solution of sodium thiosulfate, Na2S203, is 0.4203 M. 8.52 mL of this solution reacts with 26.21 mL of I₂ solution. What is the molarity of the 12 solution? Na2S203) + 12-Na₂S406 + 2(Nal) Submit Answer Tries 0/99 29.07 mL of the 12 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H₂0) + 212 2(H3ASO4) + 4HI Submit Answer Tries 0/99 This discussion is closed.

solution of sodium thiosulfate, Na2S203, is 0.4203 M. 8.52 mL of this solution reacts with 26.21 mL of I₂ solution. What is the molarity of the 12 solution? Na2S203) + 12-Na₂S406 + 2(Nal) Submit Answer Tries 0/99 29.07 mL of the 12 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H₂0) + 212 2(H3ASO4) + 4HI Submit Answer Tries 0/99 This discussion is closed.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 135CP: A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of...

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95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?
Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?
Try and answer the following questions without using a calculator. a A solution is made by mixing 1.0 L of 0.5 M NaCl and 0.5 L of 1.0 M CaCl2. Which ion is at the highest concentration in the solution? b Another solution is made by mixing 0.50 L of 1.0 M KBr and 0.50 L of 1.0 M K3PO4. What is the concentration of each ion in the solution?
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?
What volume of 0.250 M NaOH is required to react completely with 0.0100 moles of H2SO4? (a) 80.0 mL (b) 60.0 mL (c) 40.0 mL (d) 125 mL
Two liters of a 1.5 M solution of sodium hydroxide are needed for a laboratory experiment. A stock solution of 5.0 M NaOH is available. How is the desired solution prepared?
A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.
An experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many mL of 11.9 M HCl would be required to make 250 mL of 2.00 M HCl?
Distinguish between the terms slightly soluble and weak. electrolyte.
Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to neutralize 0.3602 g carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?
Follow the directions for Question 9 for the following pairs of solutions. (a) sodium phosphate and barium chloride (b) zinc sulfate and potassium hydroxide (c) ammonium sulfate and sodium chloride (d) cobalt(III) nitrate and sodium phosphate
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?

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