Concept explainers
Interpretation:
Whether the reaction that occurs when aqueous solutions of sodium cyanide and hydrobromic acid are mixed is an example of redox reaction or precipitation reaction has to be predicted based on the acitivity series and solubility guidelines. The net ionic equation has to be written.
Concept introduction:
Metals are tabulated in decreasing order of their reducing power or increasing order of their oxidizing power. The table is termed as activity series. Any element in the activity series will replace the ions of the elements from a solution, written below it. If the product formed is an insoluble compound, the reaction is termed as precipitation reaction. If the elements in the reactants undergo
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Introductory Chemistry: An Active Learning Approach
- For each of the following, write molecular and net ionic equations for any precipitation reaction that occurs. If no reaction occurs, indicate this. a Zinc chloride and sodium sulfide are dissolved in water. b Sodium sulfide and calcium chloride are dissolved in water. c Magnesium sulfate and potassium bromide are dissolved in water. d Magnesium sulfate and potassium carbonate are dissolved in water.arrow_forwardConsider the following generic equation: H+(aq)+ B(aq)HB(aq)For which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) nitric acid and calcium hydroxide (b) hydrochloric acid and CH3NH2 (c) hydrobromic acid and aqueous ammonia (d) perchloric acid and barium hydroxide (e) sodium hydroxide and nitrous acidarrow_forwardMany plants are poisonous because their stems and leaves contain oxalic acid H2C2O4, or sodium oxalate, Na2C2O4. When ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, C2O42 in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Write die net ionic equation for the reaction between sodium oxalate and calcium chloride. CaCl2, in aqueous solution.arrow_forward
- Without first writing a full molecular or ionic equation, write the net ionic equations for any precipitation reactions that occur when aqueous solutions of the following compounds are mixed. If no reaction occurs, so indicate. l type='a'> iron(III) nitrate and sodium carbonate mercurous nitrate and sodium chloride sodium nitrate and ruthenium nitrate copper(II) sulfate and sodium sulfide lithium chloride and Iead(II) nitrate calcium nitrate and lithium carbonate gold(III) chloride and sodium hydroxidearrow_forwardAn aqueous sample is known to contain either Sr2+ or Hg22+ ions. Use the solubility rules (see Table 4.1) to propose an experiment that will determine which ion is present.arrow_forwardWrite the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid [HClO4(aq)] and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acidarrow_forward
- Explain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound.arrow_forwardNickel(II) sulfate solution reacts with sodium hydroxide solution to produce a precipitate of nickel(II) hydroxide and a solution of sodium sulfate. Write the molecular equation for this reaction. Then write the corresponding net ionic equation.arrow_forwardThe Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b From everyday experience you are probably aware that table sugar (sucrose), C12H22O11, is soluble in water. When sucrose dissolves in water, it doesnt form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water. c Both NH3 and C12H22O11 are soluble molecular compounds, yet they behave differently in aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte. d Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water. e Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes? f Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte. g Classify each of the following substances as either ionic or molecular. KCl NH3 CO2 MgBr2 HCl Ca(OH)2 PbS HC2H3O2 h For those compounds above that you classified as ionic, use the solubility rules to determine which are soluble. i The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water. j Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water? k How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer. l Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m Are NaCl and HI strong electrolytes because they have similar behavior in aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case. Part 2: You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water. AX(aq)+H2O(l)AH2O+(aq)+X(aq)AY(aq)+H2O(l)AH2O+(aq)+Y(aq) a Explain how the relative amounts of AX(aq) and AY(aq) would compare if you had a beaker of water with AX and a beaker of water with AY. b How would the relative amounts of X(aq) and Y(aq) in the two beakers compare? Be sure to explain your answer.arrow_forward
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