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 30.2 mL of 0.490 M Na2S2O3(aq) to titrate a 20.0 mL sample of I−3(aq), calculate the molarity of I−3(aq) in the solution.

A buret is filled with 0.1517 M NaOH(aq).NaOH(aq). A 25.0 mL portion of an unknown acid HA(aq)HA(aq) and two drops of indicator are added to an Erlenmeyer flask, and the titration experiment is carried out. If the initial buret reading was 0.55 mL, and the buret reading at the end point was 22.50 mL, what is the molarity of the unknown acid, HA?

In a precipitation reaction between FeCl2(aq) and LiOH(aq), 109ml of 0.18 M FeCl2(aq) completely reacted with 0.17 M of LiOH(aq) solution. What was the volume (in ml) of LiOH?

A particular solution of NaOH is supposed to be approximately 0.100 M. To determine the exact molarity of the NaOH(aq), a 0.5000 g sample of KHC8H4O4 is dissolved in water and titrated with 24.03 mL of the NaOH(aq). What is the actual molarity of the NaOH(aq)?

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 25,0 (aq) +(aq)- SO (aq) + 31 (aq) Given that it requires 31.9 mL of 0.210 M Na₂S₂O, (aq) to titrate a 10.0 mL. sample of I5 (aq), calculate the molarity of I5 (aq) in the solution. = x10 TOOLS - I M

The amount of nitrogen in an organic substance can be determined by an analytical method called the Kjeldahl method, in which all the nitrogen in the organic substance is converted to ammonia. The ammonia, which is a weak base, can be neutralized with hydrochloric acid, as described by the equation NH3(aq) + HCl(aq) ->> NH₂Cl(aq) If 6.0 mL of 0.150 M HCl(aq) is needed to neutralize all the NH3(g) from a 2.25 g sample of organic material, calculate the mass percentage of nitrogen in the sample.

A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation- reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCI from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution. A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the KOH solution if 13.2 mL of 1.50 M H₂SO4 was needed? The equation is 2KOH(aq) + H₂SO4 (aq)→K₂SO4 (aq) + 2H₂O(1) Express your answer with the appropriate units. ► View Available Hint(s) molarity = Submit…

The following chemical reaction takes place in aqueous solution: AgNO3(aq)+KCl(aq) → AgCl(s)+KNO3(aq) Write the net ionic equation for this reaction.

2 NaOH(aq) + H2C2O4 = 2H2O(s) Na2C2O4(aq) + 4 H2O(l)  Calculate the molarity of an oxalic acid solution if it takes 34.0 mL of 0.200 M NaOH solution to consume the acid in a 25.0 mL sample of this oxalic acid solution.

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 ?