Use the References to access important values if needed for this question. Solid ammonium sulfide is slowly added to 175 mL of a 0.270 M lead(II) nitrate solution until the concentration of sulfide ion is 0.0263 M. The percent of lead ion remaining in solution is 96. Submit Answer Retry Entire Group 8 more group attempts remaining

Use the References to access important values if needed for this question. Solid ammonium sulfide is slowly added to 175 mL of a 0.270 M lead(II) nitrate solution until the concentration of sulfide ion is 0.0263 M. The percent of lead ion remaining in solution is 96. Submit Answer Retry Entire Group 8 more group attempts remaining

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter4: Stoichiometry Of Chemical Reactions

Section: Chapter Questions

Problem 86E: Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C),...

See similar textbooks

Similar questions

A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?
Gold metal will not dissolve in either concentrated nitric acid or concentrated hydrochloric acid It will dissolve, however, in aqua regia, a mixture of the two concentrated acids. The products of the reaction are the AuCl4 ion and gaseous NO. Write a balanced equation for the dissolution of gold in aqua regia.
A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?
ow do chemists know that the ions behave independently of one another when an ionic solid is dissolved in water?
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?
60. Suppose 325 in L of 0.150 M NaOH is needed for your experiment. How would you prepare this if all that is available is a 1.01 M NaOH solution?
Complete and balance the following acid-base equations: (a) HCl gas reacts with solid Ca(OH)2(s). (b) A solution of Sr(OH)2 is added to a solution of HNO3.
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.
The US Environmental Protection Agency (EPA) places limits on the quantities of toxic substances that may be discharged into the sewer system. Limits have been established for a variety of substances, including hexavalent chromium, which is limited to 0.50 mg/L. If an industry is discharging hexavalent chromium as potassium dichromate (K2Cr2O7), what is the maximum permissible molarity of that substance?
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.
In an accident, a solution containing 2.5 kg of nitric acid was spilled. Two kilograms of Na2CO3 was quickly spread on the area and CO2 was released by the reaction. Was sufficient Na2CO3 used to neutralize all of the acid?
Use the References to access important values if needed for this question. A student wants to prepare a solution of chromium(II) iodide with a known molarity. How many grams of Crl₂ must be weighed out to prepare 300. mL of a 0.222 M aqueous solution of the salt? g Submit Answer Retry Entire Group 9 more group attempts remaining