Download SOLUBILITY RULES FOR IONIC COMPOUNDS IN WATER

HOMEWORK 1A
1. Write the correct equilibrium-constant expressions for the following reactions.
(a) 4NH3 (g) + 7O2 (g) ⇆ 4NO2 (g) + 6H2O (g)
(b) 2NO2 (g) + 7H2 (g) ⇆ 2NH3 (g) + 4H2O (g)
(c) NH4Cl (s) ⇆ NH3 (g) + HCl (g)
(d) 2ZnS (s) + 3O2 (g) ⇆ 2ZnO (s) + 2SO2 (g)
(e) Cl2 (g) + H2O (g) ⇆ 2HCl (g) + ½O2 (g)
2. In a 2.50 L flask at 298 K, 0.125 mol SO2, 0.145 mol O2, and 0.465 mol SO3 are at equilibrium.
Calculate the equilibrium constant for the reaction:
2SO2 (g) + O2 (g) ⇆ 2SO3 (g)
3. At 450 K the equilibrium constant for the reaction:
NO (g) + ½O2 (g) ⇆ NO2 (g)
is given by:
Keq = 1.25 x 102
(a) At equilibrium are the products or reactants favored for this reaction?
(b) What is the numerical value of Keq for the reaction:
2NO (g) + O2 (g) ⇆ 2NO2 (g)
(c) What is the numerical value of Keq for the reaction:
2NO2 (g) ⇆ 2NO (g) + O2 (g)
4. The equilibrium constant for the reaction:
N2 (g) + O2 (g) ⇆ 2NO (g)
at 2,130ºC is 2.0 x 101 . For the following conditions, determine whether the reaction is spontaneous
forward or in reverse, or whether it is at equilibrium.
(a) A 1.0 L box contains 0.02 mole of N2, 0.01 mole of O2, and 0.02 mole of NO at 2,130ºC.
(b) A 1.0 L box contains 0.2 mole of N2, 0.01 mole of O2, and 0.02 mole of NO at 2,130ºC.
(c) A 1.0 L box contains 0.2 mole of N2, 0.01 mole of O2, and 0.2 mole of NO at 2,130ºC.
HOMEWORK 1B
1. At 1,476 K the equilibrium constant for the reaction:
CO (g) + ½O2 (g) ⇆ CO2 (g)
is given by:
Kc = 2.50 x 105
(a) Determine the numerical value of Kp for the above reaction.
(b) What would be the numerical value of the Kp for the reaction:
2CO (g) + O2 (g) ⇆ 2CO2 (g)
2. When sulfur trioxide is produced from the combustion of sulfur dioxide at 1,000. K, a sample of the
equilibrium gas mixture showed 0.562 atm of SO2, 0.101 atm of O2, and 0.332 atm of SO3.
(a) Calculate the equilibrium constant, Kp, for the reaction:
2SO3 (g) ⇆ 2SO2 (g) + O2 (g)
(b) Determine the numerical value of Kc for the above reaction.
(c) Calculate the numerical value of the Kc for the reaction:
SO2 (g) + ½O2 (g) ⇆ SO3 (g)
3. At 298 K, Kc = 2.25 x 102 for the reaction:
2NO (g) ⇆ N2 (g) + O2 (g)
(a) If a container is initially charged with 7.50 M NO, calculate the equilibrium concentration of NO.
(b) What is the percent dissociation of NO?
4. A solution is prepared by dissolving 0.125 moles of calcium chloride in enough water to make 500.0
mL of solution.
(a) Calculate the molarity of the calcium chloride in the solution.
(b) A 100.0 mL sample of the calcium chloride solution is mixed with 10.0 mL of water. Calculate
the molarities of the calcium ions and the chloride ions in the new solution.
(c) Calculate the molarities of the calcium ions and the chloride ions in the new solution.
