To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.260M silver nitrate (AgNO,) solution to a 21.0 g sample of the fluid and collects the solid silver chloride (AgCl) product. When no more AgCl is produced, she filters, washes and weighs it, and finds that 725. mg has been produced. The balanced chemical equation for the reaction is: CI (ag) + AgNO,(aq) → A£CI(s) - No, (aq) olo + O precipitation What kind of reaction is this? O acid-base O redox If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits. 0% O

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.260M silver nitrate (AgNO,) solution to a 21.0 g sample of the fluid and collects the solid silver chloride (AgCl) product. When no more AgCl is produced, she filters, washes and weighs it, and finds that 725. mg has been produced. The balanced chemical equation for the reaction is: CI (ag) + AgNO,(aq) → A£CI(s) - No, (aq) olo + O precipitation What kind of reaction is this? O acid-base O redox If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits. 0% O

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...

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3. You are asked to determine the percentage of the components of a mixture containing sodium iodide Nal, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82 g. First you extracted the Nal from the mixture with water and filtered insoluble Mg(OH)2 and Baso from the solution, containing the Nal. After evaporating and drying the filtrate, you find that you have recovered 0.95 g of Nal When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCI, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04 g of BasO4 Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering the solution and drying the precipitate, you recovered 1.21 g of Mg(OH)2. a) Calculate the percent Nal in the original sample mixture b) Calculate the percent Mg(OH)2 in the original sample mixture c) Calculate the percent BaSO,…
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2. Calculate the percent Mg(OH)2 in the original sample mixture.
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2.
18. A beverage mixture contains citric acid, C6H8O7 (molar mass 192 g/mol), plus sugar and flavorings. The mass of citric acid in a sample was determined by titration with sodium hydroxide solution. If a 1.500 g sample of the beverage mix required 46.65 mL of 0.1068 N NaOH for complete neutralization, how many grams of citric acid were initially present in the sample? (Citric acid has three dissociable protons) A) 4.98 g B) 1.11 g C) 0.956 g D) 0.319 g E) None of these is correct
M Complete and balance the chemical equation associated with the neutralization of aqueous sodium hydroxide with aqueous boric acid. If it takes 20.45 ml of a 0.1026 M standard sodium hydroxide solution to titrate 25.00 ml of an unknown boric acid solution, what was the original concentration of the unknown boric acid solution?
Does a reaction occur when aqueous solutions of manganese(II) chloride and silver(I) sulfate are combined? If a reaction does occur, write the net ionic equation.
A gravimetrical analysis is done with an unknown sample containing AgNO3. A 1.5020-g solid mixture is dissolved in water and treated with an excess of NaCl solutions, resulting in the precipitation of 0.6168 g of AgCl. What is the mass of AgNO3 in the mixture?
8. Sodium thiosulfate, Na2S₂O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2 (389.912 g/mol), is allowed to react with excess potassium iodide in acidic solutions. The net ionic equations are: production of iodine from KH(IO3)2: IO3¯¯ +5 I¯¯+ 6H* → 3 1₂ + 3 H₂O 1₂+2 S₂03² → 2 I¯+S406²- 2- titration of iodine: What is the molarity of a sodium thiosulfate solution if 39.66 mL are required to titrate the iodine released from 0.1022 g of KH(IO3)2?
A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. Write the balanced molecular equation for the reaction. Write the net ionic equation for the reaction. How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).
To measure the amount of nickel in some industrial waste fluid, an analytical chemist adds 0.190M sodium hydroxide (NaOH) solution to a 25.00 g sample of the fluid and collects the solid nickel(II) hydroxide (Ni(OH)2) product. When no more Ni(OH)₂ is produced, she filters, washes and weighs it, and finds that 558. mg has been produced. The balanced chemical equation for the reaction is: ft C W rosoft Icrosoft 52.210. BSC .2+ Ni²+ (aq) + 2NaOH(aq) → Ni(OH)₂ (s) + 2 Na* (aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Ni in the sample. Be sure your answer has the correct number of significant digits. Explanation Q A option T Z 2 Check 8,935) W S X 88 command 3 E D DEC…
8. A chemist wants to make 100 of a 0.15 M AlCl 3 (aq) solution. How many grams of aluminum chloride should the chemist use?
A student soaks willow bark (a natural source of salicylic acid) in ethanol. After a few minutes, the student has 12.5 mL of salicylic acid. The student determines the concentration of salicylic acid is 0.30 M. Calculate the amount, in grams, of acetylsalicylic acid that can be produced when the salicylic acid is reacted with excess acetic acid.