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The solubility of KI is 144.0 g per 100 g H₂O at20degrees celcius, and the density of the saturated solution is1.70 g/ml. Calculate the molarity of a standard solution of KI.

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The equilibrium constant for I2(ag)+ I- (ag)=&gt;I3- (aq) may also be found by measuring two solubilities. The solubility of I2 (s) in .100 M NaN03 solution at 25 degrees celcius , where no complexes are formed, is .00131 moles per liter. The solubility of I2 (s) in .100 M KI solution at 25 degrees celcius is .05135 moles per liter. The .1 M NaN03 provides the same ionic environment as .1 M KI. From this information calculate the concentration of I3-, I-, I2 in the latter solution and then calculate K1.

What is the molarity of a saturated solution of potassium sulfate (K2SO4) if the solubility is13 g per 100 g H2O at 25Â°C? The density of the solution is 1.1 g/mL

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Part A: In lab, 74.42 grams of H₂O is saturated with KNO₃ at 75.0ÂºC where the solubility is 145 g KNO₃/100 g H₂O. It is then cooled to 20.0ÂºC where the solubility is 35g KNO₃/100 g H₂O. How many grams of KNO₃ will precipitate out of the solution? Put your answer in 3 significant figures.

âPart B: What is the molarity of a solution that has 55.78 g KNO₃ dissolved in 100 g of water at 45ÂºC and a solution density of 1.23 g/ml. Put your answer in 3 significant figures.

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The solubility of KI is 144.0 g per 100 g H₂O at20degrees celcius, and the density of the saturated solution is1.70 g/ml. Calculate the molarity of a standard solution of KI.

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The solubility of KI is 144.0 g per 100 g H2O at20degrees celcius, and the density of the saturated solution is1.70 g/ml. Calculate the molarity of a standard solution of KI.

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

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The solubility of KI is 144.0 g per 100 g H₂O at20degrees celcius, and the density of the saturated solution is1.70 g/ml. Calculate the molarity of a standard solution of KI.