Copper(I) ions in aqueous solution react with NH, (aq) according to Cu* (aq) + 2 NH,(aq) Cu(NH,) (aq) Kr = 6.3 x 1010 Calculate the solubility (in g-L) of CuBr(s) (Kp = 6.3 x 10-9) in 0.50 M NH, (aq). %3D solubility of CuBr(s): Question Source: MRG - General Chemistry Publisher: University
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- The concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q) Ksp = [Ba2+][NO3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPaIn an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(??3)2(?) ⇄ ??2+(?q) + 2??-3(?q) ??p = [??2+][??3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPa
- In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15oC. Barium nitrate dissociates via the process: Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q) Ksp = [Ba2+][NO3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPaOne mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will formCalculate 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: gL
- 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 solutionThe 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 mLIn the interface between sediment and water around a deep lake bottom, dissolved oxygen (DO) is usually low. Under such a condition, iron and sulfur typically exist in their reduction forms (i.e. Fe2+ and S2-). Fe2+ and S2- can readily react with each other to produce ferrous sulfide (FeS), which is a black solid substance and finally settles down into the sediments at the lake bottom. The solubility product constant (i.e. equilibrium constant) of FeS is 8 x 10-9. At a chemical equilibrium state, what is the concentration of S2- in the water nearby the sediments if Fe2+ concentration in water is 10 - 4 M.
- 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.On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) + S2(g)was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0L vessel.Calculate the equilibrium constant, Kc, for this reaction.