Directions: Read and analyze the following questions and compute for what isunknown in the given problem. Show complete solution by stating the given andunknown, and show the process from writing the formula to unit conversion (ifapplicable).1. Suppose you added 4.0 moles of sugar to 10.0 L of solution. Calculate the molarconcentration of the solution.2. A sample of water taken from a nearby lake is found to have 0.0035 mol of salt in a100mL solution. Determine the molar concentration of the solution in the lake.3. You dissolve 30.0g of sodium sulfate (Na2SO4(s) into 300mL of water. Calculate themolar concentration of the solution.

We are to calculate the molar concentration for the given samples. Molar concentration is molarity.

Answered: Directions: Read and analyze the…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 2A

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Similar questions

A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?
What is the difference between a solute and a solvent?
A student was given a 1.6240-g sample of a mixture of sodium nitrate and sodium chloride and was asked to find the percentage of each compound in the mixture. She dissolved the sample and added a solution that contained an excess of silver nitrate. The silver ion precipitated all of the chloride ion in the mixture as silver chloride. It was filtered, dried, and weighed. Its mass was 2.056g. What was the percentage of each compound in the mixture?
A common method for determining how much chloride ion is present in a sample is to precipitate the chloride from an aqueous solution of the sample with silver nitrate solution and then to weigh the silver chloride that results. The balanced net ionic reaction is :math>Ag+(aq)+Cl(aq)AgCl(s) ppose a 5.45-g sample of pure sodium chloride is dissolved in water and is then treated with a solution containing 1.15 g of silver nitrate. Will this quantity of silver nitrate be capable of precipitating all the chloride ion from the sodium chloride sample?
Molarity is a conversion factor relating moles of solute in solution to the volume of the solution. How does one use molarity as a conversion factor to convert from moles of solute to volume of solution, and from volume of solution to moles of solute present?
A throat spray is 1.40% by mass phenol, C6H5OH, in water. If the solution has a density of 0.9956 g/mL, calculate the molarity of the solution.
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
A solution is defined as a homogeneous mixture. Is a small sample of air a solution? Is the atmosphere a solution?
A solution is formed by mixing 1 gal ethanol with 10 gal gasoline. Identify the solvent and the solute.
Find the molarity of a 40.0% by mass aqueous solution of sulfuric acid, H2SO4, for which the density is 1.3057 g/mL.
The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample. :math>Ag+(aq)+Cl+(aq)AgCl(s) ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
Explain how you would prepare the following dilute solutions from the more concentrated ones: a.5.00L of 6.00MH2SO4 from a 18.0MH2SO4 solution b.250mL of 0.500MCaCl2 from a 3.00MCaCl2 solution c.200mL of 1.50%(w/v)KBr from a 10.0%(w/v)KBr solution d.500mL of 10.0%(v/v) alcohol from 50.0%(v/v) alcohol

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