The concentration of hydrogen peroxide in a solution is determined by titrating it with a 0.1217 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnO4 (aq) + 5H₂O2 (aq) + 6H3O+ (aq) → 2Mn²+ (aq) +50₂ (1) + 14H₂O(1) In one experiment, 19.09 mL of the 0.1217 M permanganate solution is required to react completely with 40.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. Concentration = M

The concentration of hydrogen peroxide in a solution is determined by titrating it with a 0.1217 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnO4 (aq) + 5H₂O2 (aq) + 6H3O+ (aq) → 2Mn²+ (aq) +50₂ (1) + 14H₂O(1) In one experiment, 19.09 mL of the 0.1217 M permanganate solution is required to react completely with 40.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. Concentration = 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

Balance the following equation, in basic solution, ClO4− (aq) + C6H14O4(aq) → Cl−(aq) + HCO3− (aq)
To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a 4.30 g sample of the shell to a fine powder and titrates it to the endpoint with 233. mL of 0.2700M hydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCl(aq) + CO3(aq) → H₂CO3(aq) + 2Cl(aq) 19 0 What kind of reaction is this? O precipitation O acid-base redox X olo If you said this was a precipitation reaction, enter the chemical formula of the precipitate. 0 Ar 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 CaCO3 in the sample. Be sure your answer has 3 significant digits. П 0 0% S ?
Write the net ionic equation, including phases, that corresponds to the reaction Pb(NO3)2(aq)+Na2CO3(aq)⟶PbCO3(s)+2NaNO3(aq)
The following chemical reaction takes place in aqueous solution: CuBr2 (aq) + 2NaOH (aq) → CuOH2 (s) + 2NaBr (aq) Write the net ionic equation for this reaction.
The concentration of SO32- in a solution is determined by titrating it with a 0.1464 M dichromate solution. The balanced net ionic equation for the reaction is: Cr₂O72-(aq) + 3SO32(aq) + 8H30*(aq) → 2Cr³+ (aq) + 3504²(aq) + 12H₂O(l) In one experiment, 23.91 mL of the 0.1464 M dichromate solution is required to react completely with 30.00 mL of the SO32- solution. Calculate the concentration of the SO3²- solution. M
The amount of I3 (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 2 S₂O3(aq) + 13(aq) - S₂O²(aq) + 31¯(aq) Given that it requires 37.4 mL of 0.470 M Na₂S₂O3(aq) to titrate a 25.0 mL sample of 13 (aq), calculate the molarity of I3 (aq) in the solution. [¹] : 0.159 Incorrect M
A solution of permanganate is standardized by titration with oxalic acid, H₂C₂O4. To react completely with 1.000 × 10-³ mol of oxalic acid required 35.29 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is MnO4 (aq) + H₂C₂O4 (aq) → →Mn²+ (aq) + CO2 (9) Determine the concentration of the permanganate solution in molarity. Concentration = M
A volume of 10 mL of an unknown hydrochloric acid sample was diluted to 100 mL. The diluted solution was then titrated against a solution of sodium carbonate (prepared by dissolving 0.2188 g of solid in 50 mL distilled water). Hydrochloric acid reacted with sodium carbonate according to the following equation: 2 HCI (aq) + Na,CO3 (aq)H20 () + CO2 (g) + 2 NaCl (aq) A volume of 15.2 mL of the hydrochloric acid was required to complete the reaction in the titration process. A second titration was done between the same acid sample against a blank for indicator correction, a volume of 0.3 mL was consumed by the indicator. Find the moles of HCI added and concentration of dilute HCI solution. [MM of Na CO3 = 105.99 g/mol, MM of HCI = 36.46 g/mol] 2.06x10-3 mol ; 0.277 M B 2.06 x10-3 mol; 0.135 M 4.13x10-3 mol ; 0.277 M 4.13x10-3 mol ; 0.272 M
The amount of I, (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 2 S₂O3(aq) + ₂ (aq) → S₂O²(aq) + 31 (aq) Given that it requires 35.5 mL of 0.440 M Na₂S₂O3(aq) to titrate a 30.0 mL sample of I3 (aq), calculate the molarity of I3 (aq) in the solution. [1] = M
What is the balanced net ionic equation for the reaction between aqueous solutions of acetic acid and sodium hydroxide? CH3CO₂H(aq) + OH (aq)-CH3 (aq) + CO2(g) + H₂O(0) Ob CH3CO₂H(aq) + 2 Na* (aq) + 2 OH (aq) → CH3CO₂2 (aq) + 2Na* (aq) + H₂O(0) OCH3CO₂H(aq) + 3 NaOH(aq)-CCO₂H³ (aq) + 3 Na* (aq) + H₂O(0) OCH3CO₂H(aq) + OH (aq) → CH3(aq) + CO3²- (aq) + H₂(g) OCH3CO₂H(aq) + OH (aq)-CH3CO2 (aq) + H₂O(l)
The following equation represents the reaction that occurs when aqueous solutions of sodium hydroxide and magnesium acetate are combined. Mg(CH3COO)2(aq) + 2NaOH(aq) Mg(OH)2(s) + 2NaCH3COO(aq) Write a balanced net ionic equation for the reaction. Assume that all ionic compounds that are in aqueous solution are dissociated. Use the pull-down choices to specify states such as (aq) or (s). If a box is not needed leave it blank. ______ + ______ + ______ + ______ >>> ______ + ______
Balance the following chemical equation (if necessary): Na:PO:(aq) + NİCI:(aq) → Nis(PO+)>(s) + NaCI(aq)