. Write the three equations and identify the spectator ions in the following mixtures (your instructor...
.
Write the three equations and identify the spectator ions in
the following mixtures (your instructor may assign different or additional ones):
a. Hydrochloric acid and silver nitrate.
b. Silver nitrate and sodium carbonate.
c. Potassium chromate and lead (II) acetate.
d. Sodium sulfate and barium chloride.
e. Lead (II) acetate and ammonium chloride
Homework Answers
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Write the three equations and identify the spectator ions in
the following mixtures (your instructor...
help! Section 1: Balance each of the following reactions. Your instructor may discuss the different types...
help!
Section 1: Balance each of the following reactions. Your instructor may discuss the different types of reactions present in these examples. Reaction Type Al + O2 +Al:03 Synthesis Synthesis N2 + H2 + NH3 MgCO3 → MgO + CO2 KCIO: → KCI + 02 Cu + AgNO3 → Ag + Cu(NO3)2 Cl2 + Nal → NaCl + 1; HCI + NaOH + H:0 + NaCI BiCl3 + H2S → Bi2S3 + HCI Section II: Balance each of the following...
What's the complete molecular equation, net ionic equation, and spectator ion(s) of each of the following...
What's the complete molecular equation, net ionic equation, and spectator ion(s) of each of the following reactions. 1.) hydrochloric acid and ammonium carbonate 2.) hydrochloric acid and magnesium metal 3.) hydrochloric acid and lead(ii) nitrate 4.) hydrochloric acid and sodium hydroxide 5.) hydrochloric acid and silver nitrate 6.) hydrochloric acid and ammonium sulfate 7.) barium nitrate and ammonium sulfate 8.) sodium hydroxide and copper(ii) nitrate 9.) aluminum nitrate and sodium hydroxide 10.) hydrochloric acid and copper metal
Post Laboratory Questions 1. Write the equation for the decomposition of sulfurous acid. Usingl 2. Using...
Post Laboratory Questions 1. Write the equation for the decomposition of sulfurous acid. Usingl 2. Using the three criteria for double displacement reactions, and the solubility table. predict whether a double displacement reaction will occur for each of the following. If the reaction will occur, balance the reaction write conventional, total ionic and net ionic equations. Box the net ionic equation. Be sure to include the proper phase labels. If no reaction will occur. write "no reaction". All reactants are...
Chemistry Molecular Equations Write the molecular equations (including phase labels), ionic, and net ionic equations. Indicate...
Chemistry Molecular Equations Write the molecular equations (including phase labels), ionic, and net ionic equations. Indicate the type of reaction, if there isn't one, please specify with "no reaction". 1. Potassium chloride + silver nitrate 2. Silver nitrate + nickel 3. Iron (II) sulfate + ammonium sulfide 4. Sulfuric acid and magnesium hydroxide 5. Hydrochloric acid + sodium hydrogen carbonate
Write formula for compounds wite the correct formula for the following compounds: sodium bromide calcium chloride...
Write formula for compounds
wite the correct formula for the following compounds: sodium bromide calcium chloride calcium sulfide copper(I) carbonate sulfuric acid diphosphorus pentoxide _ chloric acicd ammonium sulfate hydrochloric acid mercury(II) acetate lead (II) nitrite ammonium sulfite sodium sulfate nitrous acid nitric acid iron(III) sulfate barium fluoride copper(I) sulfite ammonium nitrate iron(III) hydroxide mercury(II) nitrate sulfurous acid hydrosulfuric acid iron(II) hydroxide lead(II) chloride calcium hydrogen carbonate sulfur trioxide phosphoric acid bromine pentafluoride dinitrogen tetroxide carbon monoxide aluminum carbonate ammonium...
T UI water. Trial Reagent Pair Waste 0.5 M ammonium chloride + 0.5 M sodium hydroxide...
T UI water. Trial Reagent Pair Waste 0.5 M ammonium chloride + 0.5 M sodium hydroxide 5 6 7 8 0.1 M barium chloride + 0.1 M sodium sulfate 0.1 M barium nitrate +0.1 M potassium chromate 0.1 M calcium chloride + 0.1 M sodium carbonate 0.1 M copper (II) nitrate + 0.1 M sodium chloride 0.1 M lead (II) nitrate + 0.1 M potassium iodide 0.1 M magnesium sulfate + 0.1 M potassium hydroxide Mg 2.0 M potassium hydroxide...
Silver nitrate and sodium sulfate RESULTS Observation. No Pppt Molecular Equation: Net lonic Equation: 2. Silver...
Silver nitrate and sodium sulfate RESULTS Observation. No Pppt Molecular Equation: Net lonic Equation: 2. Silver nitrate and sodium chloride Observation: Molecular Equations Net Ionic Equation: Silver nitrate and sodium carbonate Observation_ ppt Molecular Equation: Net lonic Equation: 4. Silver nitrate and potassium chromate Observation: Molecular Equation Net Ionic Equation: Silver nitrate and sodium hydroxide tot Observation Molecular Equation: Net lonic Equation: Silver nitrate and sodium acetate Observation: Molecular Equation: Net Ionic Equation: Solubility - 7 Lead (1) acetate and...
Study Exercise 3 Name Write chemical formulas for the following compounds: 1. 2. 3. Potassium iodide...
Study Exercise 3 Name Write chemical formulas for the following compounds: 1. 2. 3. Potassium iodide Barium sulfate Aluminum nitrate Copper (II) carbonate Gold (III) chloride Ferric hydroxide 7. Lead (II) chromate Nickel (II) hydroxide Mercury (II) bromide Silver acetate Magnesium chlorate 12. Sodium peroxide 13. Manganese (II) phosphate Ammonium sulfide 15. Platinum (IV) fluoride Chromium (III) hydroxide Calcium oxalate Antimony trichloride Ammonia Silicon dioxide Carbon monoxide 22. Hydrobromic acid Nitrous acid 24. - Acetic acid 25. Sulfuric acid
Write molecular and net ionic equations for the following reactions. (Include state symbols and balance reactions...
