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Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when...
Experiment 8 Double Replacement Reactions Background: Some reactions have the net effect of causing the cation...
Experiment 8 Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of each reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms a product with chloride. Note that the formula of each product is determined by the charges of the ions,...
When you write the answers, please write the page number for which the question is located....
When you write the answers, please write the page number for
which the question is located. Thank you!
Experiment 8 Name: Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of cach reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms...
translate each word equationinto a balanced chemical equation: D. Double Replacement Reactions 1. silver nitrate(n) +...
translate each word equationinto a balanced chemical
equation:
D. Double Replacement Reactions 1. silver nitrate(n) + potassium iodide(n) silver iodide(s) potassium nitrate(a) 2. mercury(II) nitrate(aq) + potassium iodideng) - mercury(II) iodide(s) + potassium nitrate na) 3. aluminum nitrate(aq) + potassium iodide (aq) - no reaction 4. silver nitrate(aq) + sodium phosphate(aq) +silver phosphate(s) + sodium nitrateng) 5. mercury(II) nitrate(aq) + sodium phosphate(aq) mercury(II) phosphate(s) + sodium nitrate(aq) 6. aluminum nitrate(aq) + sodium phosphate(aq) aluminum phosphate (-) + sodium nitrate(n)
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
Write the molar equation and net ionic equation for each reaction. Reaction 1. silver nitrate +...
Write the molar equation and net ionic equation for each
reaction.
Reaction 1. silver nitrate + sodium chloride AgNO3 Nach 2. silver nitrate + sodium bromide AS Noz doim Narse 3. silver nitrate + potassium iodide A No3 KI 4. silver nitrate + sodium phosphate AS NO3 Naz PO 4 5. barium nitrate + potassium sulfate BaCNO3)2 Krsou 6. lead(II) nitrate + potassium sulfate Tome Pb(NO372 ksoy 7. barium chloride + sodium phosphate Dim Back Na₃PO4 8. calcium nitrate +...
1. A precipitate forms when aqueous solutions of copper(II) iodide and silver(I) nitrate are combined. 2....
1. A precipitate forms when aqueous solutions of copper(II) iodide and silver(I) nitrate are combined. 2. A precipitate forms when aqueous solutions of copper(II) iodide and sodium hydroxide are combined. 3. Consider the reaction when aqueous solutions of barium bromide and potassium sulfate are combined. The net ionic equation for this reaction is: 4. Consider the reaction when aqueous solutions of barium sulfide and calcium bromide are combined. The net ionic equation for this reaction is: 5. Write a net...
Chemical Reactions For each reaction you observed, the names of the reactants and products are given...
Chemical Reactions For each reaction you observed, the names of the reactants and products are given below. You must: 1. Write the correct formula for each reactant and product. Balance each equation. 2. A. Combination reactions magnesium oxide 1. Magnesium + oxygen (unbalanced) Mg+ O, MgO sulfur dioxide 2. Sulfur + oxygen B. Analysis of the Copper Content of a Penny po zinc chloride + hydrogen zinc + hydrochloric acid HCI ZnCl, 1. (unbalanced) н, Zn + C. Single Replacement...
silver nitrate + sodium phosphate + sodium nitrate yields silver phosphate + sodium phosphate Ib. Silver nitrate...
silver nitrate + sodium phosphate
+ sodium nitrate yields silver phosphate + sodium phosphate Ib. Silver nitrate Balanced: Complete lonic: Net Ionic: + sodium carbonate yields zine carbonate+ sodium nitrate 2a. Zinc nitrate (ag) (ag) Balanced: Complete lonic: Net lonic: 2b. Zinc nitrate (aq) + sodium phosphate yields zinc phosphate+ sodium nitrate (ag) () (a) Balanced: Complete Ionic: Net Ionic: Report Form - Chemical Reactions 50 yields aluminum iodide (ag) 3a. Aluminum nitrate +potassium iodide (ag) Balanced: Complete lonic: Net...
2. (10 points) Your new job now requires you to make 1.5 L of a solution...
