A water contains the following: 3.13x10-4 mol L-' Mg2+; 8.48x10-4 mol L-1 Ca²+; and 2x10-6 mol L-! CO,2.. Determine whether this water is saturated with respect to dolomite (ignore activity coefficients). Ksp = 10-17.20 mol? L-2 SP
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- The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?* A 1.20 g sample of unknown compound is disolved in 50 g of CHe. The solution freezes at 4.92 C. Calculate the MW. (f.p of CH6= 5.48 C, K; of CHo=5.12 C/m)Use the thermodynamic data to calculate the vapor pressure (in kPa) of HNO3 at 25℃. HNO3(l) ---> HNO3 (g) so far I have: ∆G° = -RTlnKp Kp = P HNO3 ∆G°f (HNO3 (g))- ∆G°f (HNO3 (l)) = 7.2
- BINARY PHASE DIAGRAMS Please answer ALL parts with as much explanation as possible, showing full working out.a)(i) What is the melting point of pure Mg?(ii) What is the maximum solubility of Mg in Pb and at what temperaturedoes this occur? (b) A 50 wt.% Pb-50wt% Mg alloy is slowly cooled from 700 °C to 400 °C.(i) At what temperature does the first solid phase form?(ii) What is the composition of this solid phase?(iii) At what temperature does all the liquid solidify?(iv) What is the composition of the last remaining liquid phase?(v) What is the freezing range? (c) What is the mass fraction of solid and liquid of a 60 wt.% Mg alloy at atemperature of 500 °C.(d) Draw and label the microstructure of an 80 wt.% Mg alloy at 600 °C.(e) A Mg-Pb alloy of mass 5.5 kg has a composition just slightly below thesolubility limit of 200 °C.(i) What mass of lead is in the alloy?(ii) If the alloy is heated to 350 °C how much more lead can be dissolvedin the α phase without exceeding the solubility…A public water supply was found to contain 0.8 partper billion (ppb) by mass of chloroform, .(a) How many molecules would be present in a350 mL glass of this water? (b) If the in part (a)could be isolated, would this quantity be detectable onan ordinary analytical balance that measures masswith a precision of g?The solubility of Ni(OH)2 in water at 25c is measured to be 4.9 x 10^-4 g/L. Use this information to calculate Ksp for Ni(OH)2.
- An aqueous solution of acetic acid with a richness of 80% by passage (ρ = 1.07 kg/dm3) is available.a) What is the molarity and molality of this solution?b) What is the percentage of acid in this solution? c) What volume of said solution should we use to prepare 1 liter of 2.14M solution?A solution was prepared by dissolving 23.6 g of MgSO4 (80% dissociation) in 1.60 L of water MW MgSO4 = 120 g/n Calculate for the boiling point of the solutionArterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 ×× 10–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209. Part1:Calculate the solubility (in M) of O2 in the blood of a climber on Mt. Everest, where Patm = 0.35 atm.___M Part2: Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm.___M
- The maximum solid solubility of carbon in ferrite occurs at 0.022 wt% C and 727 ° C, the eutectoid composition is 0.76 wt% C, the maximum solid solubility of carbon in austenite occurs at 2.14 wt% C and 1147 ° C, and the cementite composition is 6.7 wt% C. For 2122 g of a 3.2134 wt% C steel at 726 ° C, what will be the mass of carbon present as part of a compound?(a) 67.9 g(b) 74.2 g(c) 58.7 g(d) 83.5 gThe 250-mL coke was then opened. Given the atmospheric pressure is 1 atm and volume percent of CO2 in air is 0.036%, what is the solubility of CO2 in the coke at 20 C after exposed to air? And what volume of CO2, measured at 20 C and 1 atm, has expelled after the coke has opened for a prolonged time?Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 × 10–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209. Calculate the solubility (in M) of O2 in the blood of a climber on Mt. Everest, where Patm = 0.35 atm. Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm.