Under a 25°C subsurface environment, the groundwater has reached equilibrium with soil minerals and pore gas. The pH of groundwater equals to 7.4. The major component of soil minerals is CACO3, with solubility constant pKso = 8.3. The partial pressure of CO2 in the pore gas is 0.2 atm. Determine [H2CO;], [HCO;], [CO;], [Ca"]. Give your %3D answers in molar concentration (M). Hints: Acid constants of H2CO3 at 25°C: pKal = 6.3; pKa2 = 10.3 Henry's constant for CO2 at 25°C: KH = 3.39*102 M/atm
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- You place a beaker containing 1 kg of water in contact with an atmosphere that has a CO 2partial pressure of 10 -2.5 atm and you allow free exchange of gas until equilibrium is established(remember K H =10-1.5 ), then you cap the solution and change the pH by titration. There is nosubsequent exchange of gas with the atmosphere.Please answer the following questions about the solution speciation:a) What is the mass balance equation for dissolved carbonate? Is this a closed or open system?One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.
- What is the maximum Ca2+ concentration (in mol L-1) of surface water in a lime quarry if the atmospheric CO2 concentration is 381 ppm at 1.00 atm? Assume the following simplified charge balance: 2[Ca2+] = [HCO3-]. Should correct.The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…
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