1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl solution? Hint: First balance the chemical equation. 2.S8 2AGNO3(aq) BaCl2 (aq) QAGCI(s) Ba(NO3)2(aq) a.se Imol 1243,5 I 07. 00 T

1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl solution? Hint: First balance the chemical equation. 2.S8 2AGNO3(aq) BaCl2 (aq) QAGCI(s) Ba(NO3)2(aq) a.se Imol 1243,5 I 07. 00 T

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 32QAP: A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of...

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A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
Potassium acid phthalate, KNaC8H4O4, or KHP, is used in many laboratories, including general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that can be dried by warming and weighed. A 0.3420-g sample of KNaC8H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH? KNaC8H4O4(aq)+NaOH(aq)KNaC8H4O4(aq)+H2O(aq)
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.06 g of precipitate. Determine the concentration of the NaOH solution.
How many grams of precipitate are formed if 175 mL of a 0.750 M aluminum sulfate solution and 375 mL of a 1.15 M sodium hydroxide solution are mixed together?
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. :math>PbSe. BaCO3 :math>Mg(OH)2f. AlPO4 :math>Na2SO4g. PbCl2 :math>(NH4)2Sh. CaSO4
What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.
Laws passed in some states define a drunk driver as one who drives with a blood alcohol level of 0.10% by mass or higher. The level of alcohol can be determined by titrating blood plasma with potassium dichromate according to the following equation 16H+(aq)+Cr2O72(aq)+C2H5OH(aq)4Cr3+(aq)+2CO2(g)+11H2O Assuming that the only substance that reacts with dichromate in blood plasma is alcohol, is a person legally drunk if 38.94 mL of 0.0723 M potassium dichromate is required to titrate a 50.0-g sample of blood plasma?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?