a. Which phases are present? b. What is the complete composition of each of these phases? c. What is the weight amount of each of these phases?
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at 100C what is the maximum solubility (a) of Pb in Sn and (b) of Sn in Pb? The lead-tin phase diagram is shown in the animated figure
wt% Pb ?
wt% Sn ?
- In 1.00 atm of pure oxygen, the solubility of O2 (g) in water is 1.26*10-3 M at 25.0oC. The mole fraction of oxygen in air is 0.210. If the atmospheric pressure is 0.979 atm, what is the solubility of oxygen in air at 25oC? Answer is suppose to be 2.59*10-4 M, please show step by step.The solubility of CaSO4 is measured and found to be 0.689 g/L. Use this information to calculate a Ksp value for calcium sulfate. Ksp = ___________ (The attached picture is an example how to solve the given problems; The example's problem is The solubility of Ag2SO3 is measured and found to be 4.51x10-3 g/L. Use this information to calculate a Ksp value for silver sulfite.)1.0 GRAMS of an electrolyte was dissolved in 29 grams of water, the resulting solution was found to have a molarity of 0.437 mol / L. The freezing point of the solution was determined to be -4.96°C. The freezing point depression constant for water is -1.86°C and pure water may be assumed to freeze at 0°C. If the molecular weight of the electrolyte is 179.7 g/mol and it takes 15 minutes to perform the experiment, how much water was used (grams) ?
- Cyclonite, also known as RDX (Research Department Explosive), is used to make Semtex, a plastic explosive, when mixed with PETN. Semtex was used in the bomb that brought down PanAm flight 103 over Lockerbie, Scotland in 1988 killing 270 people. RDX is typically recrystallized from acetone. 1 gram of RDX is soluble in 100 mL of cold acetone (0 0C) and in 25.0 mL of boiling acetone. A student performed recrystallization starting with using 5.0 mL of acetone. a. What is the maximum amount of crude RDX the student can purify given this volume of acetone in order to maximize the % recovery? b. A student reported 65% recovery from the process of recrystallization after using 5.0 mL of acetone and the mass that can be used with that volume (part a). Is 65% the maximum % recovery of RDX using the volume you calculated in part a? Show your work.The solubility of BaF2 is measured and found to be 1.29 g/L. Use this information to calculate a Ksp value for barium fluoride. Ksp = _________ (The attached picture is an example how to solve the given problems; The example's problem is The solubility of Ag2SO3 is measured and found to be 4.51x10-3 g/L. Use this information to calculate a Ksp value for silver sulfite.)A) A saturated solution of CaCl2 in 100 gram of water at 20 0C is cooled to 5 0C. How much CaCl2 will precipitate out of solution? B) 50 gram NaCl is dissolved in 100 gram of water at 30 0C. The solution is
- The solubility of CO2 in water is a function of pressure.Calculate the concentration of CO2 in water when ???2 = 2.5 × 10−4 barI would like to calculate the molar solubility and Ksp from the following data: I have calculated them (see the solutions in the table) but, I am concerned that I have done the calculation incorrectly. See images for my calculations. These calculations are for Sample 1. Thank you! Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 23.59g 23.59g 23.60g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 26.62g 26.65g 26.69g Mass of Calcium Hydroxide Solution 3.03g 3.06g 3.09g Volume of Ca(OH)2 Density = 1.000 g/mL 3.03mL 3.06mL 3.09mL Concentration of HCl (M) 0.1M 0.1M 0.1M Initial HCl Volume in Syringe 1.00mL(1) 1.00mL(2) 1.00mL(3) 1.00mL(1) 1.00mL(2) 1.00mL(3) 1.00mL(1) 1.00mL(2) 1.00mL(3) Final HCl Volume in Syringe 0ml (1) 0ml (2) 0.65mL (3) 0ml (1) 0ml (2) 0.63mL (3) 0ml (1) 0ml (2) 0.63mL (3) Volume of HCl Delivered 2.35mL 2.37mL 2.37mL Moles of HCl Delivered…Got the Ksp values figured out i think, having trouble figuring out the solubility and trying to research online has made it more confusing as they have different ways to solve and they get different answers what is the correct way?
- Water is slightly soluble in liquid nitrogen. At-196°C(the boiling point of liquid nitrogen), the mole fraction of water in a saturated solution is 1.00 × 10-5 . Compute the mass of water that can dissolve in 1.00 kg of boiling liquid nitrogen.At 90°C, the vapor pressure of toluene is 0.534 atm and thevapor pressure of benzene is 1.34 atm. Benzene (0.400 mol)is mixed with toluene (0.900 mol) to form an ideal solution.Compute the mole fraction of benzene in the vapor in equilibrium with this solution.A. (see pic) B. When an electrolyte solution (such as NaCl) is added to ice, the ions have ____ with water molecules and thus ____ the ability of the water molecules to form a solid ice structure. C. Given that water's freezing pt is 0C and the fp depression constant is 1.86 Ckg/mol, calculate the fp depression for a 3.55 molal soln (moles/kg) of NaCl in water. Assume ideal behavior of the ions. D. Given that water's fp is 0C and fp depression constant is 1.86 Ckg/mol, calculate the fp depression for 3.55 molal solution for CaCl2 in water. Assume ideal behavior of the ions.