What is the solubility of carbon dioxide (in units of grams per liter) in water at 25 °C, when the CO, gas over the solution has a partial pressure of 0.337 atm? ky for CO, at 25 °C is 3.36x102 mol/L atm.
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- 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) ?A batch of 500 ?? of ??? dissolves in water to form a saturated solution at 350 ? (77 °?) where the solubility is 30% by weight of ??? in water. The solution cools at 293 ? (20 °?) at which the solubility is 25.4% by weight. Determine the number of crystals obtained if 3.5% of the original water evaporates on cooling. Also, determine the capacity of the container in which this solution is cooled if it is 1.20 times the volume of the solution. The density of the solution is ???? ??/??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 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?279.28 mL of 1.22 M organic salt was mixed with 168.14 mL of Ethanol (d= 0.789 g/mL, MW 46.07g/mole). Pure ethanol has a vapor pressure of 0.059 atm what will be the vapor pressure of the solution?100ml of sodium hydroxide solution is required 20ml of 0.5 N sulfuric acid solution to neutralize it. Calculate the amount of sodium hydroxide or percent purity. (mwt of sulfuric acid is 98g/mole)
- The volume over the solution in the container is 122mL. Calculate the partial pressure of the hydrogen gas inthis volume at 25 °C, ignoring any solubility of the gas inthe solution. (c) The Henry’s law constant for hydrogenin water at 25 °C is 7.8 * 10-4 mol>L@atm. Estimate thenumber of moles of hydrogen gas that remain dissolvedin the solution. What fraction of the gas molecules in thesystem is dissolved in the solution? Was it reasonable toignore any dissolved hydrogen in part (b)?The colloidal particles has tenth ofmm diameter and easily filtered tru or falseA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)The freezing point of a 0.100 M acetic acid (CH3COOH) solution is determined to be-0.1878 C. Estimate the percent dissociation of acetic acid in this solution. Is it a strong orweak electrolyte? Note that acetic acid produces acetate (CH3COO-) and hydrogen (H+) ionswhen it is dissolved in water.