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4. Draw a molecular representation of Li₂SO4 in aqueous solution. Include water molecules to demonstrate the concept of hydration shells. Hint - it is easier to represent the cation and anion as a "ball" in the model. An example of this is given in the background reading.

4. Draw a molecular representation of Li₂SO4 in aqueous solution. Include water molecules to demonstrate the concept of hydration shells. Hint - it is easier to represent the cation and anion as a "ball" in the model. An example of this is given in the background reading.

Chemistry
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
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Just number 4 needs to be solved I have also included the background reading 

Double Displacement Reactions in Aqueous Solutions - Precipitation and Acid/Base Reactions PURPOSE To explore and learn to apply the solubility rules to predict the products of double displacement reactions. INTRODUCTION AND A BACKGROUND another set of chemicals (the products) via a chemical reaction: One of the main purposes of chemistry is to transform one set of chemicals (the reactants) into Reactants → Products Many of these reactions occur in an aqueous environment (i.e. in a solution where ions and compounds are dissolved in water). When a reactant or product has the physical state "(aq)", it means the substance is dissolved in water. When an ionic compound is in the aqueous state, it is dissociated into ions so it exists as individual ions in solution; for example, NaCl (aq) exists as individual Na+ and CI ions moving around in water. BaCl2 (aq) exists as three ions moving around independently in water: one Ba2+ and two separate Cl ions (note - two separate Cl ions are represented as 2 Cl and not Cl-2). If the ionic compounds are soluble, they dissociate in water. If not, they are considered insoluble. To determine if an ionic compound is soluble-i.e., will dissolve and dissociate—in water, we use the Solubility Rules (rules in your textbook, p. 131). The Solubility Rules allow us to determine which compounds are soluble, and thus in water are represented as aqueous: (aq), BaCl2 (aq), NaOH (aq), etc. The Solubility Rules also tell us which compounds are insoluble-i.e., do not dissolve much in water and remain mostly as solids: e.g. BaSO4 (s), AgCl (s), Al2(CO3)3 (s), etc. e.g., Kl Drawing lonic Solids in Water We can represent ionic solids in water as ions if they are soluble and as solids if they are insoluble. Notice the solvent water molecules are not shown. In this lab we will draw insoluble compounds completely as solids. Potassium sulfate formula: K2SO4 K+ so²/ K+ Calcium carbonate formula: CaCO3 CaCO3
Transcribed Image Text:Double Displacement Reactions in Aqueous Solutions - Precipitation and Acid/Base Reactions PURPOSE To explore and learn to apply the solubility rules to predict the products of double displacement reactions. INTRODUCTION AND A BACKGROUND another set of chemicals (the products) via a chemical reaction: One of the main purposes of chemistry is to transform one set of chemicals (the reactants) into Reactants → Products Many of these reactions occur in an aqueous environment (i.e. in a solution where ions and compounds are dissolved in water). When a reactant or product has the physical state "(aq)", it means the substance is dissolved in water. When an ionic compound is in the aqueous state, it is dissociated into ions so it exists as individual ions in solution; for example, NaCl (aq) exists as individual Na+ and CI ions moving around in water. BaCl2 (aq) exists as three ions moving around independently in water: one Ba2+ and two separate Cl ions (note - two separate Cl ions are represented as 2 Cl and not Cl-2). If the ionic compounds are soluble, they dissociate in water. If not, they are considered insoluble. To determine if an ionic compound is soluble-i.e., will dissolve and dissociate—in water, we use the Solubility Rules (rules in your textbook, p. 131). The Solubility Rules allow us to determine which compounds are soluble, and thus in water are represented as aqueous: (aq), BaCl2 (aq), NaOH (aq), etc. The Solubility Rules also tell us which compounds are insoluble-i.e., do not dissolve much in water and remain mostly as solids: e.g. BaSO4 (s), AgCl (s), Al2(CO3)3 (s), etc. e.g., Kl Drawing lonic Solids in Water We can represent ionic solids in water as ions if they are soluble and as solids if they are insoluble. Notice the solvent water molecules are not shown. In this lab we will draw insoluble compounds completely as solids. Potassium sulfate formula: K2SO4 K+ so²/ K+ Calcium carbonate formula: CaCO3 CaCO3
the spectator ions and write the net ionic equation. 3. For the following molecular equation, write out the complete ionic equation. Then cross out 2 HBr (aq) + Na2S (aq) → H₂S(g) + 2 NaBr(aq) Molecular equation: ioni(: 2 H² (4₁) + 2 B1 (99) + 2√9+ (aq) + 5² (aq) + H₂ Scg) + 2N₁¹ (99) + 2/85 (97) 2- Net: 2 H (99) + 5² (aq) → H₂S (9) На беду 4. Draw a molecular representation of Li₂SO4 in aqueous solution. Include water molecules to demonstrate the concept of hydration shells. Hint - it is easier to represent the cation and anion as a "ball" in the model. An example of this is given in the background reading. 5. In the lab procedures, you are told to "place 5 drops of the first solution into a well add drops of the second solution." In this case, is necessary to add exactly 5 drops? Are we isolating the products from the reaction or determining yields? FD In this case, with the lab it is not necessary to add exactly 5 drops, we determining yields because 58 Qualitive observation, we 16 are not 15 a
Transcribed Image Text:the spectator ions and write the net ionic equation. 3. For the following molecular equation, write out the complete ionic equation. Then cross out 2 HBr (aq) + Na2S (aq) → H₂S(g) + 2 NaBr(aq) Molecular equation: ioni(: 2 H² (4₁) + 2 B1 (99) + 2√9+ (aq) + 5² (aq) + H₂ Scg) + 2N₁¹ (99) + 2/85 (97) 2- Net: 2 H (99) + 5² (aq) → H₂S (9) На беду 4. Draw a molecular representation of Li₂SO4 in aqueous solution. Include water molecules to demonstrate the concept of hydration shells. Hint - it is easier to represent the cation and anion as a "ball" in the model. An example of this is given in the background reading. 5. In the lab procedures, you are told to "place 5 drops of the first solution into a well add drops of the second solution." In this case, is necessary to add exactly 5 drops? Are we isolating the products from the reaction or determining yields? FD In this case, with the lab it is not necessary to add exactly 5 drops, we determining yields because 58 Qualitive observation, we 16 are not 15 a
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