6. Chemical Quantities & Aqueous Reactions

The most strongly reducing elements are listed at the top of the partial activity series table provided. Use the activity series to predict which reaction will occur. (LO 4.20) (a) (b) (c) (d)

Based on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red+ + Green ---> Red + Green+ (b) Blue + Green+ ---> Blue+ + Green (c) Red + Blue+ ---> Red+ + Blue

The following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain. (a)

(b)

(c)

(d)

Write balanced molecular and net ionic equations for the reactions of (d) aluminum with formic acid, HCOOH.

Write balanced molecular and net ionic equations for the reactions of (d) acetic acid, CH3COOH, with zinc.

Write balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) zinc metal is added to a solution of magnesium sulfate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) hydrogen gas is bubbled through a solution of silver nitrate.

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate

The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl21aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni1NO3221aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: Br21aq2 + 2 NaI1aq2¡2 NaBr1aq2 + I21aq2 Cl21aq2 + 2 NaBr1aq2¡2 NaCl1aq2 + Br21aq2 (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?

Write the balanced chemical equation for the reaction of solid strontium with iodine gas.

Write the balanced chemical equation for the reaction of solid lithium with liquid water.

Write the balanced chemical equation for the reaction of solid potassium with liquid water.

Write the balanced equation for the reaction of hydrogen gas with bromine gas.

Assume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?

Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution. (a) Given a 500-mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon?

Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are called alloys. There is a range of compositions over which the solution is considered a bronze. Bronzes are stronger and harder than either copper or tin alone. (c) Suggest a reaction that you could do to remove all the tin from this bronze to leave a pure copper sample. Justify your reasoning.

Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (d) What is the molarity of Cu2+ ions in the resulting solution?

Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (a) Which metal will react with the copper(II) nitrate solution?

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. c. 2.42gAg

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. b. 4.85gCu

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. a. 2.15gAl

Determine if HNO3 can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HNO3 and determine the minimum volume of 6.0 M HNO3 required to completely dissolve the sample. a. 5.90gAu

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (d)

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (c)

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (b)

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (a)

(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:

(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:

(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

Chlorine dioxide gas 1ClO22 is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced. (b) Why do you think that ClO2 is reduced so readily?

Some metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by (c) heating its oxide with coke?

Some metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by (a) finding it in its elemental state?

A sample of metal (M) reacted with both steam and aqueous HCl to release H2 but did not react with water at room tem-perature. When 1.000 g of the metal was burned in oxygen, it formed 1.890 g of a metal oxide, M2O3. What is the iden-tity of the metal?

An unknown metal (M) was found not to react with either water or steam, but its reactivity with aqueous acid was not investigated. When a 1.000 g sample of the metal was burned in oxygen and the resulting metal oxide converted to a metal sulfide, 1.504 g of sulfide was obtained. What is the identity of the metal?

Nickel metal is added to a solution of copper(ii) nitrate.

Chromium metal is immersed in an aqueous solution of cobalt(ii) chloride.