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 2S₂O3(aq) + (aq) → SO2 (aq) +31 (aq) Given that it requires 31.9 mL of 0.210 M Na₂S₂O, (aq) to titrate a 10.0 mL sample of 15 (aq), calculate the molarity of 15 (aq) in the solution. (5)= x10 TOOLS M

The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 5.43 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCI(aq) and passed over a reducing agent so that all the antimony is in the form Sb³*(aq). The Sb³+(aq) is completely oxidized by 28.0 mL of a 0.110 M aqueous solution of KBrO, (aq). The unbalanced equation for the reaction is Bro, (aq) + Sb³+(aq) → Br (aq) + Sb3+ *(aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: percentage of antimony: %

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

Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 539 g NaOH(s)539 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq)NaOH(aq) solution.

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

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.3600M silver nitrate AgNO3 solution to a 24.00g sample of the fluid and collects the solid silver chloride AgCl product. When no more  AgCl is produced, he filters, washes and weighs it, and finds that 1.28g has been produced. The balanced chemical equation for the reaction is: Cl−(aq) + AgNO3(aq) -> AgCl(s) + NO−3(aq) 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 Cl in the sample. Be sure your answer has the correct number of significant digits.

By titration, it is found that 39.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

Calculate the number of milliliters of 0.689 M NaOH required to precipitate all of the A1³+ ions in 163 mL of 0.784 M Al2(SO4)3 solution as Al(OH)3. The equation for the reaction is: Al2(SO4)3 (aq) + 6NaOH(aq) → 2Al(OH)3 (s) + 3Na2SO4 (aq) Volume = | mL

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.

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