1. Final Exam/ Exercises
1- The element in group 3A and period 3 is:
a) Ga b) Be c) Al d) Mg
2- Which compound has the same empirical formula as C3H12O6?
a) C12H20O b) C2H8O c) C6H3O d) C12H24O12
We need to determine the empirical formula for all compounds
C3H12O6 === CH4O2
C12H20O4 === C3H5O
C2H8O4 ===- CH4O2
C6H3O6 ==== C2HO2
C12H24O12 === CH2O

2. Final Exam/ Exercises
1- The element in group 3A and period 3 is:
a) Ga b) Be c) Al d) Mg
2- Which compound has the same empirical formula as C3H12O6?
a) C12H20O b) C2H8O c) C6H3O d) C12H24O12
3- What is the number of protons, electrons and neutrons in the atom of ?
a) 31 protons, 34 electrons, 15 neutrons b) 16 protons, 16 electrons, 16 neutrons
c) 15 protons, 18 electrons, 16 neutrons d) 18 protons, 15 electrons, 31 neutrons
P = 15, e = 15+3 = 18 , n = = 16

3. Final Exam/ Exercises
1- The element in group 3A and period 3 is:
a) Ga b) Be c) Al d) Mg
2- Which compound has the same empirical formula as C3H12O6?
a) C12H20O b) C2H8O c) C6H3O d) C12H24O12
3- What is the number of protons, electrons and neutrons in the atom of ?
a) 31 protons, 34 electrons, 15 neutrons b) 16 protons, 16 electrons, 16 neutrons
c) 15 protons, 18 electrons, 16 neutrons d) 18 protons, 15 electrons, 31 neutrons
4- The correct systematic name for Fe2O3 is
a) Iron (II) oxide b) Iron (III) oxide.
c) Diiron trioxide d) Iron oxide

4. First Exam/ Exercises Summery of naming compound Ionic Molecular
Cation: metal or NH4+
Anion: monotomic or polytomic
Nonmetal + nonmetal
Nonmetal + metalloid
Cation has only
one charge
Cation has more than
one charge
Pair Form one type
of compound
Pair Form more than
one type
of compound
Name first element
add ide to the name of second element
Alkali metal
Alkaline earth metal
Ag+, Al+3, Cd+2, Zn+2
Other metal cations
Name first element
add ide to the name of second element
Add the prefix (prefix mono usually omitted for the first element
Name metal first
Specify charge of metal cation with roman numeral (STOCK SYSTEM)
If monoatomic anion, add ide to the anion
If polyatomic anion use name of anion from previous table
Name metal first
If monoatomic anion, add ide to the anion
If polyatomic anion use name of anion from previous table

5. Final Exam/ Exercises
1- The element in group 3A and period 3 is:
a) Ga b) Be c) Al d) Mg
2- Which compound has the same empirical formula as C3H12O6?
a) C12H20O b) C2H8O c) C6H3O d) C12H24O12
3- What is the number of protons, electrons and neutrons in the atom of ?
a) 31 protons, 34 electrons, 15 neutrons b) 16 protons, 16 electrons, 16 neutrons
c) 15 protons, 18 electrons, 16 neutrons d) 18 protons, 15 electrons, 31 neutrons
4- The correct systematic name for Fe2O3 is
a) Iron (II) oxide b) Iron (III) oxide.
c) Diiron trioxide d) Iron oxide

6. Final Exam/ Exercises
5- A g sample of MgCl2 is dissolved in enough water to give 750 mL of solution. What is the molarity of this solution?
a) 3.70  10-2 M b) 1.05  10-2 M c) 2.58  10-2 M d) 7.99  10-2 M
First we calculate the number of mole
n = / 95 = 0.06 mole
M=n/V
= 0.06 / (750/1000) = 0.08 M = 8 X 10-2 M

7. Final Exam/ Exercises
5- A g sample of MgCl2 is dissolved in enough water to give 750 mL of solution. What is the molarity of this solution?
a) 3.70  10-2 M b) 1.05  10-2 M c) 2.58  10-2 M d) 7.99  10-2 M
6- Calculate the percent composition by mass of O in picric acid (C6H3N3O7)?
a) 1.3 % b) 18.3 % c) 31.4 % d) 48.9 %
Molar mass of C6H3N3O7 =229g/mol
n x molar mass of element
molar mass of compound
x 100%
7 x 16
229
x 100% = 48.9 %

