Calculate the solubility at 25 °C of Zn(OH), in pure water and in a 0.0180M ZnSO, solution. You'll find Ken data in the sp ALEKS Data tab. Round both of your answers to 2 significant digits. 믐 solubility in pure water: solubility in 0.0180 M ZnSO4 solution: :
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- 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: gL1.1The 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.
- Estimate the aqueous gram-solubility in g/L of mercury(I) chloride: Hg2Cl2(s) ↔ 2Hg+ (aq) + 2Cl– (aq), Ksp = 1.43×10–18 The molar mass of Hg2Cl2 is 472.06 g/mol.Calculate the solubility at 25°C of ZnOH2 in pure water and in a 0.0170M ZnSO4 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits.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
- Consider a body of water in equilibrium with solid calcium sulfate, CaSO4, for which Ksp = 3.0 * 10^-5 at 35 degrees C. Calculate the solubility, in g/L of calcium sulfate in water assuming that other reactions are negligible.The solubility of ZnS(s) in water at a certain temperature is 1.4 × 10–11 mol/L, i.e., x or the [Zn+2]=[S-2]. The value of the Ksp of ZnS isDetermine the molar solubility of CaF2 in a 0.10 M CaCl2(aq) solution. Clearly identify any assumptions/approximations that you make.
- Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte.found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs:CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac)and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte. found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs: CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac) and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.Write an appropriate expression for the solubility product of the sparingly soluble compound Ca(OH)2 Given the solubility product, Ksp, of Ca(OH)2 is 5.3x10-5M3 at 25oC, calculate its solubility at this temperature in Water 25 M CaCl2 solution