Enter your answer in the provided box. The mass percent of CI in a seawater sample is determined by titrating 25.00 mL of seawater with AGNO3 solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free Ag* ion is present in solution after all the CI™has reacted. If 59.44 mL of 0.2130 M AgNO, is required to reach the end point, what is the mass percent of CI in the seawater (d of seawater = 1.024 g/mL)? mass % CI

Enter your answer in the provided box. The mass percent of CI in a seawater sample is determined by titrating 25.00 mL of seawater with AGNO3 solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free Ag* ion is present in solution after all the CI™has reacted. If 59.44 mL of 0.2130 M AgNO, is required to reach the end point, what is the mass percent of CI in the seawater (d of seawater = 1.024 g/mL)? mass % CI

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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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.
Solid sodium hydroxide is slowly added to 75.0 mL of a 0.238 M iron(III) sulfate solution until the concentration of hydroxide ion is 0.0576 M. The mass of iron(III) ion remaining in solution is grams.
A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
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.
A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed. The precipitate (BaSO4) is collected, dried, and weighed. If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample? Your answer should have 3 sig. figs. Molar Masses: (Na2SO4: 142.05 g/mol) (Ba2+: 137.3 g/mol) (BaSO4: 233.37 g/mol)
Solid potassium cyanide is slowly added to 75.0 mL of a 0.360 M nickel(II) acetate solution until the concentration of cyanide ion is 0.0231 M. The mass of nickel ion remaining in solution is grams
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
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 total percent recovery based on the combined masses that were recovered.
V A chemistry student weighs out 0.135 g of phosphoric acid (H₂PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1200M NaOH solution. O CHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. icrosoft O W Welcome, Simrat - Microsoft tab os lock 0 Microsoft 6.52.210... esc mL control Explanation 1 Q A 2 option Z Check @ 2 W S #3 X command x10 X E D NOV 14 $ 4 C S R 8 F 07 dº % 5 T V tv MacBook Pro < 6 G Y & 7 H Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility U * 00 8 B N J "A ( 9 M K O W O L H P command 33 + 11 [ I opt
A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed. The precipitate (BaSO4) is collected, dried, and weighed. If 1.21 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample? Your answer should have 3 sig. figs. Molar Masses: (Na2SO4: 142.05 g/mol) (Ba2+: 137.3 g/mol) (BaSO4: 233.37 g/mol)