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A: [Ba(NO3)2] = 0.06 M Ksp = 1.57 X 10-9
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A: molar solubility of Ag2C2O4 = 2.06×10-4 mol/liter.
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Q: Calculate the solubility at 25 C of AgCl in pure water and in a 0.0070 M AgNO3 solution. Ksp= 1.77 x…
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Q: Explain the common-ion effect.
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Q: Calculate the mass solubility of Ag2CO3 (Ksp= 8.1 x 10^-12, MM = 275.74 g/mol) in a 0.010 M AgNO3…
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Q: Calculate the mass solubility of AgCO (K = 8.1 x 10, MM = 275.74 g/mol) in a 0.010 M AgNO solution…
A: The compound is actually Ag2CO3(s) with Ksp = 8.1*10-12 The other compound is AgNO3. Since AgNO3…
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Calculate the solubility of copper(I) sulfide (Cu2S, Ksp = 2.26 × 10−48) in a 0.010 M CuC2H3O2(aq) solution. (C2H3O2− = acetate)
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- What would be the KPs value of Al(OH)3, considering that its solubility is 2,5 x 10^-8 mol/L?How do you find the solubility constant for Al(OH)3, MnS, and Ca3(PO4)2?Calculate the solubility of lead iodate (Pb(IO3)2, Ksp = 3.68 x 10-13).... (a) ... in pure water (b)... in a 0.100 M (Pb(NO3)2 (aq) solution
- The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?As part of the analysis of water samples, the hardness of water is commonly measured and calculated. It is commonly expressed in ppm by mass (parts per million) of CaCO3. Parts per million is also equivalent to milligrams of CACO3 per liter of water. In a sample taken by an environmentalist, he was able to observe a hardness count of 205 mg CacO3/L. Given this hardness count of the sample, what is the molar concentration of Ca2+ ions in the water sample?The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?
- The equilibrium constant for the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g) is K = 1.03 × 105 at 298.15 K. Calculate the standard reaction Gibbs energy at this temperature.Assume that the solubility of carbon dioxide gas in pop at 5oC is 0.586 g/100 mL and at 20oC its solubility is 0.169 g/100 mL. What mass of carbon dioxide gas will escape from a 355-mL can of Coke that has been taken out of the fridge and has been sitting open at 20oC?The standard reaction Gibbs energy for the reactionH2(g) + (1)/(2)O2(g) → H2O(I) is -237.13 kJ mol-1 at 25 °c. Determine the equilibrium constant in terms of concentration, Kc, at this temperature.
- Calculate the Molar Solubility at 25.0 oC of an aqueous solution of calcium phosphate, Ca3(PO4)2, given that its Ksp = 1.20 x 10–26 at 25.0 oC.Calculate the mass solubility of AgCO (K = 8.1 x 10, MM = 275.74 g/mol) in a 0.010 M AgNO solution (AgNO is highly soluble in the water)The solubility of lead(II) fluoride, PbF2, in pure water is 2.1 × 10–3 moles per liter. Calculate the value of Ksp for lead(II) fluoride from this data.