HOMEWORK 1C
1. Kp is 0.225 at 350ºC for the reaction:
2NO (g) ⇆ N2 (g) + O2 (g)
The tank is initially charged with 0.200 atm NO, 0.100 atm N2, and 0.100 atm O2 at 350ºC.
(a) Is the forward or reverse reaction spontaneous?
(b) Calculate the pressure of NO once equilibrium has been established.
2. For the reaction:
2ClF (g) ⇆ Cl2 (g) + F2 (g)
A 2.50 L flask at equilibrium contains 0.400 moles of ClF, 0.300 moles of Cl2, and 0.100 moles of F2.
(a) Calculate the numerical value of the Kc for the above reaction.
(b) If 0.200 moles of F2 is added to the flask at equilibrium, calculate the new concentration of ClF
when equilibrium is reestablished.
3. Complete each of the following ICE tables, and tell if the x in the ICE table will be large or small.
(a)
I
C
E
(b)
I
C
E
(c)
I
C
E
(d)
I
C
E
A
1.0
+
2B
1.0
⇆
C
0
Keq = 1 x 10-9
A
0
+
2B
0
⇆
C
1.0
Keq = 1 x 10-9
2D
1.0
+
E
1.0
⇆
2F
0
Keq = 1 x 109
2D
0
+
E
0
⇆
2F
1.0
Keq = 1 x 109
4. The equilibrium constant for the reaction:
2HCl (g) ⇆ H2 (g) + Cl2 (g)
at 25ºC is 6.2 x 10-54.
(a) Why was it unnecessary to be told whether the value is for Kp or Kc?
(b) Without any calculations, what does the numerical value of this constant tell you about the
decomopition of HCl?
(c) If 0.010 mole of HCl is placed in a 1.0 liter tank and allowed to come to equilibrium at 25ºC, will
the x in the ICE table be large or small? What will be the final concentration of the hydrogen gas,
in moles per liter?
(d) If 0.0050 mole of Cl2 and 0.0050 mole of H2 are placed together in a 1.0 liter tank and allowed to
come to equilibrium at 25ºC, will the x in the ICE table be large or small? What will be the final
concentration of the hydrogen gas, in moles per liter?
HOMEWORK 1D
1. 3.00 moles of NO, 5.00 moles of ClNO, and 2.00 moles of Cl2 are placed in a 25.0 liter tank at a
temperature of 503 K. After the reaction has come to equilibrium, there are 6.12 moles of ClNO in the
tank.
(a) Write a balanced equation for the reaction producing 1 mole of ClNO from the other two
substances.
(b) Calculate Kc for this reaction at 503 K, with proper units.
(c) Calculate Kp for this reaction at 503 K, with proper units.
2. Ammonia decomposes according to the reaction:
2NH3 (g) ⇆ N2 (g) + 3H2 (g)
A 2.00 liter tank is originally charged with 0.500 moles of ammonia, and at equilibrium it is found that
the ammonia is 16.5% decomposed. Calculate the numerical value of the Kc for the above reaction.
3. A tank of O2 has an initial pressure of 2.00 atm. The O2 undergoes the reaction:
3O2 (g) ⇆ 2O3 (g)
and at equilibrium the total pressure is 1.75 atm. Find Kp for the reaction
4. At 350 K, a 14.0 g sample of N2O gas is placed in an evacuated 10.0 liter container.
(a) What is the pressure of N2O in the container, measured in atmospheres?
(b) The N2O gas decomposes, as shown by the following equation:
2N2O (g) ⇆ 2N2 (g) + O2 (g)
If the N2O from (a) is 20.0% decomposed when equilibrium is established at 350 K, calculate the
value of the Kp for this decomposition reaction.
(c) If the temperature is raised to 400 K, the N2O from (a) is 25.0% decomposed when equilibrium is
reestablished. Calculate the value of the Kc for this decomposition reaction at 400 K.
(d) If the temperature is raised to 450 K, the Kc for this decomposition reaction is 2.7 x 10-2 M. How
many moles of O2 must be added to the container to reduce the quantity of N2O to 0.200 moles at
equilibrium.
