The concentration of ions in seawater is approximately the same as that in a solution containing 4.2 g of NaCl dissolved in 125 g of water. Assume that each of the ions in the NaCl solution has the same effect on the freezing point of water as a nonelectrolyte molecule, and determine the freezing temperature the solution (which is approximately equal to the freezing temperature of seawater).

The vapor pressure of pure water at 70°C is normally 233.7 mmHg, but decreased to 227.4 mmHg upon addition of an unknown amount of sodium hypochlorite, NaOCl, to 242.9 g of water at this temperature. How many grams of sodium hypochlorite were added? Assume complete dissociation of solute.

Use the References to access important values if needed for this question. An aqueous solution of phosphoric acid, that is 0.500 percent by weight phosphoric acid, has a density of 1.0010 g/mL. A student determines that the freezing point of this solution is -0.122 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of K1? Assume that only the first ionization of the acid is important. Ke for H,O is 1.86 °C/m. % ionized =

Calculate the boiling point of 0.150 m aqueous solutions of Mg(NO3)2

Determine the enthalpy of neutralization in Joules/mmol for a solution resulting from 19 mL of 0.9 M NaOH solution and 19 mL of a HCI with the same molarity. If separately, each had a temperature of 28.8 degrees Celsius, and upon addition, the highest temperature reached by the solution was graphically determined to be 37.8 degrees Celsius. Round to the nearest whole number.

At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm? solubility: M At 298 K, what is the solubility of oxygen in water exposed to air at 0.893 atm? solubility: M If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from 3.20 L of water in an unsealed container? amount: mol

The concentration of CaF2 in an aqueous solution is measured to be 0.056 M. Calculate the concentration of CaF2 in solution in units of ppm. Calculate the concentration of F- in the solution in units of ppb. Assume a density of 1.0 g/mL for this calculation.

3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small.   D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.

A sample of an ionic solid is dissolved in 1.00 kg of water. The freezing point of the water is -0.01 °C. If three times the mass of ionic solid is dissolved in 1.00 kg of water and the resulting freezing point of the solution is -0.09 °C, which of the following would be possible formulas for the solid: MX, MX2, or MX3, where M represents a metal cation and X an anion with a 1- charge? Explain your reasoning.

Assuming 100% ionized in solution, what would be the calculated freezing point of 0.10 m solutions in wqter of a NaCl solution and BaCl2 solution. If the actual freezing points are -0.348 °C for NaCl and -0.470 °C for BaCl2 , explain the difference between these values and the calculated freezing points.