None Be sure to answer all parts.Complete the following precipitation reaction with balanced molecular, total ionic, and net ionicequations. Remember to include the proper physical states and charges of ions. When writing ions, if acharge number is not "1", place the charge number before the charge sign. If a charge number is "1", donot include the charge number in the formula.Na2S(aq) + ZnSO4(aq)-Molecular:Na,S(aq)+ZnSO4(aq) → ZnS (s) + Na, SO4(aq)Total ionic: Reactants+2Na (aq)+S2-2+2-(aq)+Zn (aq) + SO4 (aq)Products->+ZnS (aq) +2Na (aq)+ SO2 (aq)Net ionic:2+2-Zn (aq)+S (aq)-ZnS (s)S

Step 1: Step 2: Step 3: Step 4:

Answered: Be sure to answer all parts. Complete…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 82GQ

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ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
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.
You are given mixtures containing the following compounds. Which compound in each pair could be separated by stirring the solid mixture with water? (a) NaOH and Ca(OH)2 (b) MgC12 and MgF2 (c) AgI and KI (d) NH4Cl and PbCl2
Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?
Which symbols are used to indicate solids, liquids, gases, and aqueous solutions in chemical equations?
Write a balanced equation for the reaction of hydroiodic acid, HI, with calcium hydroxide, Ca(OH)2. Then, write the balanced complete ionic equation and the net ionic equation for this neutralization reaction.
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 is meant by a strong acid? Are the strong acids also strong electrolytes? Explain.
Molarity is a conversion factor relating moles of solute in solution to the volume of the solution. How does one use molarity as a conversion factor to convert from moles of solute to volume of solution, and from volume of solution to moles of solute present?
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
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
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.

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