5. The following reaction is exothermic:
PCl3 (g) + Cl2 (g) ⇆ PCl5 (g)
For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2)
whether the new equilibrium pressure of PCl5 will be higher, lower, or remain the same.
(a) The addition of a catalyst
(b) A decrease in the volume of the reaction container
(c) Addition of chlorine gas at constant volume
(d) An increase in temperature
(e) Adding argon gas to the reaction container
(f) Addition of PCl5 gas at constant volume.
(continued on next page)
6. The following reaction is endothermic:
CaCO3 (s) ⇆ CaO (s) + CO2 (g)
For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2)
whether the new equilibrium pressure of CO2 will be higher, lower, or remain the same.
(a) A decrease in the volume of the reaction container
(b) Addition of carbon dioxide gas at constant volume
(c) An increase in temperature
(d) Addition of solid CaCO3 at constant volume.
7. For the same reaction in problem 6, indicate whether the new equilibrium mass of CaCO3 will be
higher, lower, or remain the same.
(a) An decrease in the volume of the reaction container
(b) Addition of carbon dioxide gas at constant volume
8. The following reaction is exothermic:
N2 (g) + 3H2 (g) ⇆ 2NH3 (g)
For each of the following properties, indicate how it must change to force the equilibrium to shift to
the right.
(a) Pressure
(b) Temperature
(c) Concentration of N2
(d) Concentration of NH3
HOMEWORK 1E
1. Rank the following acids from weakest to strongest: H4SiO4, H3PO4, H2SO4, HClO4.
2. For the following reaction: C3H7NH2 + CH3OH ⇆ C3H7NH3+ + CH3O(a) Identify the acid, base, conjugate acid and conjugarte base
(b) If the reverse reaction is favored, identify the strongest ascid and strongedt base in the reaction
3. Identify the conjugate base for each of the following:
(a) HF
(b) H2O
(d) HSO4-
(c) NH3
4. Identify the conjugate acid for each of the following:
(a) F-
(b) H2O
(d) HSO4-
(c) NH3
5. Give the missing information for each:
Acid
(a)
Solution 0
H2SO4
Solution 1
H3PO4
Base
HSO4
Solution 3
H2SO4 + H2O → H3O+ + HSO4-
NO3-
(b) Solution 2
(c)
Reaction of the acid in water
-
NH4+
CO32-
(d) Solution 4
(e)
Solution 5
HSO4-
(f)
Solution 6
H 2O
6. Give the missing information for each solution at 25ºC:
[H3O+]
(a)
Solution 1
(b) Solution 2
(c)
[OH-]
pH
pOH
-3
1.25 x 10
5.00 x 10-5
Solution 3
(d) Solution 4
4.50
6.40
7. A detergent box must bear a warning label if its contents will form a solution of pH greater than 11,
because a strong base degrades protein structure. Should a box bear such a label if the H3O+
concentration of a solution of its contents is 2.5 x 10-12 moles per liter?
8. A solution of ammonia has a hydronium ion concentration of 8.0 x 10-9 moles per liter. What is the
pOH of the solution?
9. The Kw for pure water at 60ºC is 9.5 x 10-14.
(a) Calculate the pH of pure water at 60ºC.
(b) Is pure water at 60ºC acidic, basic, or neutral?
HOMEWORK 1F
1. For the following acids, write (1) the reaction for their ionization in water, and (2) their acid ionization
constant expression.
(a) HClO2
(b) HCN
(c) HCO2H
2. Rank the following acids from weakest to strongest: HOC6H5, HClO2, H2O, NH4+.
3. For the following bases, write (1) the reaction for their ionization in water, and (2) their base
dissociation constant expression.
