What is the boiling point of a mixture composed of 75.0 g HOCH2CH2OH (ethylene glycol) and 165 g H2O? The boiling point elevation constant for H2O is 0.512 °C/m.

Consider the graph below that displays the solubility of KCI in water as a function of temperature. 50 g of KCI is mixed with 100 g of water at 25 °C and is then heated to 50 °C. Select which statement best describes what would be observed as the system proceeds to establish equilibrium. 100 Solubility (g per 100 g H₂O) 80 60 40 20 0 20 KCI 40 60 Temperature (°C) 80 100 O a. A homogeneous solution of hydrated ions is initially observed, when a further 10 g of KCI is added, some of the added KCI is observed to dissolve, but some of the additional KCI remains in solid form. O b. A heterogenous system involving an equilibrium between hydrated KCI ions and solid KCI is observed. O c. A homogeneous solution of hydrated ions is initially observed, when a further 1 g of KCI is added, this additional KCI is also observed to dissolve. O d. A homogeneous solution of hydrated ions is observed before spontaneous crystallisation of KCl occurs when the solution is poured onto a crystal of KCI.

What masses of sodium chloride, magnesium chloride, sodium sulfate, calcium chloride, potassium chloride, and sodium bicarbonate are needed to produce 1 L of artificial seawater for an aquarium? The required ionic concentrations are  [Na+]  = 2.97 M;  [K+]  = 0.0082 M;  [Mg2+]  = 0.0627 M;  [Ca2+]  = 0.0123 M;  [HCO3−] = 0.0018 M;  [Cl−]= 3.01 M;  [SO42−]= 0.0590 M.

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The following graph shows the solubility of KBr in water in units of grams of KBr per 100 g of H,O. If 80 g of KBr is added to 100 g of water at 10°C and the mixture is heated slowly, at what temperature will the last KBr dissolve? 100 80 60 40 20 20 40 60 80 100 Temperature (°C) Solubility (g KBr per 100 g water)

The apparent solubility products of AgCN and PbF2 at 25°C are 6.0x10-1/ and 3.3×10¬8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) 4.0 solubility of A9CN g/100. g of solution solubility of PBF2 4.0 g/100. g of solution

Palmitic Acid, CH3(CH2)14COOH, found in both bacon fat and many soaps. Palmitic acid partially ionizes in water. Write a balanced chemical reaction for the dissociation of palmitic acid into its conjugate base and hydrogen ion. Write an expression for the equilibrium constant for palmitic acid. The equilibrium concentrations are [CH3(CH2)14COOH] = 0.1 M and [H+] = [CH3COO-] = 0.0133352 M. Calculate the equilibrium constant of ionization KA. Calculate the pKA of palmitic acid. Draw (by hand) the titration curve for palmitic acid. Please label your axes appropriately.

A bubble of air escaping from a diver's mask rises from a depth of 155 ft to the surface where the pressure is 1.00 atm. Initially, the bubble has a volume of 10.0 mL. Assuming none of the air dissolves in the water, how many times larger is the bubble just as it reaches the surface? Use this data: 1. The density of seawater is approximately 1.025 g mL! 2. The density of mercury is 13.6 g mL 47 times larger Use your answer to explain why scuba divers constantly exhale as they slowly rise from a deep dive. Since the pressure decreases by a factor of approximately factor of approximately 47 the volume must Increase : by a Divers exhale to decreases the amount of gas in their lungs, so it does not expand : to a volume larger than the diver's lungs.

At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute can dissolve in 125.5 g of water at the same temperature?

The CO2 gas sealed inside a carbonated beverage bottle has a pressure of 1.9atm. At this pressure, the solubility of CO, in water is 0.065g CO2/100 g H20. When the bottle is opened,the CO2 in the space above the liquid escapes, and the partial pressure of the CO2 falls to 2.3 mmHg, the value in the surrounding atmosphere of the room. Calculate the solubility of CO2 in the beverage at this new pressure, assuming no changes in temperature occur. Give the result in 2 sig. figs. 2.6 x 10^ -4 g of CO2 in 100 g of water.