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OWLv2 with Student Solutions Manual eBook for Masterton/Hurley's Chemistry: Principles and Reactions, 8th Edition, [Instant Access], 4 terms (24 months)
8th Edition
ISBN: 9781305863170
Author: William L. Masterton; Cecile N. Hurley
Publisher: Cengage Learning US
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Chapter 4, Problem 65QAP
Using circles to represent cations and squares to represent anions, show pictorially the reactions that occur between aqueous solutions of
(a) Fe3+ and OH-.
(b) Na+ and PO43-.
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When a solution of dithionite ions (S2O42–) is added to a solution of chromate ions (CrO42–), the products of the ensuing chemical reaction, which occurs under basic conditions, include soluble sulfite ions and solid chromic hydroxide. This reaction is used to remove Cr(VI) from wastewater generated by factories that make chrome-plated metals.
(a) Write the net ionic equation for this reaction. Do not include phases.
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Calculate (a) the percentage of P,0s in the sample; (b) the weight of the precipitate of
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Chapter 4 Solutions
OWLv2 with Student Solutions Manual eBook for Masterton/Hurley's Chemistry: Principles and Reactions, 8th Edition, [Instant Access], 4 terms (24 months)
Ch. 4 - Write the formulas of the following compounds and...Ch. 4 - Prob. 2QAPCh. 4 - Describe how you would precipitate (a) zinc...Ch. 4 - Name the reagent, if any, that you would add to a...Ch. 4 - Write net ionic equations for the formation of (a)...Ch. 4 - Write net ionic equations to explain the formation...Ch. 4 - Decide whether a precipitate will form when the...Ch. 4 - Follow the directions of Question 7 for solutions...Ch. 4 - Write a net ionic equation for any precipitation...Ch. 4 - Follow the directions for Question 9 for the...
Ch. 4 - What volume of 0.2500 M cobalt(III) sulfate is...Ch. 4 - Prob. 12QAPCh. 4 - A 50.00-mL sample of 0.0250 M silver nitrate is...Ch. 4 - Aluminum ions react with carbonate ions to form an...Ch. 4 - When Na3PO4 and Ca(NO3)2 are combined, the...Ch. 4 - When solutions of aluminum sulfate and sodium...Ch. 4 - Prob. 17QAPCh. 4 - Prob. 18QAPCh. 4 - Prob. 19QAPCh. 4 - Follow the directions of Question 19 for the...Ch. 4 - For an acid-base reaction, what is the reacting...Ch. 4 - Follow the directions of Question 21 for the...Ch. 4 - Prob. 23QAPCh. 4 - Prob. 24QAPCh. 4 - Consider the following generic equation: H+(aq)+...Ch. 4 - Consider the following generic equation...Ch. 4 - Prob. 27QAPCh. 4 - Prob. 28QAPCh. 4 - Prob. 29QAPCh. 4 - Consider several 25.00-mL solutions of perchloric...Ch. 4 - Prob. 31QAPCh. 4 - A student tries to determine experimentally the...Ch. 4 - Prob. 33QAPCh. 4 - For a product to be called vinegar, it must...Ch. 4 - The percentage of sodium hydrogen carbonate,...Ch. 4 - Prob. 36QAPCh. 4 - An artificial fruit beverage contains 12.0 g of...Ch. 4 - Lactic acid, C3H6O3 is the acid present in sour...Ch. 4 - Prob. 39QAPCh. 4 - Prob. 40QAPCh. 4 - Assign oxidation numbers to each element in (a)...Ch. 4 - Assign oxidation numbers to each element in (a)...Ch. 4 - Classify each of the following half-reactions as...Ch. 4 - Classify each of the following half-reactions as...Ch. 4 - Classify each of the following half-reactions as...Ch. 4 - Prob. 46QAPCh. 4 - For each unbalanced equation given below • write...Ch. 4 - Prob. 48QAPCh. 4 - A solution of potassium permanganate reacts with...Ch. 4 - Prob. 50QAPCh. 4 - Hydrogen gas is bubbled into a solution of barium...Ch. 4 - Consider the reaction tween silver and nitric acid...Ch. 4 - The molarity of iodine in solution can be...Ch. 4 - A wire weighing 0.250 g and containing 92.50% Fe...Ch. 4 - Glycerol (C3H8O3) is commonly used as an additive...Ch. 4 - Laws passed in some states define a drunk driver...Ch. 4 - A sample of limestone weighing 1.005 g is...Ch. 4 - The iron content of hemoglobin is determined by...Ch. 4 - In order to determine the purity of ammonium...Ch. 4 - Gold metal will dissolve only in aqua regia, a...Ch. 4 - Prob. 61QAPCh. 4 - Ten mL of concentrated H3PO4 (91.7% by mass,...Ch. 4 - Consider the following balanced redox reaction in...Ch. 4 - Prob. 64QAPCh. 4 - Using circles to represent cations and squares to...Ch. 4 - Assuming that circles represent cations and...Ch. 4 - Consider four beakers. Beaker A has an aqueous...Ch. 4 - The following figures represent species before and...Ch. 4 - A student is asked to identify the metal nitrate...Ch. 4 - Three students titrate different samples of the...Ch. 4 - Calcium in blood or urine can be determined by...Ch. 4 - Copper metal can reduce silver ions to metallic...Ch. 4 - Copper metal can reduce silver ions to metallic...Ch. 4 - A solution contains both iron(II) and iron(III)...Ch. 4 - A student is given 0.930 g of an unknown acid,...Ch. 4 - Solid iron(III) hydroxide is added to 625 mL of...Ch. 4 - A 300.0-g sample of a solid is made up of a...Ch. 4 - When 85.0 mL of 0.250 M Ba(OH)2 solution is added...
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- What volume of 0.200 M NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl3 is an excess of water? Note that when H3PO3 i5 titrated under these conditions, only one proton of the acid molecule reacts.arrow_forwardIodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese dioxide, MnO2. The reaction is 2I(aq)+4H+(aq)+MnO2(s)Mn2+(aq)+2H2O+I2(s) If an excess of hydrogen iodide is added to 0.200 g of MnO2, how many grams of iodine are obtained, assuming 100% yield?arrow_forwardMagnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?arrow_forward
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