1. The iodide in a sample that also contained chloride was converted to iodate by treatment with an excess of bromine: 3H,O + 3Br, + I¯ → 6Br + I0,¯ + 6H+ The unused bromine was removed by boiling; an excess of barium ion was then added to precipitate the iodate: Ba?+ + 2IO, Ba(IO3), In the analysis of a 2.0375 g sample, 0.0678 this analysis as percent potassium iodate. g barium iodate was recovered. Express the results of

1. The iodide in a sample that also contained chloride was converted to iodate by treatment with an excess of bromine: 3H,O + 3Br, + I¯ → 6Br + I0,¯ + 6H+ The unused bromine was removed by boiling; an excess of barium ion was then added to precipitate the iodate: Ba?+ + 2IO, Ba(IO3), In the analysis of a 2.0375 g sample, 0.0678 this analysis as percent potassium iodate. g barium iodate was recovered. Express the results of

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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A 0,4500 g sample of a pesticide (DDT, C14H9Cl5, MM 354,49 g mol^-1) was decomposed with metallic sodium in alcohol and the released chloride ions were precipitated as AgCl (MM 143,32 g mol-1) . If the precipitate mass corresponds to 0,1706 g of AgCl, calculate the percentage of DDT in the sample.
Please help me solve this. I need to see the steps taken with explanations so that I can keep this as study notes. A 1.345 gram sample of a compound containing barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ions (Ba+2), which was then completely precipitated out with excess potassium chromate to give 2.012 grams of barium chromate, BaCrO4. (a) How many moles of barium ions(Ba+2) were in the original sample? (b) How many grams of barium ions (Ba+2) were in the original sample? (c) How many grams of oxygen ions(O-2) were in the original sample? (d) What is the percentage by mass of O ions (O-2) in the original(1.345g) sample? .
A quality control technician needs to determine the percentage Arsenic (As) in particular pesticide.The pesticide is dissolved and all of the arsenic present is converted to arsenate ions (AsO43-). Then the amount of AsO43- is determined by titrating with a solution containing silver ions (Ag+). The silver reacts with the arsenate according to the net ionic equations: 3 Ag+ + AsO43- → Ag3AsO4 When a 1.22 g sample of pesticide was analyzed this way, it required 25.0 mL of 0.102 M Ag+ solution to precipitate all of the AsO43-. What was the mass percentage of arsenic in the pesticide?
esc 100. mL of 0.10 M CaCl₂ is mixed with 50.0 mL of a 0.10 M solution of either Al₂(SO4)3, Na₂SO4, or AgNO3. 1.36 g of precipitate is produced. Is the solution Al₂(SO), Na₂SO, or AgNO₂? Fn Al₂(SO)₂(aq) + 3CaCl(aq) → 3CaSO4(s) + 2 AICI₂ (aq) 3 Select the single best answer. Na₂SO (aq) + CaCl₂(aq) 2AgNO3(aq) + CaCl₂(aq) → ⒸAL₂(SO4)3 O Na₂SO4 O AgNO3 Continue 61°F Partly cloudy CaCl₂(aq) → CaSO (s) + 2 NaCl(aq) 4 F1 3 F2 F3 2AgCl(s) + 2AgCl(s) + Ca(NO3)₂ (aq) X Ś DII F4 Search F5 S F6 F7 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A P 8 F8 > H F9 DOLL prt sc F10 home Submit Assig F11 end F12 in
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?
The concentration of borax (Na₂B4O5(OH)4) in aqueous solution can be determined through titration with HCI as titrant. The net ionic equation for the titration reaction is: B4O5(OH)42 (aq) + 2 H*(aq) + 3 H₂O 4 H3BO3(aq) In an experiment, a student titrated 5.0 mL borax solution with 5.43 0.249 M HCI solution. Determine the concentration of borax in mol/L. For a strong electrolyte compound with formula X3Y2, if the concentration of cation X is 0.614 M, find the concentration of anion Y in mol/L. The molar solubility of a compound AX₂ is 3.8 x 103 M. Calculate the value of natural log of Ksp (Inksp) for AX₂. The enthalpy change (AH) and entropy change (AS) of a process can be obtained by plotting In(Kea) versus 1/Temperature (temperature in Kelvin). A student did the graph and obtained the slope as 7,712 and y-intercept as 6.41, respectively. Determine the enthalpy change of the reaction in kilojoule/mol Question 7 The enthalpy change (AH) and entropy change (AS) of a process can be…
In the laboratory you are given the task of separating Ca2+ and Fe2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the lons, give the formula of the precipitate. If it cannot, type "No" Y or N 1. 12. 3 Reagent Formula of Precipitate if YES ка K₂SO4 Na CO
In the laboratory you are given the task of separating Ba2+ and Co2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. fill in the blank K2S 1 2. fill in the blank 3 KCI 3. fill in the blank 5 КОН
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite. involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MNCO,(s)-0,(g)→2 MnO,(s)-2 C0 (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO, (s)- 4 Al(s)-3 Mn(s)–2 Al,O,(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.
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