As2O3(s) reacts with NO3 – (aq) to produce NO(g) and H3AsO4(aq) When As2O3(s) was added to 27.50 mL of Solution B, 1.710 × 1021 molecules of NO(g) were obtained from the reaction in 88.75% yield. (a) If As2O3(s) was the limiting reactant, calculate the mass of As2O3(s) which reacted  with NO3

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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

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

A sample of iron ore is dissolved in acid, and the iron is converted to Fe2*. The sample is then titrated with 47.20 mL of 0.02240 M MnO4 solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) + 4H2O How many moles of MnO4¯ were added to the solution? Blank 1 2+ How many moles of Fe were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer Blank 4 Add your answer

To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a 4.20 g sample of the shell to a fine powder and titrates it to the endpoint with 302. mL of 0.210M hydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCl(aq) + CO3(aq) → H₂CO3(aq) + 2Cl¯ (aq) 1 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 CaCO3 in the sample. Be sure your answer has 3 significant digits. precipitation O acid-base O redox 0 0 0 п% X

Lead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction Pb(NO,),(aq) + 2 NH,I(aq) PbI, (s) + 2 NH,NO; (aq) What volume of a 0.170 M NHẠI solution is required to react with 119 mL of a 0.340 M Pb(NO3)2 solution? volume: mL How many moles of PbI, are formed from this reaction? moles: mol Pbl2 Aa A étv MacBook Air DD F12 DII F11 • F9 F10 80 888 F8 F7 F6

KSCN(aq) + Ag+(aq) → AgSCN(aq) + K+(aq)   By calculation she determines the buret delivered: 6.52108 moles of KSCN. The moles of Ag+ which were present in her sample was:

6 a b U d [Tutorial: Titration stoichiometry] This question will walk you through the steps of calculating the volume of titrant required to reach the endpoint based on the volume and concentration of analyte. Consider the standardization of NaOH by titration with C,H,O, according to the following chemical reaction: 3 NaOH(aq) + C,H,O,(aq) = Na,C,H,O,(aq) + 3 H₂O(l) Step 1: Evaluate the question. How many moles of aqueous sodium hydroxide (NaOH) will react to completely neutralize one mole of aqueous citric acid (C,H,O,)? Which equation will be most helpful for solving this problem? Calculate the volume in mL of a 0.200 M NaOH solution needed to neutralize 345 mL of 0.033 MC,H,O, standard solution. Based on the fact that NaOH is a strong base and C,H,O, is a weak acid, how would you describe the pH of the solution at the endpoint, where moles of base = 3 times the moles of acid?