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- According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?A student set up an experiment for six different trials of the reaction between 1.00-M aqueous acetic acid, CH3COOH, and solid sodium hydrogen carbonate, NaHCO3. CH3COOH(aq) + NaHCO3(s) NaCH3CO2(aq) + CO2(g) + H2O() The volume of acetic acid was kept constant, but the mass of sodium bicarbonate increased with each trial. The results of the tests are shown in the figure. (a) In which trial(s) is the acetic acid the limiting reactant? (b) In which trial(s) is sodium bicarbonate the limiting reactant? (c) Explain your reasoning in parts (a) and (b).applications of precipitation in chemistry?
- The concentration of arsenic in an insecticide can be determined gravimetrically by precipitating it as MgNH4AsO4. The precipitate is ignited and weighed as Mg2As2O7. Determine the %w/w As2O3 in a 1.627-g sample of insecticide that yields 106.5 mg of Mg2As2O7.6.) One way to determine the amount of nitrogen in a sample is through a method called Kjeldahl Method. In this method, the nitrogen in the sample is converted first to ammonium ions (N ? NH4+). The ammonium ions are then converted to ammonia by making the solution basic with the use of sodium hydroxide (NH4+ ? NH3). The ammonia produced is reacted with hydrochloric acid (NH3 +HCl ? NH4Cl). The unreacted hydrochloric acid is then titrated with standard sodium hydroxide solution. Using the method outlined, a 1-mL fish sample was analyzed. The liberated ammonia was collected in 100 mL of 0.0503 M HCl. The unreacted HCl then required 28.3 mL of 0.124 M NaOH for titration. Calculate the nitrogen in the sample as mg N/mL.Refer to the solubility graph, how much LiCl can be added in 150g H2O until it reaches its saturation point at 70C?
- ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2 (aq) + H2O (l) H2CO3 (aq) What would be the equilibrium constant expression (Kc) for this reaction?1. Consider the following reaction: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 A 5.0 L vessel contains 0.060 mol NO, 1.0 mol O2, and 0.80 mol NO2. Is this system at equilibrium? If the system is not at equilibrium, does the reaction proceed in the forward or reverse direction to reach equilibrium?
- Aluminum in the Al3 + form can be precipitated as Al (OH) 3, adding ammonia to an aluminum solution, but the precipitate is usually gelatinous and difficult to filter. Precipitation from a homogeneous solution provides a more filterable precipitate. The reaction used in this process is the hydrolysis of urea: (image attached) Suppose this reaction occurs in a 100.00 mL solution with an initial Al3 + concentration of 1.50x10-3 mol / L. How many moles of urea must be hydrolyzed to supply enough hydroxide to stoichiometrically combine Al3 + and form the precipitate Al (OH) 3?What is (are) the most likely product(s) for the following reaction? I || Br ||| IV OH HBr Br Br || V Br. Br |||Constants Periodic Table Hydrates are solid compounds that contain water molecules. When hydrates are heated, the water molecules evaporate, producing the anhydrous form of the compound. The formula of a hydrate may be written in two different ways. For example, aluminum chloride hexahydrate can be written as (Al(H2O)6]Cl3 or as AlCls 6H2O. The first formula more accurately shows the bonding arrangement, whereas the second formula makes it easier to see that the anhydrous form of the compound is aluminum chloride. Part B IF 12.0 g of MgSO4 - 7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain? Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) IA ? Value Units Submit Previous Answers X Incorrect; Try Again; 28 attempts remaining 3:18
