OBSERVATIONS If there's are reaction, predict the products and balance the equation. If no reaction. Put "NR" as the product. 1. Aqueous ammonia solution and copper (II) nitrate NH4OH (aq) + Cu(NO3)2(aq) → 2. Barium chloride and ammonium sulfate BaCl2(aq) + (NH4)2SO4(aq) 3. Calcium chloride and silver nitrate CaCl2(aq) + AgNO3(aq) 4. Barium chloride and calcium chloride BaCl2(aq) CaCl2(aq) 5. 3 M sodium hydroxide and 6 M hydrochloric acid NaOH (aq) + HCl(aq) 6. Sodium carbonate and 6 M hydrochloric acid Na2CO3(aq) + HCl(aq) 7. 3 M sodium hydroxide and iron(III) chloride. NaOH(aq) + FeCl3(aq) 8. Zinc nitrate solution and copper(II) nitrate Zn(NO3)2(aq) + Cu(NO3)2(aq) Discussion Evidence of a Reaction

OBSERVATIONS If there's are reaction, predict the products and balance the equation. If no reaction. Put "NR" as the product. 1. Aqueous ammonia solution and copper (II) nitrate NH4OH (aq) + Cu(NO3)2(aq) → 2. Barium chloride and ammonium sulfate BaCl2(aq) + (NH4)2SO4(aq) 3. Calcium chloride and silver nitrate CaCl2(aq) + AgNO3(aq) 4. Barium chloride and calcium chloride BaCl2(aq) CaCl2(aq) 5. 3 M sodium hydroxide and 6 M hydrochloric acid NaOH (aq) + HCl(aq) 6. Sodium carbonate and 6 M hydrochloric acid Na2CO3(aq) + HCl(aq) 7. 3 M sodium hydroxide and iron(III) chloride. NaOH(aq) + FeCl3(aq) 8. Zinc nitrate solution and copper(II) nitrate Zn(NO3)2(aq) + Cu(NO3)2(aq) Discussion Evidence of a Reaction

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...

See similar textbooks

Similar questions

Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. Rb:CO:(aq) + Fe(C:H3O±)>(aq) 1 3 4 18 (aq), + NR Rb Fe Reset Delete 2.
How to balance this equation? FeCO3(s) + H2CO3(aq) ------> Fe(HCO3)2(aq)
Determine the net ionic equation for the following reaction (if any) that occurs when the aqueous solution of K2S and Fe(NO3)2 are mixed. (A) K+ (ac) + NO3- (ac) → KNO3 (s) (B) Fe2+ (ac) + S2- (ac) + 2K+ (ac) + 2NO3- (ac) → FeS (s) + 2K+ (ac) + 2NO3- (ac) (C) Fe2+ (ac) + S2- (ac) + 2K+ (ac) + 2NO3- (ac) → Fe2+ + S2- (ac) + 2KNO3 (ac) (D) Fe2+ (ac) + S2- (ac) → FeS (s) (E) No ocurre reacción.
Balance the equation and choose the coefficient of the (?) Na2CO3 + HCI → NaCl + H20 + CO2 (x)N22CO3 + (x)HCl → (x)NaCl + (x)H20 + (? )CO2 ->
Find The net ionic equation for the following reaction, and explain your answer. Fe(OH)3 (s) + 3 HNO3 (aq) -----> Fe(NO3)3 (aq) + 3H2O (l) is: A Fe(OH)3 (s) + 3 H+ (aq) -----> Fe3+ (aq) + 3H2O (l) B OH- (aq) + H+ (aq) -----> H2O (l) C Fe(OH)3 (s) + 3 HNO3 (aq) -----> Fe3+(aq) + 3NO3- (aq) + 3H2O (l) D None of the above
The following reaction occurs in acid solution. Identify the reducing agent. (Note: The equation is not balanced.) Fe2*(aq) + Cr2O (aq) + H*(aq) → Cr*(aq) + Fe3*(aq) + H2O(I) O H20(e) O Fe2(s) O Cr20,2 (aq) O Cr3"(aq) OH (aq)
What is the oxidizing and reducing agent in the balanced equation? Mg(s) + Cr(C2H3O2)3(aq) ---> Mg(C2H3O2)3 (aq) + Cr(s)
Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. | - Ka(ag) + H,0(!) H,0(1)
FE(NO3)3+(NH4)2s→Fe2S3+2NH4NO3 net ionic equation
The concentration of a Fe2+ solution is determined by titrating it with a 0.1934 M solution of dichromate. The balanced net ionic equation for the reaction is shown below. Cr2O72-(aq) + 6 Fe2+(aq)+14 H3O+(aq)2 Cr3+(aq) + 6 Fe3+(aq)+21 H2O(l) In one experiment, 17.15 mL of the 0.1934 M Cr2O72- solution is required to react completely with 25.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
In an analysis of metal carbonate M2CO3∙3H2O, 1.500g of the unknown carbonate was dissolved in enough water to make a 100.0mL solution. 20.00mL of such solution was treated with 10.00mL of 1.000M HCl solution, and the excess acid was titrated with 54.92mL of 0.1138M NaOH solution. The equations are given below: CO32-(aq) + 2 H+(aq) → H2O(l) + CO2(g) H+(aq) + OH-(aq) → H2O(l) a) the moles of NaOH used in the titration is (enter the answer in 4 sig. figs.) Answer mol b) the mole of HCl reacted with the carbonate is (enter the answer in 4 sig. figs.) Answer mol c) the molar mass of M2CO3∙3H2O is (enter the answer in 4 sig. figs.) Answer g/mol d) the identity of metal M is (enter the element symbol) Answer
KO2(s) + H2O(l) → KOH(aq)+ O2 (g) + H2O2 (aq) balance the equation