(a) CH3NH2
(b) F-
(c) NO2-
4. For the following acids, predict the numerical values for their acid ionizations constants.
(a) HBrO3
(b) HBrO2
(c) HBrO
5. Calcualte the pH of each of the following strong acid and strong base solutions.
(a) 0.001 M HCl
(b) 0.02 M HNO3
(c) 0.001 M NaOH
(d) 0.001 M Ba(OH)2
6. The acid ionization constant for arsenious acid, HAsO2, is 6.0 x 10-10.
(a) Calculate the pH of a 0.10 M solution of arsenious acid.
(b) Calculate the pOH of a 0.10 M solution of arsenious acid.
7. A 0.10 M solution of trichloroacetic acid, CCl3CO2H, is 1.3% ionized.
(a) Calculate the Ka for the acid.
(b) Calculate the pH of the solution.
8. A solution is 0.25 M in nitrous acid.
(a) Calculate the equilibrium concentration of NO2- in the solution.
(b) Calculate the pH of the solution.
(c) Calculate the percent ionization of HNO2.
9. The base dissociation constant for the organic base pyridine, C5H5N, is 1.58 x 10-8.
(a) Calculate the concentration of C5H5NH+ in a solution that was originally 0.10 M in pyridine.
(b) Calculate the pH of the solution.
10. The base dissociation constant for the weak base hydrazine, N2H4, is 2.0 x 10-6. Calcualte the molar
concentration of hydrazine would yield a pOH of 3.52.
HOMEWORK 1G
1. When sulfur dioxide gas is dissolved in water, it produces a 0.050 M sulfurous acid solution.
(a) Calcualte the concentrations of H+, HSO3-, SO32-, and H2SO3 in the sulfurous acid solution.
(b) Calcualte the pH of the solution?
2. A solution is 0.30 M in sulfuric acid.
(a) Calculate the concentrations of H+, HSO4-, SO42-, and H2SO4 in the sulfuric acid solution.
(b) Calcualte the pH of the solution?
3. A solution is 0.18 M in ammonium chloride.
(a) Which ion is reacting with water?
(b) Is the solution acidic or basic?
(c) What constant is used to calculate the pH?
(d) Calculate the pH of the solution.
4. A solution is 0.025 M in sodium acetate.
(a) Which ion is reacting with water?
(b) Is the solution acidic or basic?
(c) What constant is used to calculate the pH?
(d) Calculate the pH of the solution.
5. A 0.100 M solution of sodium iodite, NaIO2, has a pH of 10.85.
(a) Write the equation for the hydrolysis of NaIO2.
(b) Write the equilibrium constant expression for the hydrolysis reaction. Is it a Ka or Kb expression?
(c) Calculate the value for the equilibrium constant in (b).
(d) Calculate the acid ionization constant for HIO2.
HOMEWORK 1R
1. Write the Kc and Kp expressions for the following reactions.
(a) 2CO2 (g) ⇆ 2CO (g) + O2 (g)
(b) PCl3 (g) + 3NH3 (g) ⇆ 3HCl (g) + P(NH2)3 (g)
(c) H2O (g) + C (s) ⇆ CO (g) + H2 (g)
2. At 298 K the equilibrium constant for the reaction:
N2O4 (g) ⇆ 2NO2 (g)
is given by:
Kc = 4.63 x 10-3
(a) What is the numerical value of Kc for the reaction:
2NO2 (g) ⇆ N2O4 (g)
(b) What is the numerical value of Kc for the reaction:
½N2O4 (g) ⇆ NO2 (g)
(continued on next page)
3. The equilibrium constants for the following reactions are given:
H2CO3 (aq) ⇆ HCO3- (aq) + H+ (aq)
Kc’ = 4.2 x 10-7
HCO3- (aq) ⇆ CO32- (aq) + H+ (aq)
Kc” = 4.8 x 10-11
Calculate the equilibrium constant for the reaction:
H2CO3 (aq) ⇆ CO32- (aq) + 2H+ (aq)
4. The equilibrium constant for the reaction:
H2 (g) + I2 (g) ⇆ 2HI (g)
At 430ºC is 1.6 x 102. The reaction absorbs heat. Determine whether the reaction is spontaneous
forward or in reverse, or whether it is at equilibrium.
