Balance the equations under basic solution. (Show each step) a. SO32- + Cu(OH)2 ➡️ SO42- + Cu(OH) b. CH3CH2OH + MnO4- ➡️ CH3COO- + MnO2

Q: 2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 .  Begin this calculation by…

A: #Q.2.1: Given the concentration of HC2H3O2 solution = 1.0 M Equation for the dissociation of…

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Q: 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask.…

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Q: Titration of a 0.485 g sample by Mohr method required 36.80 mL of the standard 0.1060 M AgNO3…

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Q: a) Cr.0,2- + Fe* → Fe3* + Cr3+ (in acidic solution) b) Mn* + BiO3 → MnOq¯ + Bi³* (in acidic…

A: a) Cr2O72-+Fe2+→Fe3++Cr3+ The oxidation state of Cr is +6. b) Mn2++BiO3-→MnO4-+Bi3+ The oxidation…

Q: An unknown 8.00 ml sample containing a certain concentration of tin Sn*2 (118.7 g/mol), was treated…

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Q: alculate the amount of manganese (54.94 g/mol) from a processed ore using the following data.

A: Solution: Blank titration part: Here we have 0.1012 g of manganese ore. Which is digested with…

Q: A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid.…

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A: metallic aluminum (m(Al) = 0.5540 g) is dissolved in dilute sulfuric acid, the resulting solution is…

Q: A 1.025 g sample containing Cl- is analyzed through the Mohr method. The sample is dissolved in 250…

A: Given that -  Mass of a sample containing Cl- ions = 1.025 g  Volume of Solution prepared = 250 mL…

Q: A sample containing iron (Fe) is brought into solution in acetic medium and titrated with KMN04…

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Q: The sulfur content of an iron pyrite ore sample is determined by converting it to H2S gas, absorbing…

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Q: Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation :…

A: Dissociation of the given complex is shown.

Q: To determine the concentration of an EDTA solution, the following aluminum(III) solution is…

A: metallic aluminum (m(Al) = 0.5943 g) is dissolved in dilute sulfuric acid, the resulting solution is…

Q: The tetraethyl lead Pb(C2H5)4 in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL of…

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

Q: Determine the solubility of Ag2SO3 (Ksp=1.5x10-14; MW=295.8 g/mole) in a 0.2 M solution of Na2SO3.

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Q: The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01…

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Q: 3. Indirect analysis. A 0.6200-g sample that contains NaCl, NaBr, and impurities gives a precipitate…

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Q: 1. Determine the Ecell values for the following: a. TI (s) | TI* (aq) || Sn2+ (aq) | Sn(s) b. Zn(s)|…

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Q: A 0.4435-g sample of impure Na2CO3 (FW 105.99) was analyzed by the Volhard method. After adding…

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Q: A 0.6892 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW = 49.005 g/mol) was dissolved in water.…

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Q: Mass of zinc = 1.050 g. Calculate the number of moles of zinc in the 250 mL flask (show workings)…

A: There are multiple questions asked in a single question,  so as per our guidelines,  I will answer…

Q: Balance the reaction in acid and base medium using half reaction method 1. Cu + HNO3 — Cu^+2 + NO

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: It is desired to prepare a 250 ppm 500 ml stock copper (II) solution to work at A.A.S. According to…

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Q: In the following experiment, you will titrate 2.00 mL of 0.0100 M KMnO4 in base with 0.0200 M…

A: Given: Volume= 2.00 mL= 0.002 L Molarity of KMnO4= 0.0100 M Molarity of NaHSO3= 0.0200 M

Q: PART 1: A solution contains 0.00010 M copper(II) ions and 0.0020 M lead(II) ions. a) What minimal…

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Q: Q2- A 30.0 mL H2C204 acidified solution, was treated with 25.0 ml of 0.102 M KMNO, solution. The…

A: The moles of Fe2+ ions can be calculated by - Moles = Molarity × volume in Liter Moles = 0.053 ×(…

Q: Calculations for Acetate Buffer Solutions  Molarity of acetic in acetate buffer       (below is…

A: Molarity = Moles of soluteL of solution Moles = Molarity x L of solution

Q: A 0.2585 gram amount of H₂C₂O4 is dissolved in approximately 100 mL of 0.5 M H₂SO4. A KMnO4 solution…

A: Given :-  Mass of H2C2O4 = 0.2585 g  Molarity of H2SO4 = 0.5 M  Volume of H2SO4 (approximately) =…

Q: A Cu2+ solution is prepared by dissolving a 0.4728 g piece of copper wire in acid. The solution is…

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Q: Andrew dissolved 10.00 grams of an iron ore sample in 5.00 L of acid to produce a stock solution.…

A: The diluted solution was found to be containing 1.62×10-5 M Fe2+.

Q: Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation :…

A: The given compound first undergoes dissociation in its aqueous solution as:

Q: A 1.000-g sample containing KHC2O4, H2C2O4, and impurities required 38.22 mL of 0.1000 M NaOH for…

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Q: How many milliliters of 0.05 M EDTA are required to react with the calcium and magnesium in a 0.1414…

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Q: Ascorbic acid (Vitamin C, MW = 176.126g/mol) is a reducing agent, reacting as follows:  C6H8O6 →…

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Q: In the analysis of 1.500 g sample of feldspar, a mixture of the chlorides of sodium and potassium…

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Q: The amount of Fe in a 0.4891 gm sample of an ore was determined by redox titration with K Cr , 0 ,.…

A: Iron Ore is Fe2O3, and redox titration is done with Potassium dichromate K2Cr2O7  Mole of K2Cr2O7 =…

Q: 3. A 4.326 g sample containing ethyl mercaptan (C₂H_SH) was treated with 50.00 mL of 0.1287 M 1₂ in…

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Q: A 10.0 g sample of KCgH5O4 (A)(MW = 204.23 g A) was titrated with 50.00 mL of KOH (B) to endpoint.…

A: The balanced reaction taking place is given as, => Given: Mass of KC8H5O4 taken = 10.0 g. The…

Q: The tetraethyl lead [Pb(C2H5)4] in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL…

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Q: The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of…

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Q: the thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and…

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Q: 1. A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with…

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Q: The Zn in a 0.8872-g sample of foot powder was titrated with 24.24 mL of 0.01842 M EDTA. Calculate…

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