Explain why dissolving potassium nitrate is an endothermic reaction while dissolving sodium...
Question:
Explain why dissolving potassium nitrate is an endothermic reaction while dissolving sodium carbonate is exothermic.
Endothermic and Exothermic Reactions:
Endothermic reactions are those reactions where energy is absorbed during the reaction and exothermic reactions involve evolution or release of energy during the reaction.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe energy required to separate the particles of potassium nitrate is more than the energy released by bonding of water molecules to the particles of...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Endothermic and Exothermic Reactions
from
Chapter 1 / Lesson 10
85K
Learn exothermic and endothermic reactions, their process, and the differences between them. See common endothermic vs exothermic examples.
Related to this Question
- From a molecular/ionic point of view (bonds broken/formed), why is it that dissolving potassium nitrate is endothermic while dissolving sodium carbonate is exothermic?
- Is the dissolution of ammonium nitrate in water an endothermic or exothermic process? Explain.
- When potassium nitrate dissolves in water, the beaker containing the solution gets cooler. Is dissolving this salt an exothermic or an endothermic process?
- Diluting and dissolving of potassium nitrate is very endothermic. Suggest what would be observed to the temperature if 2.0g of the salt is added to 2cm^3 of water.
- Explain why the solubility in 0.01 potassium nitrate is greater than it is in water.
- What occurs as potassium nitrate is dissolved in a beaker of water, indicating that the process is endothermic? a) The temperature of the solution decreases. b) The temperature of the solution increases. c) The solution changes color. d) The solution give
- Explain, why a precipitate forms when the silver nitrate solution is added to sodium chloride solution?
- Why does mixing silver nitrate with ammonium chloride, sodium carbonate, sodium hydroxide, and sulfuric acid form a precipitate?
- Which is more endothermic in water, ammonium chloride or potassium nitrate?
- Why did PbCl_2(s) dissolve in hot water, but AgCl(s) did not? Answer in terms of K_{sp} and Delta H (which is endothermic).
- Why does sodium nitrate (166.5) has a bigger molar entropy than sodium bromide (86.8)?
- When aqueous NaOH is added to the aqueous salt KNO3, will a precipitate form? Explain.
- Based on their solubility, can potassium nitrate and sodium sulfate be separated by extraction with water? Explain.
- NH_4CL can dissolve. Can very soluble salts precipitate? Is the dissolution of NH_4CL an endo or an exothermic process?
- Is there a reaction when NaNO3 is added to some H2O, or does it just dissolve? Explain.
- Explain why sodium chloride is an electrolyte. Write the equation for the dissolving of solid sodium chloride in water.
- Will a precipitate form from the reaction of NH4NO3 and Na2CO3? Explain why or why not.
- Explain why when aqueous sodium hydroxide is added to an aqueous solution of iron(III) nitrate, and a brown, gelatinous precipitate is formed, the net ionic equation is 3OH (aq) + Fe3+ (aq) =>Fe(OH)3
- There are a few compounds whose solubility decreases with increasing temperature. Briefly explain how the signs (+ or -) of delta H^o, delta S^o and delta G^o for these reactions would differ from the dissolution of potassium nitrate.
- Thermodynamics of potassium nitrate dissolving in water experiment post-lab questions: Look up the solubility of KNO3 per 100g H20 for 54 degrees celsius. Use a graph of solubility for different salts
- Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because: a. of the increase in disorder upon dissolution of this strong electrolyte. b. of the increase in
- Will mixing a KNO3 solution with a CaCl2 solution result in a precipitation reaction? Explain.
- Why is the dissolving of many ionic solids in water an endothermic process, whereas the mixing of most miscible liquids is an exothermic process?
- Explain why you can dissolve Ni(OH)3 in aqueous ammonia. Explain how (in procedures step format), the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) and nickel(II) h
- Explain why you can dissolve Ni(OH)3 in aqueous ammonia. Explain how (in procedures step format), the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) and nickel(II) hy
- When aqueous NaOH is added to the aqueous salt NH4NO3, will a precipitate form? Explain.
- If you mixed a silver nitrate solution with a potassium nitrate solution, would you precipitate a silver salt? Explain.
- Will the mixing of aqueous solutions of Ba(NO3)2 and Na2CO3 result in a precipitation reaction? Explain.
- When ammonium nitrate (NH_4NO_3) spontaneously dissolves in water, the solution becomes cold. What can you infer about the following parameters? 1) Delta H 2) Delta S 3) Delta G
- Do potassium hydroxide and ammonium nitrate make a precipitate? If so, what is it?
