im confused on how to do this problem can you do a step by step for me? calculate the volumn percentof solute in each solution A solution made by adding 28.5 mL of methyl alcohol to enough water to give 487mL of solution %(v/v)= A solution made by adding 81.1mL of ethylene glycol to enough water to give 211 mL of solution %(v/v)=

im confused on how to do this problem can you do a step by step for me? calculate the volumn percentof solute in each solution A solution made by adding 28.5 mL of methyl alcohol to enough water to give 487mL of solution %(v/v)= A solution made by adding 81.1mL of ethylene glycol to enough water to give 211 mL of solution %(v/v)=

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.42E

See similar textbooks

Similar questions

Consider two solutions at a certain temperature. Solution X has a nonelectrolyte as a solute and an osmotic pressure of 1.8 atm. Solution Y also has a nonelectrolyte as a solute and an osmotic pressure of 4.2 atm. What is the osmotic pressure of a solution made up of equal volumes of solutions X and Y at the same temperature? Assume that the volumes are additive.
Solutions Introduced directly into the bloodstream have to be isotonic with blood; that is, they must have the same osmotic pressure as blood. An aqueous NaCl solution has to be 0.90% by mass to be isotonic with blood. What is the molarity of the sodium ions in solution? Take the density of the solution to be 1.00 g/mL.
Specifications for lactated Ringers solution, which is used for intravenous (IV) injections, are as follows to reach 100. mL of solution: 285315 mg Na+ 14.117.3 mg K+ 4.9Q.O mg Ca2+ 368408 mg Cl 231261 mg lactate, C3H5O3 a. Specify the amount of NaCl, KCl, CaCl2 2H2O, and NaC3H5O3 needed to prepare 100. mL lactated Ringers solution. b. What is the range of the osmotic pressure of the solution at 37C, given the preceding specifications?
Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.
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.)
(a) If you dissolve 10.0 g (about one heaping teaspoonful) of sugar (sucrose, C12H22O11) in a cup of water (250. g), what are the mole fraction, molality, and weight percent of sugar? (b) Seawater has a sodium ion concentration of 1.08 104 ppm. If the sodium is present in the form of dissolved sodium chloride, what mass of NaCl is in each liter of seawater? Seawater is denser than pure water because of dissolved salts. Its density is 1.05 g/mL
In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
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?