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Problem 49a,b
Determine the oxidation number for the indicated element in each of the following substances: (a) S in SO3 (b) Ti in TiCl4
Problem 49c
Determine the oxidation number for the indicated element in each of the following substances: (c) P in AgPF6
Problem 49d
Determine the oxidation number for the indicated element in each of the following substances: (d) N in HNO3
Problem 50e,f
Determine the oxidation number for the indicated element in each of the following substances: (e) Pt in PtCl4 (f) O in OF2.
Problem 50f
Determine the oxidation number for the indicated element in each of the following substances: (f) Cl in NaClO4.
Problem 51a
Which element is oxidized, and which is reduced in the following reactions? (a) N2(g) + 3 H2(g) → 2 NH3(g)
Problem 51c,d
Which element is oxidized, and which is reduced in the following reactions? (c) Cl2(aq) + 2 NaI(aq) → I2(aq) + 2 NaCl(aq) (d) PbS(s) + 4 H2O2(aq) → PbSO4(s) + 4 H2O(l)
Problem 52
Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P4(s) + 10 HClO(aq) + 6 H2O(l) → 4 H3PO4(aq) + 10 HCl(aq) (b) Br2(l) + 2 K(s)→ 2 KBr(s) (c) CH3CH2OH(l) + 3 O2(g) → 3 H2O(l) + 2 CO2(g) (d) ZnCl2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaCl(aq)
Problem 53
Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid (b) chromium with hydrobromic acid (c) tin with hydrochloric acid (d) aluminum with formic acid, HCOOH.
Problem 54a,b
Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel (b) dilute sulfuric acid with iron
Problem 54c,d
Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium (d) acetic acid, CH3COOH, with zinc.
Problem 55a,b
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate (b) zinc metal is added to a solution of magnesium sulfate
Problem 55d
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
Problem 55e
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.
Problem 56a
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
Problem 56d
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
Problem 56e
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.
Problem 57a
The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)(aq), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations.
Problem 57b
The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)(aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?
Problem 58a
The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:
Br2(aq) + 2 NaI(aq) → 2 NaBr(aq) + I2(aq)
Cl2(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br2(aq)
(a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?
Problem 58b
The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:
Br2(aq) + 2 NaI(aq) → 2 NaBr(aq) + I2(aq)
Cl2(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br2(aq)
(b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed.
Problem 59a
(a) Is the number of moles of ions present in a solution an intensive or an extensive property?
Problem 59b
(b) Can you identify which one between 0.10 mol ZnCl2 and 0.1M ZnCl2 contains more Zn2+ ion? Why?
Problem 60b
You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C12H22O11). (b) How many liters of water would you have to add to this solution to reduce the molarity you calculated in part (a) by a factor of two?
Problem 61a
(a) Calculate the molarity of a solution that contains 0.175 mol ZnCl2 in exactly 150 mL of solution.
Problem 61c
(c) How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?
Problem 62a
a) Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water to form exactly 750 mL of solution.
Problem 62b
(b) How many moles of KBr are present in 150 mL of a 0.112 M solution?
Problem 62c
(c) How many milliliters of 6.1 M HCl solution are needed to obtain 0.150 mol of HCl?
- The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood?
Problem 63