(a) A 1.0 L box contains 0.010 mole of H2, 0.010 mole of I2, and 0.40 mole of HI at 430ºC.
(a) A 1.0 L box contains 0.10 mole of H2, 0.10 mole of I2, and 0.40 mole of HI at 430ºC.
(a) A 1.0 L box contains 0.010 mole of H2, 0.10 mole of I2, and 0.40 mole of HI at 430ºC.
5. At 350.ºC, the equilibrium constant for the reaction:
2SO3 (g) ⇆ 2SO2 (g) + O2 (g)
is given by:
Kp = 1.8 x 10-5
(a) What are the proper units (in atmospheres) for the given Kp value?
(b) What is the numerical value of Kc for the reaction?
(c) What would be the proper units for the Kc?
6. Ammonium carbamate, NH4CO2NH2, decomposes as follows:
NH4CO2NH2 (s) ⇆ 2NH3 (g) + CO2 (g)
Starting with only the solid, it is found that at 40°C the total gas pressure at equilibrium is 0.363 atm.
Calculate the numerical value of Kp with proper units.
7. Phosgene gas , COCl2, can be prepared from carbon monoxide gas and chlorine gas as follows:
CO (g) + Cl2 (g) ⇆ COCl2 (g)
3.00 x 10-2 moles of pure phosgene gas was placed in a 1.50 L container, heated to 800. K, and at
equilibrium the pressure of CO was found to be 0.497 atm. Calculate the numerical value of Kp with
proper units.
8. The equilibrium constant for the reaction:
2HF (g) ⇆ H2 (g) + F2 (g)
at a particular temperature is 3.6 x 10-35. A 0.500 L container is originally charged with 0.025 moles of
H2 and 0.025 moles of F2, and allowed to reach equilibrium. Calculate the equilibrium concentrations,
in moles per liter, of H2 and F2 in the container.
(continued on next page)
9. Nitrosyl chloride, NOCl, decomposes as follows:
2NOCl (g) ⇆ 2NO (g) + Cl2 (g)
When a 2.50 mole sample of NOCl was placed in a 1.50 L chamber at 400.°C, and allowed to reach
equilibrium, it was found to be 28.0% decomposed. Calculate the Kp and Kc for the reaction, with
proper units for each.
10. At 500 K, the equilibrium constant for the reaction:
SF6 (g) ⇆ SF4 (g) + F2 (g)
is given by:
Kp = 2.50 x 10-1
A flask is originally charged with 0.500 atm of SF6 and an unknown amount of F2. At equilibrium the
pressure of SF6 was found to be 0.365 atm. Find the initial pressure of the F2.
11. The following reaction produces the deep blue tetraamminecopper(II) complex ion:
Cu2+ (aq) + 4NH3 (aq) ⇆ Cu(NH3)42+ (aq)
To determine the equilibrium constant for the reaction above, an equilibrium solution was prepared by
mixing together 10.00 mL of a 0.0750 M Cu(NO3)2 solution with 5.00 mL of a 0.600 M NH3 solution.
The absorbance of the equilibrium solution was measured at a wavelength of 546 nm in a 1.00 cm
cuvet, and found to be 0.356.
(a) Determine the initial concentrations of
Cu2+ and NH3 in the equilibrium solution.
(b) Using the calibration line to the right,
determine the equilibrium concentration
of Cu(NH3)42+ in the equilibrium
solution.
(c) Determine the equilibrium concentrations
of Cu2+ and NH3 in the equilibrium
solution
(d) Determine the equilibrium constant for
the given reaction.
12. The following reaction is exothermic:
SO2 (g) + Cl2 (g) ⇆ SO2Cl2 (g)
For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2)
whether the new equilibrium moles of SO2Cl2 will be higher, lower, or remain the same.