Write molecular and net ionic equations for the following reactions. (Include state symbols and balance reactions if necessary) 1) Copper(II) sulfate and sodium hydroxide solutions are combined: 2) A piece of solid aluminum metal is put into an aqueous solution of lead(II) nitrate: 3) Solutions of hydrobromic acid and potassium carbonate are combined: 4) Aqueous solutions of sodium hydroxide and hydrochloric acid are combined: 5) Aqueous solutions of silver nitrate and nickel(II) chloride are combined:
Page 157 IONIC AND NET IONIC EQUATIONS Some Solubility Rules: (a) Group 1A, ammonium, acetate, and...
Page 157 IONIC AND NET IONIC EQUATIONS Some Solubility Rules: (a) Group 1A, ammonium, acetate, and nitrate compounds are soluble. (b) Chloride, bromide, and iodide compounds are soluble except silver, lead(II) and mercury(1). (c) Carbonates and phosphates are insoluble except for Group IA and ammonium compounds. (d) Hydroxides are usually insoluble except for Group IA, strontium, barium and ammonium compounds. (e) Sulfides are usually insoluble. Some exceptions are Group IA and ammonium compounds Use the solubility rules given above and...
help!
Section 1: Balance each of the following reactions. Your instructor may discuss the different types of reactions present in these examples. Reaction Type Al + O2 +Al:03 Synthesis Synthesis N2 + H2 + NH3 MgCO3 → MgO + CO2 KCIO: → KCI + 02 Cu + AgNO3 → Ag + Cu(NO3)2 Cl2 + Nal → NaCl + 1; HCI + NaOH + H:0 + NaCI BiCl3 + H2S → Bi2S3 + HCI Section II: Balance each of the following...
Post Laboratory Questions 1. Write the equation for the decomposition of sulfurous acid. Usingl 2. Using the three criteria for double displacement reactions, and the solubility table. predict whether a double displacement reaction will occur for each of the following. If the reaction will occur, balance the reaction write conventional, total ionic and net ionic equations. Box the net ionic equation. Be sure to include the proper phase labels. If no reaction will occur. write "no reaction". All reactants are...
Write formula for compounds
wite the correct formula for the following compounds: sodium bromide calcium chloride calcium sulfide copper(I) carbonate sulfuric acid diphosphorus pentoxide _ chloric acicd ammonium sulfate hydrochloric acid mercury(II) acetate lead (II) nitrite ammonium sulfite sodium sulfate nitrous acid nitric acid iron(III) sulfate barium fluoride copper(I) sulfite ammonium nitrate iron(III) hydroxide mercury(II) nitrate sulfurous acid hydrosulfuric acid iron(II) hydroxide lead(II) chloride calcium hydrogen carbonate sulfur trioxide phosphoric acid bromine pentafluoride dinitrogen tetroxide carbon monoxide aluminum carbonate ammonium...
T UI water. Trial Reagent Pair Waste 0.5 M ammonium chloride + 0.5 M sodium hydroxide 5 6 7 8 0.1 M barium chloride + 0.1 M sodium sulfate 0.1 M barium nitrate +0.1 M potassium chromate 0.1 M calcium chloride + 0.1 M sodium carbonate 0.1 M copper (II) nitrate + 0.1 M sodium chloride 0.1 M lead (II) nitrate + 0.1 M potassium iodide 0.1 M magnesium sulfate + 0.1 M potassium hydroxide Mg 2.0 M potassium hydroxide...
Silver nitrate and sodium sulfate RESULTS Observation. No Pppt Molecular Equation: Net lonic Equation: 2. Silver nitrate and sodium chloride Observation: Molecular Equations Net Ionic Equation: Silver nitrate and sodium carbonate Observation_ ppt Molecular Equation: Net lonic Equation: 4. Silver nitrate and potassium chromate Observation: Molecular Equation Net Ionic Equation: Silver nitrate and sodium hydroxide tot Observation Molecular Equation: Net lonic Equation: Silver nitrate and sodium acetate Observation: Molecular Equation: Net Ionic Equation: Solubility - 7 Lead (1) acetate and...
Study Exercise 3 Name Write chemical formulas for the following compounds: 1. 2. 3. Potassium iodide Barium sulfate Aluminum nitrate Copper (II) carbonate Gold (III) chloride Ferric hydroxide 7. Lead (II) chromate Nickel (II) hydroxide Mercury (II) bromide Silver acetate Magnesium chlorate 12. Sodium peroxide 13. Manganese (II) phosphate Ammonium sulfide 15. Platinum (IV) fluoride Chromium (III) hydroxide Calcium oxalate Antimony trichloride Ammonia Silicon dioxide Carbon monoxide 22. Hydrobromic acid Nitrous acid 24. - Acetic acid 25. Sulfuric acid
Page 157 IONIC AND NET IONIC EQUATIONS Some Solubility Rules: (a) Group 1A, ammonium, acetate, and nitrate compounds are soluble. (b) Chloride, bromide, and iodide compounds are soluble except silver, lead(II) and mercury(1). (c) Carbonates and phosphates are insoluble except for Group IA and ammonium compounds. (d) Hydroxides are usually insoluble except for Group IA, strontium, barium and ammonium compounds. (e) Sulfides are usually insoluble. Some exceptions are Group IA and ammonium compounds Use the solubility rules given above and...
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