At room temp, solubility of table salt in water is 359 g/L of water. If a solution was prepared at a high temp with 40 g of table salt in 100mL of water and then cooled back to room temp the solution would best be described as which of

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 19QRT

See similar textbooks

Related questions

Q: A solution contains 19.30 mg of hemoglobin in 14.5 mL of solution. The molar mass of hemoglobin is…

Q: Describe a solution. What kind of mixture is considered a solution: homo- or heterogeneous, explain…

A: Mixtures are defined as those substances or materials which are made of two or more components…

Q: 2. How does increasing the temperature of a solvent affect the solubility of a gas and a liquid?…

A: To solve this problem we have to know about the affect of temperature on Solubility of gas and…

Q: 1. Give 3 examples of each type of solution and identify the solutes and solvents -Gaseous Solution…

Q: A concentrated solution has (more, less, some) solute than a (molar, concentrated, dilute,…

A: A solution is the mixture of solute and solvent. Its concentration is defined based on the amount of…

Q: ensity of 3M solution of NaCl is 1. 25 g/ mL. Calculate the volume of water required to make 1000 mL…

Q: A scientist was hired for an up and coming biotech company. She used 25.00 g of iron (III)…

A: Given: Mass of Iron (III) hydroxide = 25.0 g Volume of Iron (III) hydroxide solution = 500.0 mL =…

Q: A 5.00% by mass dextrose solution contains how many grams of dextrose dissolved in 1.00 kg of water?

A: Mass percent :- The mass of solute in grams dissolved in 100 grams of solution is defined as mass…

Q: A solute has a solubility in water of 21 g/kg solvent. Is this value the same as 21 g/kg solution?…

Q: If 0.98 g of an unknown was dissolved in 10.30 g of solvent and the resulting solution has a…

A: Molality is moles of the solute that is present in 1000g or one kilogram(Kg) of solvent. Its SI unit…

Q: What does it mean to say that a substance is soluble in another substance? Which units are used in…

A: What is meant by a substance soluble in another substance is to be explained. The units that are…

Q: Which of the following statements concerning solution concentration is NOT true? The number of…

A: Since molarity is defined as the moles of solute present in 1 L of the solution Hence option 1 is…

Q: 13) During the process of diluting a solution to a lower concentration, A) the amount of solute does…

A: Given: Process of diluting a solution to a lower concentration.

Q: 2. What is the difference between a strong electrolyte and a weak electrolyte?

A: " Since you have asked multiple question , we will solve first question for you. If you want any…

Q: household bleach contains 6% sodium hypochlorite. How much household bleach should be combined with…

A: Answer: In this question we have to find out volume of household bleach needs to be mixed in weaker…

Q: 14. A 25.0 mL sample of concentrated H3PO4 (14.7 M) is diluted to a final volume of 750.0 mL. What…

A: Dilution is the process of decreasing the concentration of a solute in a solution usually simply by…

Q: What does NOT change when a solution is diluted by the addition of solvent? Select the correct…

A: As per bartleby guidelines I answered only first question so please don't mind.Thanks in advance.

Q: A 12.63 g sample contains only ethylene glycol (C2H6O2) and propylene glycol (C3H8O2). When the…

A: given: mass of water = 104 g mass of sample = 12.63 g freezing point of solution = -3.40oC we know…

Q: 50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known…

Q: A saturated solution of a compound contains .15g of solute in 100 g of water. Is a second solution…

Q: a 64.0mL portion of a 1.60M solution is diluted to a total volume of 238mL. A 119mL portion of that…

A: Consider the given information is as follows; 64.0mL portion of a 1.60M solution is diluted to a…

Q: A potassium bromide solution is 7.55 % potassium bromide by mass and its density is 1.03 g/mL. What…

Q: What mass of NaCl is dissolved in 400. g water in as 0.250 m solution?

A: 1- First calculate the moles of NaCl : Mass of solvent = 400g × ( 1kg / 1000g ) We know that, 1kg…

Q: True or false? A solution is formed when a solute dissolve in a solvent to form a single phase that…

A: Welcome to bartleby !

Q: Identify the solutions as saturated or supersaturated. Solubility information is given in the table.…

A: 1. Solubility of sucrose at 0 °C = 179.2 g sucorse /100 g of water = 1.792 g/1 g of water Cone, of…

Q: Use the information given to find the answer Part A.) 6MM IN 25 mol of hexane (g) (Keep in mind…

A: Given the experimental information, we can calculate the desired unknowns.

Q: Which of the following is true about solution? A solute is a minor component of a solution. All…

A: The solution is defined as the homogenous mixture of atleast two or more than two substance. Every…

Q: 2. A beaker of water and a beaker containing a sugar solution were placed in a closed container at…

A: Since the sugar solution has lower molar fraction of water than other water beaker.(pure water)).…

Q: A solution is prepared by mixing 631 mL of methanol with 501 mL of water. The molarity of methanol…

Q: To prepare 100 ml of 0.40 M NaCl solution from a 1.0 M solution you should mix: a) 40 ml of 1.0 M…

A: To prepare 100 ml of 0.40 M NaCl solution from a 1.0 M stock solution, the volume of stock solution…

Question

At room temp, solubility of table salt in water is 359 g/L of water. If a solution was prepared at a high temp with 40 g of table salt in 100mL of water and then cooled back to room temp the solution would best be described as which of the following? A) superdaturated solution B)unsaturated solution C)dominate solution D)saturated solution E)an incomplete solution

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
Every pure substance has a definite and fixed set of physical and chemical properties. A solution is prepared by dissolving one pure substance in another. Is it reasonable to expect that the solution will also have a definite and fixed set of properties that are different from the properties of either component? Explain your answer.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
Explain why the distinction between solute and solvent is not clear for some solutions.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
Refer to Figure 13.10 ( Sec. 13-4b) to answer these questions. (a) Does a saturated solution occur when 65.0 g LiCl is present in 100 g H2O at 40 C? Explain your answer. (b) Consider a solution that contains 95.0 g LiCl in 100 g H2O at 40 C. Is the solution unsaturated, saturated, or supersaturated? Explain your answer. (c) Consider a solution that contains 50. g Li2SO4 in 200. g H2O at 50 C. Is this solution unsaturated, saturated, or supersaturated? Explain your answer. Figure 13.10 Solubility of ionic compounds versus temperature.