- Is the reaction between an aqueous solution of iron(III) nitrate and an aqueous solution of potassium iodide an example of a precipitation reaction? Explain.
- When NaCl (table salt) dissolves in water, the reaction is endothermic. When added to water, it dissolves easily (spontaneously) without added energy. How can this be?
- When NaCl (table salt) dissolves in water, the reaction is endothermic. Yet, when added to water, it dissolves easily (spontaneously) without added energy. How can this be?
- Will a precipitate form from the reaction between Ni(NO3)2 and Na2CO3? Explain why or why not.
- In an experiment, 95.0 mL of 0.225 M silver nitrate was mixed rapidly with 47.5 mL of 0.225 M calcium chloride in a coffee cup calorimetre. If a reaction occurred, was it exothermic or endothermic? If
- Will a precipitate form from the reaction of NH4NO3 and NaBr? Explain why or why not.
- Should a precipitate form when 25.00 mL of 0.0100 M silver nitrate is added to 15.00 mL of 0.0500 M potassium acetate? Explain.
- A sample of CaCO_3 (s) is placed in water and ionizes to Ca^{+2} (aq) + CO_3^{-2} (aq) with K_{sp} = 3.3 times 10^{-9} at 298 K. Show mathematically if this is an endo or exothermic process.
- Explain why some ionic compounds precipitate and others do not.
- Will a precipitate form from the reaction between Ba(NO3)2 and Na2CO3? Explain why or why not.
- Sodium nitrate dissolves readily in water according to the equation NaNO3(s) NaNO3(aq); DH = +21.0 kJ mol 1 Determine the energy change when 1.0 g of solid NaNO3 is dissolved in water.
- Explain why you can dissolve Ni(OH)2 in aqueous ammonia.
- Explain why the solubility of sodium sulfate in water decreases with increasing temperature.
- What is the chemical equation for the dissolution of NaNO3?
- Will a precipitate form from the reaction of NH4NO3 and NaOH? Explain why or why not.
- 1. What would the flame color of potassium carbonate be? 2. What is the cation after potassium carbonate reacts with (NH4)2CO3 and (NH4)2SO4? 3. What is the anion after it has reacted with AgNO3, AgNO
- If you mixed a silver nitrate solution with a sodium chlorate solution, would you precipitate a silver salt? Explain.
- Why do Cl and Na ions disappear in the reaction between NH4Cl and NaNH2 in liquid ammonia, and why is liquid ammonia used as a solvent for this reaction? Additionally, why does lithium disappear while NH3 remains when gaseous NH3 is added to ethyllithium
- Explain why potassium bromide is very soluble in water, while calcium oxide's solubility in water is very weak. Hint: Refer to the ionic structure, in your answer.
- Briefly explain why Cu^2+ ion does not precipitate as the hydroxide when you add NH_3 solution to make the solution basic in Part B of the procedure. Include the appropriate chemical equation to suppo
- Why mixture of NaNO_2 and NH_4Cl are taken in aqueous form?
- Will a precipitate form from the reaction of AgNO3 and Na2CO3? Explain why or why not.
- Is sodium carbonate soluble or insoluble in water? Explain.
- Will a precipitate form from the reaction of NH4NO3 and Na2SO4? Explain why or why not.
- Explain why we get different colored precipitate when we mix two different aqueous solutions. For example, why do we get a white precipitate or black precipitate?
- Will a mixture of NH4Cl and Ba(ClO4)2 form a precipitate? Explain.
- Explain why o-chlorobenzoic acid is insoluble in water, but sodium o-chlorobenzoate is soluble in water
- The dissolution of sodium chloride into its ionic components is an endothermic reaction. To allow the ionic bonds of salt crystals to break apart requires an input of energy; that energy comes from the water molecules of the surroundings. Therefore, the w
- Will aqueous solutions of NH4NO3 and Li2CO3 form a precipitate when mixed? Explain.
- Why does the Al(OH)_3 precipitate dissolve when excess NaOH(aq) is added? (i.e., what chemical change accounts for this observation?)
- Will a precipitate form from the reaction of Pb(NO3)2 and Na2CO3? Explain why or why not.
- What happens when you dissolve CO2(g) into NaOH(aq) (explain using net ionic equation)?
- How does changing the volume of strontium nitrate solution, added to 8 cm^3 of sodium carbonate solution, affect the amount of precipitate formed?
- Is KNO3 soluble in water? Explain.
