Consider these compounds: A. BaF2 B. Ag2SO3 C. Fe₂S3 D. CA3(PO4)2 Complete the following statements by entering the letter corresponding to the correct compound. Without doing any calculations it is possible to determine that zinc cyanide is more soluble than and zinc cyanide is less soluble than. It is not possible to determine whether zinc cyanide is more or less soluble than comparing Ksp values. by simply

Consider these compounds: A. BaF2 B. Ag2SO3 C. Fe₂S3 D. CA3(PO4)2 Complete the following statements by entering the letter corresponding to the correct compound. Without doing any calculations it is possible to determine that zinc cyanide is more soluble than and zinc cyanide is less soluble than. It is not possible to determine whether zinc cyanide is more or less soluble than comparing Ksp values. by simply

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 91AE: The solubility of benzoic acid (HC7H5O2), is 0.34 g/100 mL in water at 25C and is 10.0 g/100 mL in...

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An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of 5.20C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
The solubility of benzoic acid (HC7H5O2), is 0.34 g/100 mL in water at 25C and is 10.0 g/100 mL in benzene (C6H6) at 25C. Rationalize this solubility behavior. (Hint: Benzoic acid forms a dimer in benzene.) Would benzoic acid be more or less soluble in a 0.1-M NaOH solution than it is in water? Explain.
A carbonated beverage is made by saturating water with carbon dioxide at 0C and a pressure of 3.0 atm. The bottle is then opened at room temperature (25C), and comes to equilibrium with air in the room containing CO2(PCO2=1.0103M/atm). The Henry's law constant for the solubility of CO2 in water is 0.0769 M/atm at 0C and 0.0313 M/atm at 25C. (a) What is the concentration of carbon dioxide in the bottle before it is opened? (b) What is the concentration of carbon dioxide in the bottle after it has been opened and come to equilibrium with the air?
Which of the following is most soluble in water? Assume that all Ksp values are for identical conditions. a) Ksp = 7.2 x 10–7 b) Ksp = 4.8 x 10–30 c) Ksp = 7.0 x 10–2 d) Ksp = 8.9 x 10-15
1. A 12% by mass sodium chloride solution is prepared by dissolving enough of the salt to give 200.0 g of solution. What is the mass of water required? 2. Calculate the solubility of carbon dioxide in water at 0 °C and a pressure of 2.5 atm. The solubility of carbon dioxide is 0.348 g/100 mL water at 0 °C and 1.00 atm. Compute the solubility in g/L 3.You are tasked to prepare 1L of 0.85% Normal saline solution (NSS) for the Lab. How much more NaCl do you need to add if you initially dissolved 0.5g of NaCl? 4.An aqueous solution of hydrochloric acid contains 24% HCl by mass. Calculate the mole percent of HCl in the solution. 5.What is the molality of 12.5N HNO3 solution? Density=1.503 g/mL
Calculate the mass (in grams) of sodium phosphate that will be added to 500 g of H2O so that the freezing point of the solution is −8.3 ??? (Kfp(?????) = 1.86 °?/?).
What is the normal boiling point of 1.21 M solution of CaI2 that has a density of 1.92 g/ml? (Kb for H2O =0.512 ° C .kg/mole)
a. Water has a high specific heat. Relate this property to the changing climate and the capacity of bodies of water to act as temperature buffer. b. The boiling point of water is unusually high. Relate this property to cases of small bodies of water which dries up easily considering the fact that the boiling point of water is unusually high.
The presence of the radioactive gas radon (Rn) in well waterpresents a possible health hazard in parts of the UnitedStates. (a) Assuming that the solubility of radon in waterwith 1 atm pressure of the gas over the water at 30 °C is7.27 * 10-3 M, what is the Henry’s law constant for radon (c) The free-base form of cocaine has a solubility of 1.00 g in6.70 mL ethanol (CH3CH2OH). Calculate the molarityof a saturated solution of the free-base form of cocaine inethanol.(d) The hydrochloride form of cocaine has a solubility of1.00 g in 0.400 mL water. Calculate the molarity of a saturatedsolution of the hydrochloride form of cocaine inwater.(e) How many mL of a concentrated 18.0 M HCl aqueoussolution would it take to convert 1.00 kilograms(a “kilo”) of the free-base form of cocaine into its hydrochlorideform?
Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?
A solution of anhydrous dextrose (m.w. 180) contains 25 g in 500 mL of water.Calculate the freezing point of the solution.
Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 × 10–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209. Calculate the solubility (in M) of O2 in the blood of a climber on Mt. Everest, where Patm = 0.35 atm. Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm.