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- KNO3 (aq) added to CaC2O4 (Ksp = 1.3 x 10-8) in solution will lead to __________ in solubility of the solid no effect then decrease increase no effectFor a solution containing 0.050 M sodium butanoate (the sodium salt of butanoic acid, butanoic acid can be found in appendix G). Calculate the fraction of association A)0.011%B)1.84%C)5.25%D)3.09%E)0.008% Do not give handwriting solution.The following reaction is the basis for automatized breath tests for the detection of alcohol(e.g. the Breathalyzer):C2H6O + Cr2O72- --> C2H4O2 + Cr3+ The Cr2O72- ions generate a reddish orange aqueous solution that changes to green as Cr3+ ions are produced due to the reaction with ethanol (C2H6O). If the concentration of the dichromate (Cr2O72-) solution is 0.5 M, theconcentration of Cr3+ is 0.1 M, the concentration of ethanol in the solution is1x10-4 M and the concentration of acetic acid (C2H4O2) is 1×10-4 M calculate the value of Ecell for this reaction at 298 K. The value of E0cell is 1.27 V.
- 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 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 osmotic pressure in atm to three decimal placesA 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 boiling 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. 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)In non-aqueous volumetric methods:I. Carbon dioxide and water is excluded to prevent these from reacting with the sample.II. The temperature is controlled to prevent loss of solvent.III. Samples are usually organic acids and organic bases which are weak electrolytes. I & III II only II & III I only I, II & IIIAn 7.50 ml aliquot of a 125 ppm stock Red 40 dye solution was diluted to a final volume of 25.0 mL with deionized water. What is the concentration of the dilute Red 40 dye solution (in ppm)? 37.5 ppm is the answer. (please show me how to calculate)