For each of the following, use the solubility guidelines to determine if a precipitate will form. If aprecipitate forms, write the following for each reaction:the balanced chemical equationthe net ionic equation14. Aqueous lithium sulfide and aqueous silver nitrate are mixed in a beaker.15. NaCl(aq) and (NH.),SO.(aq) are added to a test tube.Chemistry 12 College Preparation WorksheetCopyright 2014 McGraw-HRyasn978-1-25-927538-8

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Answered: For each of the following, use 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

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 41A

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According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
Magnesite (magnesium carbonate, MgCO3) is a common magnesium mineral. From the solubility product constant, find the solubility of magnesium carbonate in grams per liter of water.
A 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium sulfate precipitates. Write the balanced equation for this reaction. Calculate the minimum volume of barium nitrate solution that was used. Calculate the minimum volume of sodium sulfate needed to precipitate 0.700 g barium sulfate. Assume 100% yield.
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?
. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?
95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?
Addition of water to concentrated sulfuric acid is dangerous because it generates enough heat to boil the water, causing it to spatter out of the container. For this reason, chemists remember to add acid to water. In a dilution experiment, we calculate the amount of the more concentrated solution that must be measured out. If we place this concentrated solution (Figure 4.7) in the volumetric flask first, then dilute with water, we violate the caution Add acid to water. Describe a safer variation on the method shown in Figure 4.7 that allows the quantitative dilution of concentrated sulfuric acid. Figure 4.7 Preparing a dilute solution from a concentrated solution. (a) Draw the concentrated solution into a pipet to a level just above the calibration mark. (b) Allow the liquid to settle down to the calibration line. Touch the tip of the pipet to the side of the container to remove any extra liquid. (c) Transfer this solution to a volumetric flask. Again touch the pipet to the wall of the flask to ensure complete transfer, but do not blow out the pipet because it is calibrated for a small amount of liquid to remain in the tip. (d) Dilute to the mark with solvent. Frequently, especially with concentrated acids, it is best to have some solvent present in the volumetric flask before you add the concentrated sample.
you would like to remove cadmium ions from a waste stream using precipitation. The final concentration of cadmium needs to be less than 0.001 mg/L. identify a chemical that could be used to precipitate cadmium out of solution to meet this goal. Show calculations and prove if it can be calculated.
A student mixes an aqueous solution of ammonium chromate and an aqueous solution of lead (II) nitrate and notices a precipitation form. If 55.0mL of 0.125M ammonium chromate and 35.0mL of 0.175M lead (II) nitrate are mixed in the reaction above, what mass of solid will precipitate?
measure out a 10 mL portion of 10% sodium sulphate into another test tube. making sure to count the drops, use a dropper to add 30% calcium chloride solution. swirl the solution after each drop. continue until a white precipitate occurs. write an equation to explain your observations. which solubility product has the smaller numerical value, that for calcium sulphate or barium sulphate. explain. measure out another 10 mL portion of 10% sodium sulphate into a clean test tube. add 8 drops of 50% sulphuric acid and swirl. count the number of drops (swirl after each drop) of 30% calcium chloride needed to produce a precipitate of calcium sulphate. explain why the number of drops of calcium chloride differs in the two experiments.

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