The amount of I5 (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S₂O3(aq) + 15 (aq) - SO2 (aq) +31 (aq) Given that it requires 41.0 mL of 0.450 M Na₂S₂O3(aq) to titrate a 20.0 mL sample of 15 (aq), calculate the molarity of 15 (aq) i the solution. [13] = M

The amount of I5 (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S₂O3(aq) + 15 (aq) - SO2 (aq) +31 (aq) Given that it requires 41.0 mL of 0.450 M Na₂S₂O3(aq) to titrate a 20.0 mL sample of 15 (aq), calculate the molarity of 15 (aq) i the solution. [13] = M

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...

See similar textbooks

Similar questions

Calculate the pH of 0.225 M RbOH(aq).
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
A 0.200 g sample of an unknown monoprotic acid (e.g., HX) is dissolved in water and titrated with NaOH. The equivalence point of the titration is reached after the addition of 19.03 mL of 0.1750 M NaOH. Calculate the molar mass of the acid. NaOH(aq) + HX(aq) → H₂O(1) + NaX(aq) (Balanced) Reminder - the equivalence point is where stoichiometric amounts of acid and base have been added! 36.56 g/mol (HCI) O20.00 g/mol (HF) O100.46 g/mol (HCIO4) 60.05 g/mol (HCH3COO) 80.91 g/mol (HBr)
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) The concentration of KOH is 0.2205 M Calculate the concentration of the KOH in g/L (you will need to find the formula weight of KOH to do this) 15| ΑΣΦ ? g/L
Please don't provide handwritten solution
Write a balanced net-ionic equation for the neutralization reaction between CH3COOH (aq) and Ba(OH)2 (aq). 2 CH3COOH (aq) + Ba(OH)2 (aq) --> 2 CH3COO- (aq) + 2 H₂O (1) + Ba²+ (aq) 2 CH3COOH (aq) + 2 OH" (aq) --> 2 CH3COO(aq) + 2 H₂O (1) CH3COOH (aq) + OH" (aq) --> CH3COO (aq) + H₂0 (1) OH(aq) + OH- (aq) --> H₂O (1) 2 H (aq) + 2 OH- (aq) --> 2 H₂O (1)
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 150.mL of a 0.023 M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
To measure the concentration of an aqueous solution ofH2O2, an analytical chemist adds strong acid to a 39.00g sample of the solution and titrates it to the endpoint with 49.5mL of 0.2700M potassium permanganate KMnO4 solution. The balanced chemical equation for the reaction is: 6H+(aq) + 5H2O2(aq) + 2MnO−4(aq) -> 5O2(g) + 2Mn2+(aq) 8H2O(l) 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 H2O2 in the sample. Be sure your answer has the correct number of significant digits.
A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined. 2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.
The concentration of Sn²+ in a solution is determined by titrating it with a 0.1890 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnOq°(aq) + 5Sn²*(aq) + 16H3O*(aq) → 2Mn²+(aq) + 5Sn*(aq) + 24H,O(1) In one experiment, 24.99 mL of the 0.1890-M permanganate solution is required to react completely with 40.00 mL of the Sn2+ solution. Calculate the concentration of the Sn2+ solution. M
A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH(aq) →A¯(aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 10 ", is titrated with NaOH. 6 Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit ▾ Part B pH = IVE] ΑΣΦ Submit A → c More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 66.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IVE ΑΣΦ A + Ċ ? Doowoon Review | Constants | Periodic Table ?
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.