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How do you calculate KF factor using disodium tartarate dihydrate?
To calculate the KF factor using disodium tartarate dihydrate, you would need to first prepare a solution of known concentration of disodium tartarate dihydrate. Then, titrate this solution using Karl Fischer reagent until the endpoint is reached. Finally, use the volume of Karl Fischer reagent consumed and the known concentration of the solution to calculate the KF factor.
What concentration of aqueous NaOH solution freezes at -32 degrees Celsius the freezing point of pure water is 00 degrees and kf of pure water is -186 degrees Celsius over m?
We can use the freezing point depression formula: ΔTf = Kf * m. Given ΔTf = -32°C, Kf = -1.86 °C/m, and ΔTf = i * m * Kf in which i = 2 for NaOH. Rearranging the equation, we get m = ΔTf / (i * Kf) = (-32) / (2 * -1.86) = 8.6 mol/L. Therefore, the concentration of the NaOH solution is 8.6 mol/L.
What concentration of aqueous NaOH solution freezes at -3.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC m?
The change in freezing point is calculated as ΔTf = Kf * m, where Kf = -1.86°C/m for water. The change in temperature is -3.2°C - 0.0°C = -3.2°C. In this case, m = ΔTf / Kf = -3.2°C / -1.86°C/m = 1.72 m. Therefore, the concentration of NaOH solution is 1.72 mol/L.
How many moles of KF are contained in 347 g of water in a 0.175m KF solution?
This value is 0,06 moles.
How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?
The definition of 0.175 m KF is that 1 kg of water contains 0.175 moles of KF. Thus, 347 g of water is equivalent to 0.347 kg, and to find moles of KF, you calculate as follows:0.175 moles/Kg x 0.347 kg = 0.0607 moles of KF are present (3 significant figures).
How do you calculate KF factor using disodium tartarate dihydrate?
To calculate the KF factor using disodium tartarate dihydrate, you would need to first prepare a solution of known concentration of disodium tartarate dihydrate. Then, titrate this solution using Karl Fischer reagent until the endpoint is reached. Finally, use the volume of Karl Fischer reagent consumed and the known concentration of the solution to calculate the KF factor.
What is the molarity of a kf(aq) solution containing 116grams of kf in 1.00 liter solution?
The molar mass of KF is 58.1 g/mol. Given that there are 116 grams of KF in the solution, this corresponds to 2 moles of KF. Therefore, the molarity of the solution is 2 M.
What concentration of aqueous NaOH solution freezes at -32 degrees Celsius the freezing point of pure water is 00 degrees and kf of pure water is -186 degrees Celsius over m?
We can use the freezing point depression formula: ΔTf = Kf * m. Given ΔTf = -32°C, Kf = -1.86 °C/m, and ΔTf = i * m * Kf in which i = 2 for NaOH. Rearranging the equation, we get m = ΔTf / (i * Kf) = (-32) / (2 * -1.86) = 8.6 mol/L. Therefore, the concentration of the NaOH solution is 8.6 mol/L.
What concentration of aqueous NaOH solution freezes at -3.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC m?
The change in freezing point is calculated as ΔTf = Kf * m, where Kf = -1.86°C/m for water. The change in temperature is -3.2°C - 0.0°C = -3.2°C. In this case, m = ΔTf / Kf = -3.2°C / -1.86°C/m = 1.72 m. Therefore, the concentration of NaOH solution is 1.72 mol/L.
What concentration of aqueous NaOH solution freezes at -3.2C The freezing point of pure water is 0.0C and Kf of pure water is 1.86Cm?
0.86m
The solution has a freezing point of -2.79 . The freezing point depression constant for water is 1.86 K m-1. What is the nitrate concentration in the solution?
To find the nitrate concentration in the solution, you can use the formula: ΔTf = Kf * m, where ΔTf is the freezing point depression (-2.79°C), Kf is the freezing point depression constant (1.86 K m^-1), and m is the molality of the solution. Calculate the molality of the solution and then convert it to nitrate concentration using the molecular weight of the nitrate ion.
What is the experimentally determined concentration of particles for an 2.25 molal solution of an ionic substance in water if the boiling point of the solution is 100.3 oC?
The experimentally determined concentration of particles for a 2.25 molal solution can be calculated using the formula: ΔTb = i * Kf * molality, where ΔTb is the boiling point elevation, i is the Van't Hoff factor, Kf is the ebullioscopic constant for water (0.512 oC/kg/mol), and molality is 2.25 mol/kg. From the given values, you can solve for the Van't Hoff factor (i) to determine the concentration of particles in the solution.
What concentration of aqueous NaOH solution freezes at -3.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºCm?
0.86 m
What is the molarity of KF solution containing 116 g of KF in 1.00 L?
The molar mass of KF is approximately 58.10 g/mol. To calculate the molarity, divide the given mass of KF (116 g) by its molar mass to get moles, then divide by the volume (1.00 L) to get the molarity. The molarity of the KF solution is approximately 2.00 M.
What concentration of aqueous CaCl2 solution freezes at -10.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC m?
To calculate the molality of the solution, we first need to determine the change in freezing point. ΔTf = 0.0°C - (-10.2°C) = 10.2°C. Next, use the formula ΔTf = Kf * m to find molality. Rearrange the formula to solve for molality: m = ΔTf / Kf = 10.2°C / 1.86°C m^-1 = 5.48 m. Thus, the concentration of the solution is 5.48 mol/kg.
What is the boiling point of a 2.35 m solution of sodium sulfate?
The boiling point of a solution increases with the concentration of solute particles. To calculate the boiling point elevation, you can use the formula: ΔTb = i * Kf * m, where i is the van't Hoff factor (2 for sodium sulfate), Kf is the ebullioscopic constant, and m is the molality of the solution. If you have these values, you can calculate the boiling point elevation using this formula.
How many moles of KF are contained in 347 g of water in a 0.175m KF solution?
This value is 0,06 moles.