(a) The addition of a catalyst
(b) A decrease in the volume of the reaction container
(c) Addition of SO2 gas at constant volume
(d) The removal of SO2Cl2 gas at constant volume
(e) An increase in temperature
(f) Adding helium gas to the reaction container
(continued on next page)
13. The following reaction is endothermic:
2Fe(OH)3 (s) ⇆ 2Fe2O3 (s) + 3H2O (g)
For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2)
whether the new equilibrium pressure of water vapor will be higher, lower, or remain the same.
(a) The addition of a catalyst
(b) A decrease in the volume of the reaction container
(c) Addition of water vapor at constant volume
(d) An increase in temperature
(e) Adding argon gas to the reaction container
(f) Addition of solid Fe(OH)3 at constant volume.
14. For the following equilibrium reaction:
Ag2CO3 (s) ⇆ 2Ag+ (aq) + CO32- (aq)
write the net ionic equation for each of the following shifts, and underline the added substance that
caused the shift.
(a) The addition of AgNO3 (aq)
(b) The addition of NaCl (aq)
(c) The addition of HCl (aq)
15. For the following acids, write (1) the reaction for their ionization in water, and (2) their acid ionization
constant expression.
(a) HClO2
(b) NH4+
16. Rank the following acids from weakest to strongest: H2SO4, H2SO3, HSO3-, H2S, HS17. Rank the following acids from weakest to strongest: HC3H5O2, HNO2, HBr, H2O, C5H5NH+
18. For the following bases, write (1) the reaction for their ionization in water, and (2) their base
dissociation constant expression.
(a) (CH3)3N
(b) C6H5O-
19. Rank the following bases from weakest to strongest: NH3, H2NNH2, CH3NH2
20. Rank the following bases from weakest to strongest: F-, H2O, HCO3-, CO3221. What is the pH of each of the following strong acid or strong base solutions?
(a) 0.015 M HClO4
(b) 0.015 M Ca(OH)2
(continued on next page)
22. Formic acid, HCO2H, is a weak acid.
(a) Write the equation for the ionization of formic acid.
(b) Write the equilibrium constant expression for the reaction.
(c) If a 0.10 M formic acid solution has a pH of 2.39, what is formic acid’s acid ionization constant?
(d) If a 0.25 M formic acid solution is 2.7% ionized, what is the pH of the solution?
23. The acid ionization constant for benzoic acid, C6H5CO2H, is 6.5 x 10-5.
(a) Write the equation for the ionization of benzoic acid.
(b) Write the equilibrium constant expression for the reaction.
(c) What is the pH of a 0.10 M solution of benzoic acid?
(d) What is percent ionization of benzoic acid in a 0.10 M solution?
24. Propylamine is a weak base that reacts with water as follows:
C3H7NH2 + H2O ⇆ C3H7NH3+ + OHThe base dissociation constant for this reaction, Kb, is 4.8 x 10-6.
(a) What is the concentration of C3H7NH3+ in a solution that was originally 0.050 M in propylamine?
(b) What is pH of the solution?
25. A solution is 0.250 M in ascorbic acid.
(a) What are the concentrations of H3O+, HC6H6O6-, C6H6O62-, and H2C6H6O6 in the solution?
(b) What is the pH of the solution?
26. Predict whether the solutions of each of the following salts will be acidic, basic, or neutral.
(a) KClO3
(b) NH4NO3
(c) NaC2H3O2
(d) NH4CN
27. A solution is 0.035 M in ammonium bromide, NH4Br.
(a) Write the equation for the hydrolysis of NH4Br.
(b) Write the equilibrium constant expression for the reaction.
(c) Calculate the pH of the solution.
28. A solution 0.035 M in sodium hypochlorite, NaClO, has a pH of 10.00.
(a) Write the equation for the hydrolysis of NaClO.
(b) Write the equilibrium constant expression for the reaction.