8. a Ba(OH)2 + b HBr → c BaBr2 + d H2O
Final Exam/ Exercises
5- A g sample of MgCl2 is dissolved in enough water to give 750 mL of solution. What is the molarity of this solution?
a) 3.70  10-2 M b) 1.05  10-2 M c) 2.58  10-2 M d) 7.99  10-2 M
6- Calculate the percent composition by mass of O in picric acid (C6H3N3O7)?
a) 1.3 % b) 18.3 % c) 31.4 % d) 48.9 %
7- After balancing the following equation the coefficients are:
a Ba(OH) b HBr → c BaBr2 + d H2O
a) a=1, b=2, c=1, d= b) a=2, b=2, c=1, d=2
c) a=1, b=3, c=1, d= d) a=2, b=1, c=3, d=1

9. a Ba(OH)2 + b HBr → c BaBr2 + d H2O
Final Exam/ Exercises
7- After balancing the following equation the coefficients are:
a Ba(OH) b HBr → c BaBr2 + d H2O
a) a=1, b=2, c=1, d= b) a=2, b=2, c=1, d=2
c) a=1, b=3, c=1, d= d) a=2, b=1, c=3, d=1
Ba(OH) HBr → BaBr2 + H2O
Ba Ba 1
O O X2
Ba(OH) HBr → BaBr2 + 2H2O
Br Br X 2
Ba(OH) HBr → BaBr2 + 2H2O
H X2

10. a Ba(OH)2 + b HBr → c BaBr2 + d H2O
Final Exam/ Exercises
5- A g sample of MgCl2 is dissolved in enough water to give 750 mL of solution. What is the molarity of this solution?
a) 3.70  10-2 M b) 1.05  10-2 M c) 2.58  10-2 M d) 7.99  10-2 M
6- Calculate the percent composition by mass of O in picric acid (C6H3N3O7)?
a) 1.3 % b) 18.3 % c) 31.4 % d) 48.9 %
7- After balancing the following equation the coefficients are:
a Ba(OH) b HBr → c BaBr2 + d H2O
a) a=1, b=2, c=1, d= b) a=2, b=2, c=1, d=2
c) a=1, b=3, c=1, d= d) a=2, b=1, c=3, d=1

11. First we have to determine the limiting reagent:
Final Exam/ Exercises
8- What is the theoretical yield of chromium (Cr) that can be produced by the reaction of 50.0 g of Cr2O3 with 9.00 g of aluminum (Al) according to the chemical reaction?
2 Al + Cr2O3  Al2O Cr
a) 15.4 g b) g c) 19.4 g d) g
First we have to determine the limiting reagent:
First start with Al
1-Convert to mole :
n = 9 / 27 = 0.33 mol
2- from equation
2mole Al ========= 2 mole Cr
0.33 mole Al =====? Mole Cr
2x 0.33 = 2 x ?
Mole of Cr = 0.33 mol
Mass = n x molar mass
= 0.33 x 52
=17.2g
second start with Cr2O3
1-Convert to mole :
n = 50 / 152 = 0.33mol
2- from equation
1mole Cr2O3 ========= 2 mole Cr
0.33mole Cr2O3 =====? Mole Cr
2 x 0.33 = 1 x ?
Mole of Cr = 0.66 mol

12. Final Exam/ Exercises
8- What is the theoretical yield of chromium (Cr) that can be produced by the reaction of 50.0 g of Cr2O3 with 9.00 g of aluminum (Al) according to the chemical reaction?
2 Al + Cr2O3  Al2O Cr
a) 15.4 g b) g c) 19.4 g d) g
9- If the actual yield for the experiment in the above question (8) produced 13.0g, what is the percentage yield?
a) 84.4% b) 75.0% c) 67% d) 96.4%

