find net ionic equation? a Write the molecular equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution.(Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.)ZNCO,(s) V2HB1(aq)ZnBr, (aq)H2O(1)CO,(g)CorrectZNCO3 (s) + 2HBr(ag) CO2 (g) + H20(1) + ZnBr2 (ag)b What is the net ionic equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution?(Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H* for hydronium ion.)

Find net ionic equation of the given reaction--

a Write the molecular equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.) ZnCO,(s) + 2HB1(aq) ZnBr, (aq) H,O(1) Co,(g) Correct ZnCO3 (s) + 2HB1(aq) CO2 (g) + H2O(1) + ZnBr2 (ag) b What is the net ionic equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution? (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.)

a Write the molecular equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.) ZnCO,(s) + 2HB1(aq) ZnBr, (aq) H,O(1) Co,(g) Correct ZnCO3 (s) + 2HB1(aq) CO2 (g) + H2O(1) + ZnBr2 (ag) b What is the net ionic equation for the reaction of solid zinc carbonate and hydrogen bromide in an aqueous solution? (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 96AE: One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and...

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The Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b From everyday experience you are probably aware that table sugar (sucrose), C12H22O11, is soluble in water. When sucrose dissolves in water, it doesnt form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water. c Both NH3 and C12H22O11 are soluble molecular compounds, yet they behave differently in aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte. d Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water. e Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes? f Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte. g Classify each of the following substances as either ionic or molecular. KCl NH3 CO2 MgBr2 HCl Ca(OH)2 PbS HC2H3O2 h For those compounds above that you classified as ionic, use the solubility rules to determine which are soluble. i The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water. j Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water? k How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer. l Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m Are NaCl and HI strong electrolytes because they have similar behavior in aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case. Part 2: You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water. AX(aq)+H2O(l)AH2O+(aq)+X(aq)AY(aq)+H2O(l)AH2O+(aq)+Y(aq) a Explain how the relative amounts of AX(aq) and AY(aq) would compare if you had a beaker of water with AX and a beaker of water with AY. b How would the relative amounts of X(aq) and Y(aq) in the two beakers compare? Be sure to explain your answer.
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One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?
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You mix 25.0 mL of 0.234-M FeCl3 solution with 42.5 mL of 0.453-M NaOH. Calculate the maximum mass, in grams, of Fe(OH)3 that will precipitate. Determine which reactant is in excess. Calculate the concentration of the excess reactant remaining in solution after the maximum mass of Fe(OH)3 has precipitated.
An aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.
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