(c) Calculate the value for the hydrolysis constant.
(d) Calculate the acid ionization constant for HClO. Compare your answer with the value from
Handout 3.
HOMEWORK 1R ANSWERS
1. (a) Kc = [CO]2[O2]
Kp = pCO2pO2
______________________
________________
[CO2]2
pCO22
(b) Kc = [HCl]3[P(NH2)3]
Kp = pHCl3pP(NH2)3
_____________________ _____________
_______________________
[PCl3][NH3]3
(e) Kc =
[CO][H2]
pPCl3pNH33
Kp =
pCOpH2
____________________
______________
[H2O]
pH2O
2. (a) 216
(b) 0.0680
3. 2.0 x 10-17
4. (a) reverse
(b) forward
(c) equilibrium
5. (a) atm
(b) 3.5 x 10-7
(c) M
6. 7.09 x 10-3 atm3
7. 3.3 atm-1
8. 6.0 x 10-19 M each
9. 1.95 atm, 3.53 x 10-2 M
10. 0.541 atm
11. (a) 0.0500 M Cu2+, 0.167 M NH3
(c) 0.0117 M Cu2+, 0.014 M NH3
12. (a) none, none
(e) left, lower
13. (a) none, same
(e) none, same
(b) right, higher
(b) 0.383 M Cu(NH3)42+
(d) 6.6 x 106
(c) right, higher
(d) right, lower
(c) left, same
(d) right, higher
(f) none, none
(b) left, same
(f) none, same
14. (a) Ag2CO3 (s) ← 2Ag+ (aq) + CO32- (aq)
(b) Ag2CO3 (s) + 2Cl- (aq) → 2AgCl (s) + CO32- (aq)
(c) Ag2CO3 (s) + 2H+ (aq) → 2Ag+ (aq) + H2O (l) + CO2 (g)
15. (a) HClO2 + H2O ⇆ H3O+ + ClO2-
Ka = [H3O+][ClO2-]
______________________________
[HClO2]
(b) NH4+ + H2O ⇆ H3O+ + NH3
Ka = [H3O+][NH3]
____________________________
[NH4+]
(continued on next page)
16. HS-, H2S and HSO3- (tie), H2SO3, H2SO4
17. H2O, C5H5NH+, HC3H5O2, HNO2, HBr
18. (a) (CH3)3N + H2O ⇆ (CH3)3NH+ + OH-
Kb = [(CH3)3NH+][OH-]
_________________________________________
[(CH3)3N]
(b) C6H5O- + H2O ⇆ C6H5OH + OH-
Kb = [C6H5OH][OH-]
____________________________________
[C6H5O-]
19. H2NNH2, NH3, CH3NH2,
20. H2O, F-, HCO3-, CO3221. (a) 1.82
(b) 12.48
22. (a) HCO2H + H2O ⇆ H3O+ + HCO2(b) Ka = [H3O+][HCO2-]
_______________________________
[HCO2H]
-4
(c) 1.7 x 10
(d) 2.17
23. (a) C6H5CO2H + H2O ⇆ H3O+ + C6H5CO2(b) Ka = [H3O+][C6H5CO2-]
______________________________________
[C6H5CO2H]
(c) 2.59
(d) 2.5%
24. (a) 4.9 x 10-4 M
(b) 10.69
25. (a) 0.0044 M H3O+, 0.0044 M HC6H6O6-, 1.6 x 10-12 M C6H6O62-, 0.246 M H2C6H6O6
(b) 2.36
26. (a) neutral
(b) acidic
27. (a) NH4+ + H2O ⇆ H3O+ + NH3
(b) Ka = [H3O+][NH3]
__________________________
[NH4+]
(c) 5.36
28. (a) ClO- + H2O ⇆ HClO + OH(b) Kb = [HClO][OH-]
__________________________
[ClO-]
(c) 2.9 x 10-7
(d) 3.5 x 10-8
(c) basic
(d) basic