(4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as outlined in the following reaction. In a typical analysis, the oxalic acid in 10.62 g of rhubarb was extracted with a suitable solvent. The complete oxidation of the oxalic acid to 3+ CO, required 36.44 mL of 0.013 M Fe*.What is the weight percent of oxalic acid in the sample of rhubarb? 2Fe (aq) + H2C2O,laq) + 2H2O(1) → 2FE2* (aq) + 2C02(g) + 2H;0 (aq)

(4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as outlined in the following reaction. In a typical analysis, the oxalic acid in 10.62 g of rhubarb was extracted with a suitable solvent. The complete oxidation of the oxalic acid to 3+ CO, required 36.44 mL of 0.013 M Fe.What is the weight percent of oxalic acid in the sample of rhubarb? 2Fe (aq) + H2C2O,laq) + 2H2O(1) → 2FE2 (aq) + 2C02(g) + 2H;0 (aq)

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: A 0.1285-g sample of impure Na2CO3 was dissolved in 20.00 mL of 0.2034 M HCl. The excess HCl was…

A: We will first find out the actual mass of Na2CO3 present in the sample by calculating the moles of…

Q: A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is…

A: Solution : Titration is used to find out the concentration of an unknown solution(titrand or…

Q: 2. Suggest a reason why it is desirable to use an excess of barium ion in the precipitation.

A: The question is based on the concept of analytical chemistry. we have to mention the need of excess…

Q: The KCIO3 in a 0.1862-g sample of an explosive was determined by reaction with 50.00 mL of 0.01162 M…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Calculation of no. of mol of HNO3 at the end point: n=Molarity×Volume=0.340 mol/L×16.5 ×10-3…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: The objective of this question is to calculate the quantity in moles of HNO3 used in the titration.

Q: A chemist is given a piece of limestone and told that 50.00% of the sample exists as calcium oxide…

A: EDTA forms 1:1 complex with Ca+2.The balanced equation is Ca+2 + EDTA–4 ------->…

Q: The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the…

A: Mass of sample = 0.5136 g Molarity of NaOH = 0.1251 M Volume of NaOH required = 50.00 mL = 0.050 L

Q: The powerful oxidizing agent Ce(IV) can be used to quantitatively determine the concentration of…

A: Given data:Calculate initial concentration of MeMA.If a balanced chemical reaction is known along…

Q: 25.00 mL of hydrochloric acid solution required 42.00 mL of 0.150 M aqueous barium hydroxide…

A: Given that: Volume of hydrochloric acid (V1) = 25.00 mL Volume of barium hydroxide (V2) = 42.00 mL…

Q: For breakfast, the nihilistic Rick Sanchez ate 100 g of cereal mixed with 20 g of milk. A 1.500 g…

A: Given: The molar mass of N (nitrogen) is 14.07 g/mol. For cereal: The amount of cereal consumed is…

Q: In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with…

Q: In an experiment on evaluation of antacid containing magnesium carbonate, a tablet weighing 2.50 g…

A: Given, mass of tablet = 2.50 g molarity of HCl = 1.00 M volume of HCl = 5.00…

Q: When 15.11 ml of 0.102 M K2SO4 solution reacts with 35.00 ml of 0.114 M Pb(C2H3O2)2. predict the…

A: Data given: Volume of K2SO4 solution = 15.11 mL = 0.01511 L (1 L = 1000 mL) Concentration of K2SO4…

Q: 50.00 mL of a solution containing 0.15 M CH2 (CO2 H)2 and 0.020 M MnSO4 Calculate the mass in g of…

Q: A 0.6407-g sample conta ions gave a silver halide This precipitate was then pre of Cl2 gas to…

A: Introduction : The mass percent can be defined as the percentage by mass of each element present in…

Q: The titration of 86.9 mL of an unknown concentration H3PO4 solution requires 94.6 mL of 0.086 M KOH…

A: Volume of H3PO4 = 86.9 ml ...Or because 1L = 1000 ml ...so, = 86.9 ml × (1L / 1000 ml ) =…

Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: The reaction of HNO3 and Ca(OH)2 is, In the given reaction moles ratio between HNO3 and Ca(OH)2 is…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Ca(OH)2 reacts with HNO3. The balanced chemical equation for the reaction is given by:

Q: A 27.56 mL portion of a 0.337 M solution of hydrochloric acid, a monoprotic acid, is to be titrated…

A: The chemical reaction between KOH and hydrochloric acid(HCl): KOH + HCl → KCl +…

Q: A saturated solution of an unknown solid reacted with AgNO3 to give a pale yellow precipitate and…

A: The anion is reacting with AgNO3 gives pale yellow precipitate, therefor the compound might be…

Question

(4) The amount of oxalic acid in a sample of
3+
rhubarb was determined by reacting with Fe
as outlined in the following reaction. In a
typical analysis, the oxalic acid in 10.62 g of
rhubarb was extracted with a suitable solvent.
The complete oxidation of the oxalic acid to
3+
CO, required 36.44 mL of 0.013 M Fe*.What is
the weight percent of oxalic acid in the sample
of rhubarb?
2FE3" (aq) + H2C,O,(aq) + 2H2O(1) → 2Fe?*
(aq) + 2C02(g) + 2H;0 (aq)

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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

A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?
For a 50ml beaker, 0.4532g of pure iron III oxide was weighed, to which 1 ml of a concentrated hydrochloric acid solution was added and then 20 ml of deionized water was added to the beaker. After mixing, the resulting solution was transferred to a 50.00 ml flask and the volume was made up with deionized water. Then 15ml of this solution into a second beaker to which 10ml of an iron iii chloride solution of 0.200 M concentration was added. Calculate the final concentration of the iron iii cation solution expressed in mol/L and in g/L, considering that the volumes are additive.
A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of nitrogen. The liberated NH3 is caught in a solution of H3BO3, and 8.23 ml of HCl are required in the subsequent titration. A sample of pure (NH4)2SO4 (132.12) weighing 0.61 g is treated with excess NaOH and the liberated NH3 (17.04) is also caught in H3BO3. The resulting solution requires 20 ml of the acid for titration. Calculate the percentage of protein in the sample using 6.25 as the factor.
Write a formula for the following precipitate and write a balanced net ionic equation for the reaction that occured between this precipitate and 3 M HNO3(aq). CO32- and 0.2M Pb(NO3)2
2Fe(s) + 3Cu2+(aq) 2Fe3+(aq) + 3Cu(s) a)Calculate the minimum volume of 1.16M CuSO4 solution that is required to ensure complete reaction of 1.04g of Fe.Since you do not know which reaction will be the one to occur, you must base the calculation on whichever of the equations requires more CuSO4 solution. b)To ensure that sufficient CuSO4 is used, it is common practice to add an excess.Calculate the volume of 1.16M CuSO4 needed to provide a 20% excess in this case.
Caculate the volume (mL) of 1.0 M potassium carbonate (K₂CO₃) needed to prepare 5.0g of the COPPER pigment. This is where the balanced chemical equation come in. You should be able to relate the moles of pigment to the moles of K₂CO₃, and from that calculate the volume of 1.0 M K₂CO₃ solution needed. Please report your value as XX.X mL (one deicmal point and no units).