2. (10 points) Your new job now requires you to make 1.5 L of a solution that is 0.100M potassium phosphate. You find a bottle on the shelf that is 3M potassium phosphate. Describe how you would make that solution. More details = more points. 3. (12 points) Write the names of the reactants and products for the net ionic reactions for the following reactions in water, if no reaction occurs, write "no reaction and explain why. Example: NaNO, +...
2.5 pts Which of the following ionic compounds are soluble in water? [Select all that apply.)...
2.5 pts Which of the following ionic compounds are soluble in water? [Select all that apply.) Calcium carbonate Ammonium sulfide Iron(III) iodide O Mercury(I) chloride Magnesium hydroxide O Lead(II) nitrate Rubidium phosphate Silver acetate Barium sulfide Calcium perchlorate Strontium bromide
Experiment 8 Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of each reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms a product with chloride. Note that the formula of each product is determined by the charges of the ions,...
When you write the answers, please write the page number for
which the question is located. Thank you!
Experiment 8 Name: Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of cach reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms...
translate each word equationinto a balanced chemical
equation:
D. Double Replacement Reactions 1. silver nitrate(n) + potassium iodide(n) silver iodide(s) potassium nitrate(a) 2. mercury(II) nitrate(aq) + potassium iodideng) - mercury(II) iodide(s) + potassium nitrate na) 3. aluminum nitrate(aq) + potassium iodide (aq) - no reaction 4. silver nitrate(aq) + sodium phosphate(aq) +silver phosphate(s) + sodium nitrateng) 5. mercury(II) nitrate(aq) + sodium phosphate(aq) mercury(II) phosphate(s) + sodium nitrate(aq) 6. aluminum nitrate(aq) + sodium phosphate(aq) aluminum phosphate (-) + sodium nitrate(n)
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
Write the molar equation and net ionic equation for each
reaction.
Reaction 1. silver nitrate + sodium chloride AgNO3 Nach 2. silver nitrate + sodium bromide AS Noz doim Narse 3. silver nitrate + potassium iodide A No3 KI 4. silver nitrate + sodium phosphate AS NO3 Naz PO 4 5. barium nitrate + potassium sulfate BaCNO3)2 Krsou 6. lead(II) nitrate + potassium sulfate Tome Pb(NO372 ksoy 7. barium chloride + sodium phosphate Dim Back Na₃PO4 8. calcium nitrate +...
Chemical Reactions For each reaction you observed, the names of the reactants and products are given below. You must: 1. Write the correct formula for each reactant and product. Balance each equation. 2. A. Combination reactions magnesium oxide 1. Magnesium + oxygen (unbalanced) Mg+ O, MgO sulfur dioxide 2. Sulfur + oxygen B. Analysis of the Copper Content of a Penny po zinc chloride + hydrogen zinc + hydrochloric acid HCI ZnCl, 1. (unbalanced) н, Zn + C. Single Replacement...
silver nitrate + sodium phosphate
+ sodium nitrate yields silver phosphate + sodium phosphate Ib. Silver nitrate Balanced: Complete lonic: Net Ionic: + sodium carbonate yields zine carbonate+ sodium nitrate 2a. Zinc nitrate (ag) (ag) Balanced: Complete lonic: Net lonic: 2b. Zinc nitrate (aq) + sodium phosphate yields zinc phosphate+ sodium nitrate (ag) () (a) Balanced: Complete Ionic: Net Ionic: Report Form - Chemical Reactions 50 yields aluminum iodide (ag) 3a. Aluminum nitrate +potassium iodide (ag) Balanced: Complete lonic: Net...
2. (10 points) Your new job now requires you to make 1.5 L of a solution that is 0.100M potassium phosphate. You find a bottle on the shelf that is 3M potassium phosphate. Describe how you would make that solution. More details = more points. 3. (12 points) Write the names of the reactants and products for the net ionic reactions for the following reactions in water, if no reaction occurs, write "no reaction and explain why. Example: NaNO, +...
2.5 pts Which of the following ionic compounds are soluble in water? [Select all that apply.) Calcium carbonate Ammonium sulfide Iron(III) iodide O Mercury(I) chloride Magnesium hydroxide O Lead(II) nitrate Rubidium phosphate Silver acetate Barium sulfide Calcium perchlorate Strontium bromide
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