Sodium oxalate, Na2C2O4Na2C2O4, in solution is oxidized to CO2(g)CO2(g) by MnO−4MnO4− which is reduced to Mn2+Mn2+. A 50.3 −mL−mL volume of a solution of MnO−4MnO4− is required to titrate a 0.342 −g−g sample of sodium oxalate. This solution of MnO−4MnO4− is then used to analyze uranium-containing samples. A 4.60 −g−g sample of a uranium-containing material requires 33.0 mLmL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2UO2+→UO22+.     Part A Calculate the percentage of uranium in the sample.

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

The following chemical reaction takes place in aqueous solution: ZnBr₂(aq)+Na₂S(aq) → ZnS(s)+2 NaBr(aq) Write the net ionic equation for this reaction. 0 k

consider the reaction of rubidium metal with water to form aqueous rubidium hydroxide and hydrogen gas 2rb(s)+2h2o(l)->2rboh(aq) assign the oxidation state for each reaction

The calcium (40.078 g/mol) in a 500.0 mL sample of natural water was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed, and ignited in a crucible with an empty mass of 32.3555 g. The mass of the crucible plus CaO (56.077 g/moI) was 33.1471 g. A. Calculate the concentration of Ca in water in units of grams per 100 mL of the water. B. What is the molarity of Ca in the water sample?

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

In sediments and waterlogged soil, dissolved O2 concentrations are so low that the microorganisms living there must rely on other sources of oxygen for respiration. Some bacteria can extract the oxygen in sulfate ions, reducing the sulfur in them to hydrogen sulfide gas and giving the sediments or soil a distinctive rotten-egg odor.Write the net ionic equation for the reaction under acidic conditions (H3O+) that releases O2 from sulfate and forms hydrogen sulfide gas. Use water as the reactant in the half-reaction that describes the formation of oxygen.

Zinc metal reacts with nitric acid, HNO, to produce a number of products, depending on how dilute the acid solution is. In a concentrated salution, zinc reduces nitrate ion to ammonium ion; zinc is oxidized to zinc ion, Zn Write the net ionic equation for this reaction.

The standardized NaOH was used to determine the unknown concentration of H3PO4. The standard NaOH concentrtion is 0.126M. The standard sulfuric acid concentration is 0.150M. 3 NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3 H2O(l) Three flasks containing 25.00 mL H3PO4 each was titrated with NaOH. The data is below:                                    Titration 1       Titration 2.           Titration 3 Starting volume buret 2.62 mL           18.60 mL            1.20mL Buret volume at end 18.46 mL            34.40mL             16.84mL Calculate the concentration of H3PO4.

A student dissolved 0.3101 g of Na2C2O4 in 30 mL of water and 15 mL of 3 mol/L H2SO4. She titrated this solution with a KMnO4 solution. What was the molarity of the KMnO4 if it took 24.90 mL of titrant to reach a permanent pale pink equivalence point? The net redox reaction is 2 KMnO4 (aq) + 5 Na2C2O4 (aq) + 8 H2SO4 (aq) → 8 H2O (l) + 10 CO2 (g) + K2SO4 (aq) + 2 MnSO4 (aq) + 5 Na2SO4 (aq) (2 digit response) Answer: 0.037