The conversion of nitrogen to ammonia, an essential process in the nitrogen cycle, occurs only in the presence of an iron-molybdenum cofactor. The concentration of molybdenum in one such co-factor was determined by titration with an acidified permanganate solution. The titration reaction equation is 4H*(aq) + 3MnO (aq) + 5Mo³+ (aq) → 3Mn²+ (aq) + 5M002+ (aq) + 2H₂O(1) A 30 mL sample of Mo³(aq) required 21.8 mL of 0.10 mol/L permanganate solution to reach a light pink end point. From the titration data, the concentration of Mo³+ (aq) is determined to be Record your answer to 2 sig-digs; do not include units. mol/L.

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

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For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concrete

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

Potassium hydrogen phthalate (KHP, HC8H4O4K) is used to standardize sodium hydroxide. If 25.00 mL of NaOH (aq) is required to titrate 0.8500 g KHP to the equivalence point, what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HC8H4O4-(aq)  +  OH-(aq)  →  C8H4O42-(aq)  +  H2O

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.

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.