2. Classify each of the following (unbalanced) reactions as precipitation, acid-base neutralization, or oxidation-reduction ("redox") reaction. Provide the balanced equation for each below. a. H2SO4(aq) + KOH (aq) → K₂SO4(aq) + H2O (1) ... Balanced Equation: ......P A-B/N OR b. Mn(NO3)3(aq) + Na2S(aq) → Mn2S3(s) + NaNO3(aq) Balanced Equation: c. Na2CO3(aq) + H2SO4(aq) → H2O(l) + Na2SO4(aq) + CO2(g) Balanced Equation: P A-B/N OR .... P A-B/N OR

2. Classify each of the following (unbalanced) reactions as precipitation, acid-base neutralization, or oxidation-reduction ("redox") reaction. Provide the balanced equation for each below. a. H2SO4(aq) + KOH (aq) → K₂SO4(aq) + H2O (1) ... Balanced Equation: ......P A-B/N OR b. Mn(NO3)3(aq) + Na2S(aq) → Mn2S3(s) + NaNO3(aq) Balanced Equation: c. Na2CO3(aq) + H2SO4(aq) → H2O(l) + Na2SO4(aq) + CO2(g) Balanced Equation: P A-B/N OR .... P A-B/N OR

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
-N 1 Osynthesis Oprecipitation c. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. FeCl₂ (aq) + AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) oxidation-reduction decomposition [Review Topics] Osingle-displacement Odouble-displacement FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + 2AgCl(s) FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) Doxidation-reduction Odecomposition Osynthesis Oprecipitation Osingle-displacement Odouble-displacement d. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. Al(s) + Br₂ (1)→→ AlBr3 (8) [References] 2Al(s) + 3Br2 (1)→ 2A1Br3 (8) Al(s) + 3Br2(1)→ AlBr3 (s)
Write the balanced, ionic, and net ionic equations for the reactions below. Indicate the state of the reactants and products in each equation. Use (s) to represent a precipitate, (aq) for ions in the solution, and (g) for products in a gas state. If there is no reaction for net ionic write no reaction there. a) Copper (II) Nitrate + Lead (II) Nitrate - balanced: - ionic: - net ionic: b) Aluminum Sulfate + Copper (II) Nitrate - balanced: - ionic: - net ionic:
Write the net ionic equation for the following molecular equation. MnBr2 (aq) + (NH,)2CO3 (aq) → MnCO3 (8) + 2NH,Br(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aqg) or (s). If a box is not needed, leave it blank.)
List the ions and molecules that may have precipitated as part of your final salt product. Step 1. Dissolve the Aluminum metal : (adding solid Al to a Kott Solution) Peaction between Al metal and kot. AICOH and H₂ gas.. Net ionic equation: Solution produces Tetrahydroko aluminate ion 2 A1 (s) + 20H (aq) + 6 +₂0 (1) → 2 Al (OH) - (aq) + 3H2(g) K+(aq) OH(aq) equation that describes the reaction of Sulfuric acid in water: OR H₂SO4 (aq) + H₂0 (1) H₂O+ (aq) + Hs 04" (aq) 2- HSO4 (aq) + H₂O (1) H₂0+ (aq) + 504³ (aq) Step 3: Neutralize base with acid OH reacts with acid: H₂Ocaq) + OH(aq) → 2+1₂0 (1) • Al(OH), reacts with small amount of acid; Alcot)" (q) + Hy" O cag) Al(only (n+ H₂OCD Al(OH) reacts with large amount of acid (with heat): Al (DH), (s) + 3H₂ 0 (aq) → A1 " (aq) + 6 H₂0 (1)
2. Specify which of the following are oxidation-reduction reactions and identify the substance being oxidized and the substance being reduced, when appropriate. a. Cu (s) + 2 Ag (aq) + 2 Ag (s) + Cu²+ (aq) b. HCl (g) + NH, (g) → NH,Cl (s) c. SiCl, (l) + 2 H₂O (1)→ 4 HCl (aq) + SiO₂ (s) d. SiCl, (l) +2 Mg (s) 2 MgCl, (s) + Si (s) e. Al(OH), (aq) → AlO, (aq) + 2 H₂O (1) f. CH, (g) +H,O (g) + CO (g) + 3H, (g) g. Zn (s) + 2 HCl (aq) → ZnCl, (aq) + H₂(g) h. 2H* (aq) + 2 CrO, (aq) + Cr₂O," + H₂O (1)
d) A 38.5mL sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and percent yield. AGNO3(aq) + NaClaq) → AGCI6) + NaNO3(aq)
Ll.26.
Which one of the following is not a redox reaction? O Cl2(g) + 2KBr(aq)Br2() + 2KCI(aq) O Zn(s) + H2SO4laq) → ZnSO4(aq) + H2(g) 2H2(g) + O2(g) → 2H20() O 6FESO4(aq) + K2Cr207(aq)+ 7H2SO4(aq) - Cr2(SO4)3(aq) + 3FE2(SO4)3(aq)+ K2SO4(aq) + 7H20() H20() + NH3(g) → NH4*(aq) + OH (aq) Previous Page Next Page
Which of the following reaction is a precipitation reaction? A) HNO2(aq)+NaOH(aq)---NaNO2(aq)+H2O(I) B) 2C2H3OH(I)+7O2(g)---4CO2(g)+6H2O(I) C) 2H2O2(I)---2H2O(I)+O2(g) D) FeSO4(aq)+K2S(aq)---FeS(s)+K2SO4(aq)