When an anion being identified in a soluble using precipitation reaction, what needs to be added to the solution to identify the anion? -Anion of larger charge -Anion of larger size -Cation that will form a precipitation with that anion -Cation that forms compound that are always soluble -Cation that that forms compound that are almost always insoluble

Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?

Describe in words the titration of an acid with a base. Be sure to use the terms equivalence point, indicator, and end point correctly.

Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitrate

Reactions represented by the following equations take place in water solutions. Write each molecular equation in total ionic form, then identify spectator ions and write the equations in net ionic form. Solids that do not dissolve are designated by s, gases that do not dissolve are designated by g, and substances that dissolve but do not dissociate appear in blue. a. H2O(l)+Na2SO3(aq)+SO2(aq)2NaHSO3(aq) b. 3Cu(s)+8HNO3(aq)3Cu(NO3)2(aq)+2NO(g)+4H2O(l) c. 2HCl(aq)+CaO(s)CaCl2(aq)+H2O(l) d. CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(aq)+H2O(l) e. MnO2(s)+4HCl(aq)MnCl2(aq)+Cl2(aq)+2H2O(l) f. 2AgNO3(aq)+Cu(s)Cu(NO3)2(aq)+2Ag(s)

The (aq) designation listed after a solute indicates the process of hydration. Using KBr(aq) and C2H5OH(aq) as your examples, explain the process of hydration for soluble ionic compounds and for soluble covalent compounds.

Lead(II) nitrate is added to four separate beakers that contain the following: aker 1 (sodium chloride) eaker 2 (sodium hydroxide) eaker 3 (sodium phosphate) eaker 4 (sodium sulfate) ter the addition of the lead(II) nitrate solution to each beaker, in which beaker(s) will a precipitate form? Use the general solubility rules given in Table 7.1 to guide you.

Working with Concentration (Molarity Concepts) Note: You should be able to answer all of the following questions without using a calculator. Part 1: a Both NaCl and MgCl2 are soluble ionic compounds. Write the balanced chemical equations for these two substances dissolving in water. b Consider the pictures below. These pictures represent 1.0-L solutions of 1.0 M NaCl(aq) and 1.0 M MgCl2(aq). The representations of the ions in solution are the correct relative amounts. Water molecules have been omitted for clarity. Correctly label each of the beakers, provide a key to help identify the ions, and give a brief explanation of how you made your assignments. Keeping in mind that the pictures represent the relative amounts of ions in the solution and that the numerical information about these solutions is presented above, answer the following questions c through f. c How many moles of NaCl and MgCl2 are in each beaker? d How many moles of chloride ions are in each beaker? How did you arrive at this answer? e What is the concentration of chloride ions in each beaker? Without using mathematical equations, briefly explain how you obtained your answer. f Explain how it is that the concentrations of chloride ions in these beakers are different even though the concentrations of each substance (compound) are the same. Part 2: Say you were to dump out half of the MgCl2 solution from the beaker above. a What would be the concentration of the MgCl2(aq) and of the chloride ions in the remaining solution? b How many moles of the MgCl2 and of the chloride ions would remain in the beaker? c Explain why the concentration of MgCl2(aq) would not change, whereas the number of moles of MgCl2 would change when solution was removed from the beaker. As part of your answer, you are encouraged to use pictures. Part 3: Consider the beaker containing 1.0 L of the 1.0 M NaCl(aq) solution. You now add 1.0 L of water to this beaker. a What is the concentration of this NaCl(aq) solution? b How many moles of NaCl are present in the 2.0 L of NaCl(aq) solution? c Explain why the concentration of NaCl(aq) does change with the addition of water, whereas the number of moles does not change. Here again, you are encouraged to use pictures to help answer the question.

Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?

The procedures and principles of qualitative analysis are coy cred in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.