- When ammonium nitrate is added to water, it dissolves and dissociates. The reaction is endothermic; therefore, H is _____ and T of the water is _____. (a) negative, positive (b) negative, negative (c) positive, negative (d) positive, positive
- Will mixing an (NH4)2CO3 solution with a Na2CO3 solution result in a precipitation reaction? Explain.
- Does a precipitate form when aqueous ammonia is added to an aqueous solution of NaNO3? Explain.
- Why do the ions in a solution not attract each other so strongly as to reconstitute the ionic solute?
- Explain the dissolution of the sulfides of copper, bismuth, and cadmium in nitric acid. Include ionic equations.
- How is the solubility of KNO3 affected by an increase in the temperature of the solvent?
- Is a potassium nitrate solution expected to be a strong electrolyte? Explain.
- Explain, by writing equation(s), how the given insoluble compound can be dissolved by the addition of a solution of ammonium nitrate or ammonium chloride. Mn(OH)2
- What does potassium nitrate form when it decomposes?
- Based on their solubility, can iron and potassium nitrate be separated by extraction with water? Explain.
- Consider the reaction between 0.156 L of 0.105 M magnesium nitrate and 0.166 L of 0.106 M potassium hydroxide. a) What mass of precipitate will form? b) What is the concentration of nitrate ions left in the solution after the reaction is complete?
- Solutions of potassium carbonate, copper(II) chloride, and lead(II) nitrate are each added to a beaker. Will any compound(s) precipitate from solution? Write a balanced net ionic equation for any precipitation reaction that occurs.
- Is KNO3 soluble or insoluble in water? Explain.
- When 50% potassium hydroxide is diluted to 4% with water, a white precipitate is formed..Can you tell me why and what the precipitate is?
- Why were different masses of precipitate obtained when various volumes of solution lead nitrate and potassium iodide mixed?
- The addition of sodium hydroxide solution to a solution containing three solutes- lead nitrate, ammonium nitrate, and silver nitrate- will cause formation of what precipitate?
- Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify. a. NaCl, KCl b. LiF, LiCl c. Mg(OH)2, MgO d. Fe(OH)2, Fe(OH)3 e. NaCl, Na2O f. MgO, BaS
- When aqueous NaOH is added to the aqueous salt Ba(NO3)2, will a precipitate form? Explain.
- Give the dissolution reactions for the following ionic solids: a. NH4Cl b. FePO4 c. SrSO4
- If you mixed a silver nitrate solution with a sodium chloride solution, would you precipitate a silver salt? Explain.
- Why a common ion lowers the solubility of an ionic compound?
- When 18.0 mL of a 1.83 x 10-4 M nickel(II) nitrate solution is combined with 15.0 mL of a 9.16 x 10-4 M potassium carbonate solution, does a precipitate form? For these conditions, the reaction quotient, Q, is equal to.
- Describe how an ionic solute such as NaCl dissolves in water to form a solution.
- Describe the electrolysis of an aqueous solution of KNO_3.
- When aqueous NaOH is added to the aqueous salt Fe(NO3)3, will a precipitate form? Explain.
- When aqueous NaOH is added to the aqueous salt NaNO3, will a precipitate form? Explain.
- When 22.0 mL of a 4.92 x 10-4 M sodium hydroxide solution is combined with 18.0 mL of a 1.25 x 10-4 M silver nitrate solution, does a precipitate form? Explain.
- Is the compound KNO3 soluble or insoluble in water? Explain.
- Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate? Explain?
- Give the reaction for solid sodium dissolving in water.
- Explain why some substances are soluble in water and some are not? Respond to the statement: "like dissolves like".
- Why do solutions of NaNO3 and Mg(NO3)2 behave differently when aqueous ammonia is added? Be specific in your answer.
- Describe what happens when potassium chromate dissolves in water.
- Determine if the following reactants will result in the formation of a precipitate. If a precipitate is formed, what is it? a. Na2SO4 + Ba(NO3)2 b. NH4Cl + Ca(NO3)2 c. KCl + CaI2 d. AgNO3 + KCl
- Suppose you have a water solution that is 0.0010 M Ca2+ and 0.0010 M Mg2+. Describe the precipitation reactions as you slowly add a concentrated solution of sodium carbonate (Na2CO3) to this solution. What would be the concentration of carbonate ions when
- When aqueous NaOH is added to the aqueous salt Al(NO3)3, will a precipitate form? Explain.
Explore our homework questions and answers library
Browse
by subject