CHEMFILE MINI-GUIDE TO PROBLEM SOLVING PDF

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It would be tedious and time-consuming to continually measure out small amounts of ZnCl2 to make mL of this solution. Of course, you could make many liters of the solution at one time, but that would require several large containers to store the solution.

The answer to the problem is to make a much more concentrated solution and then dilute it with water to make the less concentrated solution that you need. The more-concentrated solution is called a stock solution. You could make a 1 M ZnCl2 solution by measuring out 1 mol of zinc chloride, This solution is 10 times as concentrated as the solution you need.

Every time you need the test solution, you can measure out 10 mL of the 1 M solution and dilute it to mL to yield mL of 0. To make a solution by dilution, you must determine the volume of stock solution to use and the amount of solvent needed to dilute to the concentration you need. As you have mini-gguide, the molarity of a solution is its concentration in moles of solute per liter of solution.

Molarity is found by dividing the mini-guied of solute by the number of liters of solution. Therefore, where 1 and 2 represent the concentrated and diluted solutions: Items Data Concentration of the stock solution M1 4. Even though molarity is moles per liter, you can use volumes in milliliters along with molarity whenever the units cancel.

Yes; the computation is the same as 4. Complete the table below by calculating the missing value in each row. Molarity Volume Molarity Volume ans: Yes; volume of water was required. What volume of water would be added to What is the molarity of a solution of ammonium chloride prepared by diluting A student takes a sample of KOH solution and dilutes it with The student determines that the diluted solution is 0.

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The concentration of the original solution is 2. What was the volume problrm the original sample? A chemist wants to prepare a stock solution of H2SO4 so that sam- ples of What should the molarity of the stock solution be? If the chemist wants to prepare 5. The density of What mass splving con- centrated H2SO4 should be used to make the stock prlblem in b? To what volume should 1.

What volume of a 5. What is the molarity of the stock solution? Given a solution of known percentage concentration by mass, a lab- oratory worker can often measure out a calculated mass of the solu- tion in order to obtain a certain mass of solute. Sometimes, though, it is impractical to use the mass of a solution, especially with fum- ing solutions, such as concentrated HCl and concentrated HNO3.

Measuring these solutions by volume is much more practical. In order to determine the volume that should be measured, a worker would need to know the density of the solution. This information usually appears on the label of the solution bottle.

What is the volume of 1. What volume contains 1.

Chemfile Mini Guide To Problem Solving Answers –

The density of concentrated nitric acid is 1. What volume of concentrated HNO3 would be needed to prepare What volume of concentrated HCl solution would be needed problen prepare 4. See a for data. What is the molarity of the diluted solution? A chemist prepares What is the new molarity of the solution?

You must write out procedures for a group of lab technicians. One test they will perform requires You decide to use a 6.

CHEMFILE MINI-GUIDE TO PROBLEM SOLVING CHAPTER 15 Dilutions

What procedure should the technicians use in order to get the solution they need? A chemical test has determined the concentration of a solution of an unknown substance to be 2. Calculate the molar mass of the unknown substance. Tincture of iodine can be prepared by dissolving 34 g of I2 and 25 g of KI in 25 mL of distilled water and diluting the solution to What is the molarity of I2 in the solution?

What mass of this solution would be required to prepare Commercially available concentrated sulfuric acid is What volume of concentrated H2SO4 would you use in order to make 3. Describe how to prepare 1.

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Honey is a solution consisting almost entirely of a mixture of the hexose sugars fructose and glucose; both sugars have the formula C6H12O6but they differ in molecular structure. A sample of honey is found to be What is the molality of the hexose sugars in honey? Consider the sugars to be equivalent. The density of the honey sample is 1. What mass of hexose sugars are in 1.

What is the molarity of the mixed hexose sugars in honey? Industrial chemicals used in manufacturing are almost never pure, and the content of the material may vary from one batch to the next.

For these reasons, a sample is taken from each shipment and sent to a laboratory, where its makeup is determined. This procedure is called assaying. Once the content of a material is known, engineers adjust the manufacturing process to account for the degree of purity of the starting chemicals.

Suppose you have just received a shipment of sodium carbonate, Na2CO3. You weigh out By measuring the amount of a second substance that reacts with Na2CO3you determine that the concentration of sodium carbonate in solvinv diluted solution is 0.

Calculate the percentage of Na2CO3 in the original batch of material. The molar mass of Na2CO3 is Deter- mine the number of moles in the original solution and convert to mass of Na2CO3. A student wants to prepare 0.

What mass of CuCl2 should be used to make the stock solution? You have a bottle containing a 2. You must tell other students how to dilute this solution to get various volumes of a 0. By what factor will you tell them to dilute the stock solution? In other words, when a student removes any vol- ume, V, of the stock solution, how many times V of water should be added to dilute to 0. You have a bottle containing an What mass of strontium nitrate is dissolved in How many moles of strontium nitrate are dissolved in You can publish your book online for free in a few minutes!

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