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Develop the solubility diagrams for CuCO3 in a closed system and an open system, respectively. Please provide rationale or workings for your answer.
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- I 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…How come we are not looking at the solubility data for hot and room temperature for part a and b?The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
- Calculate the solubility at 25°C of CuBr in pure water and in a 0.0100M CoBr2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0100 M CoBr2solution: gLCalculate the solubility at 25°C of CoOH2 in pure water and in a 0.0100M CoCl2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0100 M CoCl2 solution: gL(a) Derive an expression for the ratio of solubilities of AgCI at two different temperatures; assume that the standard enthalpy of solution of AgCI is independent of temperature in the range of interest. (b) Do you expect the solubility of AgCI to increase or decrease as the temperature is raised?
- At a certain temperature, the solubility of zinc(I) chromate is (7.6x10^-5) M. What is the Ksp? Report your answer to 2 sig figs. Note: Your answer is assumed to be reduced to the highest power possible1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0180M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. ksp for Ba Cr04 =1.17×10−10 Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0180 M BaCl2 solution: gL
- What sorts of additional interactions are taken into account when doing solubility calculations with activities, as opposed to those calculated only using molarities?Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is a consumption of 8 mL, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) Solubility of benzoic acid at 27 ° C .................................................; b) solubility of benzoic acid at different temperature ................................................; c) second test temperature ....................................................... (M (benzoic acid): 122.12 g / mol) Note: enter only required numerical values and units in the spaces in the question.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)