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The balanced equation for the neutralization reaction of aqueous \\(\ce{H2SO4}\\) with aqueous \\(\ce{KOH}\\) is shown.
$$\ce{H_2 SO_4 (aq) +2KOH (aq) -> 2H_2 O (l) +K_2 SO_4 (aq) }$$
What volume of \\(0.340\\) M \\(\ce{KOH}\\) is needed to react completely with \\(15.7\\) mL of \\(0.215\\) M \\(\ce{H2SO4}\\)?
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- A 100-liter empty jar was spiked with 20 mg of TCE (C2HCl3) under room temperature condition. The jar was then closed tightly. What is the concentration (in atm.) of TCE in the air at 25 C? (TCE: MW: 131.4 g/mol; TCE solubility in water (Cs) = 1100 mg/L; Pv (pure liquid at 25oC) = 10^-1.01 atm. KH = 10^1.03 L atm mol-1; KOW = 102.42). if the jar was half filled with water and half filled with air, what were the concentrations of TCE in both air and water at 25C?An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. From the stock solution (0.020 M), pipet 4.00 mL and dilute to 100.00 mL. From the diluted solution, pipet 0.00, 1.00, 1.50, 2.00, 2.50, 5.00 and 7.50 mL aliquots into 100 mL volumetric flasks. Dilute to mark. Determine the concentration of each standard solution and tabulate.
- Solution and explanation for Percentage Yield and Theoritical Yield for this data (Synthesis of Aspirin) Salicylic acid - 1.950 g Labeled watch glass - 50.664 g Labeled watch glass & piece of filter paper together - 50.872 g filter paper only - 0.208 g Where the data is from: https://youtu.be/tLXljLxRZ0U Room temperature - filter paper, watch glass and aspirin - 53.088 gThe bisulfate (or hydrogen sulfate) anion, HSO4 , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO4 (ag) = H* (ag) + SO,2- (ag) is 1.2 x 10-2 (a) Calculate AG° for this equilibrium. Assume a tempera- ture of 25.0°C. (b) At low concentrations, activity coefficients are approxi- mately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010-molal solution of sodium hydrogen sulfate.a 25.00 mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.00 mL aliquots of the diluted solution required an average of 34.88 mL of 0.09600 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid (MM:60g/mol). Consider the correct significant figures of your answer and do not forget the unit.
- Electrolytic manganese dioxide can be prepared from manganese carbonate ore by crushing,milling and leaching the ore in sulphuric acid. Manganese sulphate is crystallised from thesolution, redissolved and electrolysed to give the manganese dioxide.If the crystallisation were performed in a 30m3 tank and the concentration of the solutionentering the tank were 160 grams per litre and left the tank at 40 grams per litre, how muchMnSO4.5H2O would be produced.It is known that acid content has a major effect on theflavor of vinegars, but most cheaper vinegars are diluted similarly to 5% acidity Wt./vol. % is equivalent to gsolute per 100mL solution (so 5% is equivalent to 5 g acid/100 mL solution). a.) First, calculate the approximate molar concentration of acetic acid in the 5% wt./vol vinegar. b.) Next, calculate the expected molarity of acetic acid in the solution upon dilution by a factor of 5. Thank you!By pipet, 15.00ml of the stock solution of potassium permanganate (KMn04) that was prepared by dissolving 13.0g KMn04 with DI H20 in a 100.00ml volumetric flask, diluting to the calibration mark was then transferred to a 50.00ml volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.
- A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.A spent 1.0 percent caustic soda solution (ρNaOH = 8.42 lb/gal) with a volumetric flow rate of 3.0gpm is to be neutralized using either sulfuric acid or hydrochloric acid. First, determine the massflow rate (lb/day) of NaOH in the spent caustic soda solution, and then use that value todetermine the stoichiometric amounts (lb/day) of:1. H2SO4 required for neutralizing the OH− ions contributed by the spent caustic soda.[Hints: (1) write the balanced chemical equation for the acid-base reaction betweenNaOH and H2SO4, and use it to establish the stoichiometric weight ratio H2SO4 : NaOH.]2. HCl required for neutralizing the OH− ions contributed by the spent caustic soda. [Hints:(1) write the balanced chemical equation for the acid-base reaction between NaOH andHCl and use it to establish the stoichiometric weight ratio HCl : NaOH.]If one mixes 50cm³ of EtOH and 50cm³ of H2O at room temperature; will the total volume of the solution be 100.0 cm³? Justify answer with appropriate calculations and explanations