The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,O, (aq)(thiosulfate ion). The determination is based on the net ionic equation2 S,0 (aq) + 1, (aq) → S,0 (aq) + 31-(aq)Given that it requires 38.6 mL of 0.470 M Na, S,O, (aq) to titrate a 10.0 mL sample of I, (aq), calculate the molarity of I, (aq) inthe solution.[5] =M

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Answered: The amount of I, (aq) in a solution can…

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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The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,0 (aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S,03 (aq) + I5(aq) → S,0 (aq) + 31(aq) Given that it requires 30.1 mL of 0.310 M Na, S,O, (aq) to titrate a 15.0 mL sample of I, (aq), calculate the molarity of I, (aq) in the solution. [I]= Question Source: MRG - General Chemistry Publisher: University Science Books
Wa 5. In a laboratory activity, Ca(OH)2(s) is completely dissolved in distilled water. This solution is then used to titrate a solution of HClag- Write the equation representing this neutralization reaction. Ca(OH):(aq) + HClI(aq) >
Calculate the number of millimeters of 0.641 M NaOH required to precipitate all the Fe3+ ions in 178 mL of 0.447 M FeI3 solution as Fe(OH)3. The equation for the reaction is FeI3(aq)+3NaOH(aq)->Fe(OH)3(s)+3NaI(aq)
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 69. mg of oxalic acid (H,C,04), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 144.8 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
The quantity of Cl^- in a municipal water supply is determined by titrating the sample with Ag^+. The precipitation reaction taking place during the titration is Ag^+ (aq) + Cl^- (aq) > AgCl (s). a) How many grams of chloride ion are in a sample of the water if 20.2 mL 0f 0.100M Ag^+ is needed to react with all tghe chloride in the sample? b) if the sample has a mass of 10.0g, what percentage of Cl^- does it contain?
The amount of I−3(aq) in a solution can be determined by titration with a solution containing a known concentration of S2O2−3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S2O2−3(aq)+I−3(aq)⟶S4O2−6(aq)+3I−(aq) Given that it requires 33.5 mL of 0.430 M Na2S2O3(aq) to titrate a 15.0 mL sample of I−3(aq), calculate the molarity of I−3(aq) in the solution.
By titration, it is found that 35.3 mL of 0.141 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCI solution. [HCI] = = 0.1 Incorrect M
A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s) How many moles of Ag+ (aq) ions are used to reach the end point? How many moles of Cℓ- (aq) have reacted in the titration? How many grams of chloride are present in the sample? What is the mass percent of chloride in the sample?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 86. mg of oxalic acid (H,C,04), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 37.0 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits. x10
50 mL of a 1.067 M solution of HCI was diluted to 250 mL. The diluted HCI solution was then titrated with an unknown concentration of KOH. It is found that an average volume of 24.20 mL of KOH is required to reach an endpoint in a titration with 25.00 mL of the dilute acid solution. The equation for the reaction is; H(aq) + OH(aq) -> H₂O (1) Calculate the moles of your unknown solution (KOH). Remember to use the correct number of significant figures. G| ΑΣΦ ? moles
1. (a) Write balanced molecular equations for the following potential precipitation reactions. Indicate the states of reactants and products [(aq) or (s)]. (b) In those cases where a precipitate forms, write the net ionic equation. If there is no reaction, state "No reaction." (i) Na₂S (aq) + Pb(NO3)2 (aq) → (iii) MgCl₂ (aq) + Pb(NO3)2 (aq) → (ii) FeSO4 (aq) + Na3PO4 (aq) → (iv) K₂SO4 (aq) + Ni(NO3)2 (aq) →
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 287. mg of oxalic acid (H, C,04), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 75.9 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits. ||M

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