Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation   MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g)   How much MnO2⁢(s) should be added to excess HCl(aq) to obtain 335 mL Cl2⁢(g) at 25 °C and 1.00×102 kPa ? mass: ______g MnO2

Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.(a) Mg(OH)2(s) + HClO4(aq) ⟶(b) SO3(g) + H2 O(l) ⟶ (assume an excess of water and that the product dissolves)(c) SrO(s) + H2 SO4(l) ⟶

To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid to a 42.0 g sample of the solution and titrates it to the endpoint with 103. mL of 0.2200M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 2+ 6H* (aq) + 5H₂O₂(aq) + 2MnO4(aq) 2 MnO (aq) 50₂(g) + 2Mn² (aq) + 8H₂0 (1) - O precipitation What kind of reaction is this? O acid-base O redox Ś ? do 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. 0 0 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 3 significant digits. 0% X KI

The mercury in a 1.9458 g sample was precipitated as Hg5(IO6)2  by treatment with an excess of paraperiodic acid, H5IO6: 5 Hg+ (aq)    +          2 H5IO6 (aq)         à         Hg5(IO6)2 (s)     +          10H+(aq) After filtration, washing and drying, 0.5218 g of the precipitate was recovered. A.) Calculate the percentage of Hg2Cl2 in this sample. B.) What is the gravimetric factor in the problem?

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?

if 30.0 g of NaOH is added to  0.800L of 1.00M Zn(NO3)2, what is the mass in grams of Zn(OH)2 will be formed in the precipitation reaction? 2 NaOH (aq) +Zn(NO3)2 (aq) = Zn (Oh)2 (s) + 2 NaN)3 (aq)?

Na2CO3(aq)  +  2  HCl(aq)  →   2 NaCl(aq)  +  CO2(g)  +  H2O 0.176 g of sodium carbonate required 33.34 mL of an HCl solution to completely react the Na2CO3 ? What is the molarity of the HCl solution?

A 20.0 mL sample of an unknown HClO4HClO4 solution requires 45.3 mL of 0.105 MM NaOHNaOH for complete neutralization. What was the concentration of the unknown HClO4HClO4 solution? The neutralization reaction is HClO4(aq)+NaOH(aq)→H2O(l)+NaClO4(aq)HClO4(aq)+NaOH(aq)→H2O(l)+NaClO4(aq). answer needs to be in L

Please answer the question in the image with details.

Apply the concepts of stoichiometry and solution concentration in this section.  Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction 2 KI (aq)  + Pb(NO3)2 (aq)       KNO3 (aq)    +  PbI2 (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO3)2 solution?           An solution is made by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution,                          Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)