in an experiment 4.7g Al2O3 and excess HF were dissolved in 500 ml of 0.12M NaOH if 6.45g Na2AlF6 was obtained. a) Determine the Actual yield b) Determine the theoretical yield. c) Determine the percent yield of the experiment.

in an experiment 4.7g Al2O3 and excess HF were dissolved in 500 ml of 0.12M NaOH if 6.45g Na2AlF6 was obtained. a) Determine the Actual yield b) Determine the theoretical yield. c) Determine the percent yield of the experiment.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 2. When 50.0 mL of a 0.300 M AGNO; solution is added to 250.0 mL, 0.050 M of MgCl, a AgCl…

A: M

Q: Neohetramine, C6H21ON4 (FW = 285.37), is a common antihistamine. A 0.1642 gram sample containing…

A: The mass of sample is 0.1642 g. The volume of 0.01537 M HCl used in titration is 27.85 mL. The molar…

Q: If 20 mL of 0.5 M Pb(NO3)2 solution is added into 40 mL 0.5 M KI solution, how many grams of Pbl2…

A: A multiple choice question based on mole concept, which is to be accomplished.

Q: A 0.660 M solution of KCl needs to be prepared through dilution. A 2.00 M stock solution will be…

Q: A stock solution of potassium permanganate (KMNO4) was prepared by dissolving 10.0 g KMNO4 with DI…

A: To solve this problem we will first calculate the number of moles of KMnO4 Then Molarity will be…

Q: 0.3061 g of dissolved oxalic acid dihydrate (molecular weight = 126.064 g/mole) is reacted with 20.0…

A: The formula of oxalic acid is H2C2O4 . It is a diprotic acid and has two protons available for…

Q: At the end of a titration, 40.00 mL of base was added. The molarity of the NaOH was 0.508 M. How…

A: Number of mols of base is = Volume in L × Molarity(mol/L)

Q: A 0.786 g sample of KHP is dissolved in 50 mL of water and titrated with KOH. The initial burette…

Q: What mass of Na2CrO4 is required to precipitate all of the silver ions from 65.0 mL of a 0.800 M…

Q: Excess aluminum nitrate is mixed with 789.6 mL of sodium sulfate at a concentration of 0.679 mol/L.…

A: given balanced reaction, 2Al(NO3)3 + 3Na2SO4 → Al2(SO4)3 + 6NaNO3 volume of sodium sulfate, V =…

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: If 26.6 mLmL of AgNO3AgNO3 is needed to precipitate all the Cl−Cl− ions in a 0.755-mgmg sample of…

A: Given data contains, Volume of AgNO3 is 26.6 mL=0.0266 L. Mass of KCl=0.755 mg=0.000755 g

Q: 1.00 L of a solution is prepared by dissolving 125.6 g of NaF in it. If I took 180 mL of that…

A: Given : Mass of NaF = 125.6 g Volume of initial solution = 1.00 L Volume of initial solution used =…

Q: If 30.4 g of C₂H₅OH (MM = 46.07 g/mol) are added to a 500.0 mL volumetric flask, and water is added…

A: Molar concentration = Number of moles of solute/Volume of solution (L) Number of moles of solute =…

Q: How many grams of PbBr2 will precipitate when excess AlBr3 solution is added to 66.0 mL of 0.754 M…

A: Given: Concentration (molarity) of Pb(NO3)2 = 0.754 M Volume of Pb(NO3)2 = 66.0 mL molar mass of…

Q: -25. What is the concentration (in molarity ) of a NaOH solution if 25.0 mL of the solution are…

A: Sodium hydroxide reacts with hydrochloric acid, to form sodium chloride and water. The equation for…

Q: A 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry…

A: Molarity of a solution is defined as number of moles of a given solute per litre of the solution. It…

Q: A 0.460 M solution of KCl needs to be prepared through dilution. A 2.00 M stock solution will be…

A: The dilution equation is: C1V1 = C2V2 where C1 is the initial concentration, V1 is the initial…

Q: A solution of 100.0 mL of 0.200 M KOH is mixed with a solutionof 200.0 mL of 0.150 M NiSO4. (a)…

Q: What mass of Naz CrO4 is required to precipitate all of the silver ions from 40.0 mL of a 0.200 M…

A: Given data,Molarity of AgNO3=0.200MVolume of AgNO3=40mL=0.040L

Q: A 50.0 mL sample of 0.108 M H2SO4 is diluted to 250.0 mL. What is its new molarity?

