 2.7544 g  Mass of pure and dry…

Q: A metallurgical laboratory carried out analysis of a sample in which analysis of Mn was done by…

A:

Q: Excess Na2SO4(aq) is added to a 2.43×102 mL sample of industrial waste containing Ba2+ ions. If 20.5…

A: Total industrial sample = 2.43 x 102 mLTotal mass of BaSO4 precipitated= 20.5gThe given reaction is

Q: 38 mL volume of 1.74 M Fe(NOa)a is mixed with 43 mL of 0.98M Fe(NOa solution. Calculate the molar…

A:

Q: A sample of 0.3291 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Given Mass of sample = 0.3291 g Mass of AgBr = 0.6905 g Moles of AgBr = mass of AgBrmolar mass of…

Q: How many grams of Ag2CO3 will precipitate when excess Na2CO3 solution is added to 41.0 mL of 0.744 M…

A:

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.