A student measures the molar solubility of copper(II) carbonate in a water solution to be 1.64x10 M. Based on her data, the solubility product constant for this compound is
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Q: A student measures the molar solubility of nickel(II) cyanide in a water solution to be 1.91×108 M.…
A: Answer: the solubility product constant for this compound is 2.787 × 10-23.
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A: The solubility product constant, (Ksp) , is the equilibrium constant for a solid substance…
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A: Given, [Mg] = 0.00632 M [CO32- ] = 0.00633 M
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A: Ksp is the solubility product constant, which indicates the dissolution of solute in a solution.…
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A: Given that: Molar solubility of barium sulfite (s)= 8.70×10-4M
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A: Solubility gives the tendency of the substance to get dissolve. Solution has two parts: solute and…
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A:
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A: The solubility of a sparingly soluble salt is directly influenced by the formation of complex ion in…
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Q: ) You are doing an experiment to measure the solubility product constant of lead(II) chromate…
A: We have to write the balance solubility reaction for lead chromate .
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Q: Silver halides show the following solubility trend in water: AgF > AgCl > AgBr > AgI, explain.
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Q: The molar solubility of magnesium hydroxide in a 0.280 M magnesium acetate solution is М.
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Q: solubility
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Q: At a certain temperature, the solubility of BaF, is 7.4 x 103 moles per litre. Calculate the Ksp of…
A: To solve this problem we will use given solubility of BaF2 .
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A: Given, molar solubility of silver iodide in water solution =1.19×10-8 Mwe are asked to calculate the…
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A: The molar solubility of lead phosphate is = 7.85×10-10 M The solubility product constant for this…
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A: GIVEN: Molar solubility of lead phosphate is 7.84 x 10-10 M formula of lead phosphate Pb3(PO4)2…
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A: Molar solubility directly related to solubility product. For two ions molecules Ksp = S2 for three…
Q: A student measures the molar solubility of silver sulfite in a water solution to be 1.58×10-³ M.…
A: The answer to the following question is -
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A:
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A: Barium phosphate has the formula as Ba3 (PO4)2 has solubility, S = 6.45 × 10-7 M
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A:
Q: A student measures the molar solubility of zinc hydroxide in a water solution to be 2.18×106 M.…
A: Concentration of Zn(OH)2 is 2.18×10-6 M. Zn(OH)2 dissociates as: Zn(OH)2⇌Zn2++2OH- Solubility…
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A: A. The molar solubility can be calculated as,
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- . What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.Solid ammonium chromate is slowly added to 75.0 mL of a calcium acetate solution until the concentration of chromate ion is 0.0154 M. The maximum amount of calcium ion remaining in solution is M. Please answer asap Thanks!A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show work
- Did the solubility of the salt increase or decrease with temperature? Why? Hint: consider the thermodynamic properties of the dissociation reaction). LeChatlier's principle should appear in your answer. first temperature: 19.5 C and Ksp : 2.043E-5 second temperature 84.5 C and Ksp: 2.050E-51. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 3. Express the solubility (S) in question #2 in g/L. 4. Calculate Ksp for the ff. substances, given the molar concentration of their saturated solution. a. Ag2C2O4 ( S= 2.06 x 10-4 ) b. Al(OH)3 ( S = 1.82 x 10-9 ) 5. Calculate the molar solubility of the salts in problem #2 for the solution in which the cation concentration is 0.050 M.In 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.
- In a saturated solution of MgF2 at 18°C, the conctration of Mg2+ is 1.21*10^-3 molar. a)Write the expression for the solubility product constant also and calculate its value at 18°C. B)calculate the equilibrium concentration of Mg2+ in 1.000 liter of saturated MgF2 solution at 18°C to which 0.100 mile of solid KF has been added. The KF dissolved completely. Assume the volume change is negligible.TypeFormulaKsp Solubility Product Constants (Ksp at 25 oC) TypeFormulaKspBromidesPbBr26.3 × 10-6AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9CaCO33.8 × 10-9CoCO38.0 × 10-13CuCO32.5 × 10-10FeCO33.5 × 10-11PbCO31.5 × 10-13MgCO34.0 × 10-5MnCO31.8 × 10-11NiCO36.6 × 10-9Ag2CO38.1 × 10-12ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5AgCl1.8 × 10-10ChromatesBaCrO42.0 × 10-10CaCrO47.1 × 10-4PbCrO41.8 × 10-14Ag2CrO49.0 × 10-12CyanidesNi(CN)23.0 × 10-23AgCN1.2 × 10-16Zn(CN)28.0 × 10-12FluoridesBaF21.7 × 10-6CaF23.9 × 10-11PbF23.7 × 10-8MgF26.4 × 10-9HydroxidesAgOH2.0 × 10-8Al(OH)31.9 × 10-33Ca(OH)27.9 × 10-6Cr(OH)36.7 × 10-31Co(OH)22.5 × 10-16Cu(OH)21.6 × 10-19Fe(OH)27.9 × 10-15Fe(OH)36.3 × 10-38Pb(OH)22.8 × 10-16Mg(OH)21.5 × 10-11Mn(OH)24.6 × 10-14Ni(OH)22.8 × 10-16Zn(OH)24.5 × 10-17IodidesPbI28.7 × 10-9AgI1.5 × 10-16OxalatesBaC2O41.1 × 10-7CaC2O42.3 × 10-9MgC2O48.6 × 10-5PhosphatesAlPO41.3 × 10-20Ba3(PO4)21.3 × 10-29Ca3(PO4)21.0 × 10-25CrPO42.4 × 10-23Pb3(PO4)23.0 × 10-44Ag3PO41.3 × 10-20Zn3(PO4)29.1 ×…One 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 form
- Calculate the molar solubility (moles/L) of CaF2 in water. And also calculate the solubility of CaF2 in water in grams/L. Ksp = 5.3 x 10^-11. b). Calculate the solubility of CaF2 in moles/L and in grams/L in a solution that already contained 0.010 M F-.Answer the following question. Download the answer sheet for this activity. For problem solving, show your solution. Final answers must be encircled and must have the correct number of significant figures. 1. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. CuCO3 Ksp = 2.5 x 10-10 b.Mg(OH)2 Ksp = 2.0 x 10-13 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. CuCO3 Ksp = 2.5 x 10-10 b. Mg(OH)2 Ksp = 2.0 x 10-13 3. Express the solubility (S) in question #2 in g/L.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: gL
