2. In Part A of this experiment you will prepare 0.1 M solutions of sodium carbonate(NazCO3), sodium bicarbonate (NaHCO3), sodium chloride (NaCl), and ammoniumchloride (NH.CI). You will need 100 mL of each solution. Calculate the mass of eachsolute that you will need for each solution.Mass of NazCO; needed to make the NazCO; solution:Mass of NaHCO3 needed to make the NaHCO3 solution:Mass of Nacl needed to make the Nacl solution:Mass of NH.Cl needed to make the NH,CI solution: ProcedureA. Preparation of salt solutions1. Put on your chemical-splash safety goggles. Your goggles must be worn at alltimes while in the laboratory. Don't take off your goggles until you leave thelaboratory.2. Before you start the experiment you will need to prepare 100 mL of 0.1 M solutions ofsodium carbonate (Na2CO3), sodium bicarbonate (NaHCO3), sodium chloride (NaCI),and ammonium chloride (NH.CI) in clean 250-mL beakers. Do this as described insteps below.• Calculate the amount of solid that you will need to prepare each solution. Theamount of NaCl that you will need to prepare the sodium chloride solution iscalculated in the Theory section. Use this calculation method to determine theamounts of the other solids you will need to prepare the other solutions. (See thePrelaboratory Assignment.)• Put a clean 250-mL beaker on a balance and zero (tare) the balance. Then weighthe appropriate amount of solid into the beaker and record the solid on your datasheet. Pour 50 mL of distilled water into the beaker and stir to dissolve the solid.Measure the volume of water with a clean graduated cylinder.Pour this solution into a clean 100-mL graduated cylinder and dilute the solutionwith distilled water to the 100-mL mark. Stir the solution in the graduated cylinderwith a clean stirring rod to completely mix the solution. The solution is now ready touse.• Use this procedure to prepare all four solutions. Be sure to use clean glassware foreach solution.

Answered: Image /qna-images/answer/05093f6b-c803-4081-93be-2b850cb8f87c.jpg

2. In Part A of this experiment you will prepare 0.1 M solutions of sodium carbonate (NazCO3), sodium bicarbonate (NaHCcỏa), sodium chloride (NaCI), and ammonium chloride (NH.CI). You will need 100 mL of each solution. Calculate the mass of each solute that you will need for each solution. Mass of NazCO3 needed to make the NazCO3 solution: Mass of NaHCOs needed to make the NaHCOs solution: Mass of Nacl needed to make the NaCl solution: Mass of NH,CI needed to make the NH.CI solution:

2. In Part A of this experiment you will prepare 0.1 M solutions of sodium carbonate (NazCO3), sodium bicarbonate (NaHCcỏa), sodium chloride (NaCI), and ammonium chloride (NH.CI). You will need 100 mL of each solution. Calculate the mass of each solute that you will need for each solution. Mass of NazCO3 needed to make the NazCO3 solution: Mass of NaHCOs needed to make the NaHCOs solution: Mass of Nacl needed to make the NaCl solution: Mass of NH,CI needed to make the NH.CI solution:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 94AP: 94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on...

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94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid 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
You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?
An experiment calls for you to use 250. mL of 1.00 M NaOH, but you are given a large bottle of 2.00 M NaOH. Describe how to make the desired volume of 1.00 M NaOH.
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
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?
3.86 When a solution is diluted, solvent is added but solute is not. Explain how this idea leads to the equation frequently used in dilution calculations, M1V1= M2V2.
Two students titrate different samples of the same solution of HCl using 0.100 M NaOH solution and phenolphthalein indicator (Figure 4.12). The first student pipets 20.0 mL of the HCl solution into a flask, adds 20 mL of distilled water and a few drops of phenolphthalein solution, and titrates until a lasting pink color appears. The second student pipets 20.0 mL of the HCl solution into a flask, adds 60 mL of distilled water and a few drops of phenolphthalein solution, and titrates to the first lasting pink color. Each student correctly calculates the molarity of an HCl solution. What will the second students result be? (a) four times less than the first students result (b) four times greater than the first students result (c) two times less than the first students result (d) two times greater than the first students result (e) the same as the first students result