Q: Calculate the mass (g) of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution with…

A: The chemical reaction between Na2CO3 and Mg(NO3)2 is shown below.

Q: How many moles of precipitate will be formed when 70.0 mL of .150 M AgNO3

A: You have molarity of AgNO3 = 0.15 M Volume of AgNO3 = 70.0 mL = 0.07 L You know that Precipitation…

Q: A 0.430 M solution of KCl needs to be prepared through dilution. A 2.00 M stock solution will be…

A: To calculate the volume of the 2.00 M stock solution needed to prepare a 0.430 M solution of KCl,…

Q: How many moles of CSOH are contained in 244 mL of 0.135 m CsOH solution? The density of the solution…

A: Volumeof CsOH = 244 mlMolality of CsOH = 0.135 mDensity of solution = 1.22 g/mL

Q: 27 If 35.0 g of CH3OH (MM = 32.0 g/mol) are dissolved in 500.0 mL of solution, what is the…

A: Since, Molarity is the number of moles of solute dissolve in one litre of the solution. Thus,

Q: With 85% H2SO4 by volume in water being used in the reaction, how many moles of water will be added…

A: 85% volume of H2SO4 means 85 ml H2SO4 in 100 ml Solution. And remaining 15 % is water, that is 15 ml…

Q: If 47.1 g of C₂H5OH (MM = 46.07 g/mol) are added to a 500.0, mL volumetric flask, and water is added…

Question

in an experiment 4.7g Al2O3 and excess HF were dissolved in 500 ml of
0.12M NaOH if 6.45g Na2AlF6 was obtained. a) Determine the Actual yield
b) Determine the theoretical yield. c) Determine the percent yield of the
experiment.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Moles of the constituents in the reaction

VIEW

Step 2: Balanced reaction

VIEW

Step 3: Yield of the product

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What volume of 0.10 m NaOH can be prepared from 250. mL of 0.30 m NaOH?
Barium can be analyzed by precipitating it as BaSO4 and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H2SO4, 0.0891 g of BaSO4 formed. What percentage of barium is in the compound?
How many grams of Ni(OH)2Ni(OH)2 are produced from the reaction of 27.0 mLmL of a 1.95 M NaOH M NaOH solution and excess NiCl2NiCl2?
3. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H₂O₂. Reaction: SO2(g) + H₂O2 → H₂SO4. A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.
When 4.96 g of KHP reacts with 1.7 M NaOH, the mL of NaOH required is
It is known that when mixed in solution aqueous, silver ions will react with chloride ions to form insoluble silver chloride. Upon dissolving a 5.000 g solid mixture of AgNO3 and KNO3 in a concentrated KCl solution, 1.582 grams of a white precipitate, AgCl(s), formed. Determine the percent, by weight, of AgNO3 in the original mixture.
determine the mass of CuS formed when 100.mL of 0.100M H2S and 50.0ml of 0.150M Cu(C2H3O2)2 are reacted. What is the concentration of C2H3O2 in the resulting solution?
A 50.0-mL volume of AgNO3 solution contains 0.0345 moles AgNO3. What is the molarity of the solution?
10) A solution is made by diluting 348 mL of a 3.42M KCl stock solution with water to a final volume of 1.98L. What is the molar concentration of the diluted solution
If 10. g of AgNO3 is available, what volume of 0.35 M AgNO3solution can be prepared?
A 12.0 M solution of concentrated nitric acid has 25.0 mL withdrawn from it. The 25.0 mL sample is then diluted until the total volume of the resulting solution is 2.00 L. What is the concentration of the dilute solution?
A solution is prepared by adding 2.0 g of solid CaBr2 and 1.55g of NaBr to 100.ml of 0.15 M AlBr3. What is the molarity of the bromide ion in the final solution? ( assume the volume of solids added to be negligible.)