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- The solubility of silver chloride is 1.3 x 10-5 mol L-1. What is the Ksp for silver chloride at 25 °C?1.1The 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.4 mL of 5 x 10-3 M Fe(NO3)3 is added to 6 mL of 8x10-3 MKSCN along with 4 mL of water. The concentration of FeSCN2+ was found to be 3 x 10-4 at equililibrium. How many initial moles of Fe3+ are present in the solution? How many initial moles of SCN-are present in the solution? How many initial moles of FeSCN2+ are present?
- The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. 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 2.1? Explain you answer in a short sentence.2.3 - At temperature of 18°C was 4,7 g of silver molybdate (M = 376 g mol–1) mixed with 500 cm3 of a) distilled water b) solution of AgNO3 with concentration of 0,02 mol dm–3 c) solution of Na2MoO4 with concentration of 0,02 mol dm–3 Determine, how many percent of Ag2MoO4 will dissolve in each case. Solubility equilibrium of Ag2MoO4 is 3,1.10-11.
- The Ksp of Fe3(PO4)2 is 5.51⋅10-21 M. Calculate the solubility of Fe2+ and PO43- in a saturated solution.The Ksp of ZnCO3 (MM: 125.38) is 1.20 xx 10^(-10). a) What is the molar solubility of ZnCO3? b) What is the solubility of ZnCO3 in g/L?The Ksp value for the dissociation of barium sulfate (BaSO4) at 25°C is 1.08 x 10-10. How many milligrams (mg) of barium sulfate will dissolve in 1.43 L of pure water at this temperature? The molar mass of barium sulfate is 233.36 g/mol.
- Iodine dissolves in water, but its solubility in a nonpolar solvent such as CCl4 is greater Extracting iodine (I2) from water with the nonpolar solvent CCl4. I2 is more soluble in CCl4 and, after shaking a mixture of water and CCl4 , the I2 has accumulated in the more dense CCl4 layer. The equilibrium constant is 85.0 for the processI2(aq) ⇄ I2(CCl4) You place 0.0340 g of I2 in 100.0 mL of water. After shaking it with 10.0 mL of CCl4, how much I2 remains in the water layer?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 ×…The following synthesis reaction was conducted at 325K: A2(g) + 3B2(g) ⇌ 2AB3(g). At this temperature, KP = 5.49 x 10-6. In a 3.00L flask, 0.175atm of A2(g) and 0.410atm of B2(g) are added and allowed to reach equilibrium. Calculate the pressure of AB3(g) in the system (in atm).