13. Final Exam/ Exercises
8- What is the theoretical yield of chromium (Cr) that can be produced by the reaction of 50.0 g of Cr2O3 with 9.00 g of aluminum (Al) according to the chemical reaction?
2 Al + Cr2O3  Al2O Cr
a) 15.4 g b) g c) 19.4 g d) g
9- If the actual yield for the experiment in the above question (8) produced 13.0g, what is the percentage yield?
a) 84.4% b) 75.0% c) 67% d) 96.4%
10- What is the mass of carbon in 15 g carbon dioxide (CO2)?
a) 4.1 g b) 2.73 g c) 5.45 g d) 6.82 g

14. Final Exam/ Exercises
10- What is the mass of carbon in 15 g carbon dioxide (CO2)?
a) 4.1 g b) 2.73 g c) 5.45 g d) 6.82 g
Mole of CO2 = mass / molar mass
= 15 / 44 = 0.34 mol
From the formula
1mole C ====== 1 mol CO2
? Mole C ====== 0.34 mole CO2
Mole of C = 0.34 mol
Mass of C = n x molar mass
= 0.34 x 12 = 4.09 g.

15. Final Exam/ Exercises
8- What is the theoretical yield of chromium (Cr) that can be produced by the reaction of 50.0 g of Cr2O3 with 9.00 g of aluminum (Al) according to the chemical reaction?
2 Al + Cr2O3  Al2O Cr
a) 15.4 g b) g c) 19.4 g d) g
9- If the actual yield for the experiment in the above question (8) produced 13.0g, what is the percentage yield?
a) 84.4% b) 75.0% c) 67% d) 96.4%
10- What is the mass of carbon in 15 g carbon dioxide (CO2)?
a) 4.1 g b) 2.73 g c) 5.45 g d) 6.82 g

16. Final Exam/ Exercises
11- Which of the following electron transitions would absorb the lowest energy by the hydrogen atom?
a) from n = 1 to n = b) from n = 1 to n = 5
c) from n = 3 to n = d) from n = 1 to n = 6
12- What mass of helium is required to fill a 2.50 L balloon at STP?
a) g b) g c) g d) 267 g
V= 2.5L, T= 273K, P= 1 atm, Mwt= 4 g/mol
PV= nRT
n= PV/RT
= 1 x 2.5 /( x 273)
= mol
Mass = n x molar mass
= 0.11 x 4 = 0.44 g

17. Final Exam/ Exercises
11- Which of the following electron transitions would absorb the lowest energy by the hydrogen atom?
a) from n = 1 to n = b) from n = 1 to n = 5
c) from n = 3 to n = d) from n = 1 to n = 6
12- What mass of helium is required to fill a 2.50 L balloon at STP?
a) g b) g c) g d) 267 g
13- The electronic configuration of Fe+3 is:
a) [Ar] 4s2 3d b) [Ar] 4s1 3d c) [Ar] 3d d) [Ar] 3d6
14- If the mass of L of gaseous compound was 3.6 g at 35 °C with 1.7atm pressure, the molar mass of the compound is equal to:
a) g/mol b) g/mol c) g/mol d) 100 g/mol

18. Final Exam/ Exercises
14- If the mass of L of gaseous compound was 3.6 g at 35 °C with 1.7atm pressure, the molar mass of the compound is equal to:
a) g/mol b) g/mol c) g/mol d) 100 g/mol
V = 0.21 L, m= 3.6 g, T=35 °C = = 308 K, P= 1.7 atm,
d= mass/volume
= 3.6 / 0.21 = g/L

19. Final Exam/ Exercises
11- Which of the following electron transitions would absorb the lowest energy by the hydrogen atom?
a) from n = 1 to n = b) from n = 1 to n = 5
c) from n = 3 to n = d) from n = 1 to n = 6
12- What mass of helium is required to fill a 2.50 L balloon at STP?
a) g b) g c) g d) 267 g
13- The electronic configuration of Fe+3 is:
a) [Ar] 4s2 3d b) [Ar] 4s1 3d c) [Ar] 3d d) [Ar] 3d6
14- If the mass of L of gaseous compound was 3.6 g at 35 °C with 1.7atm pressure, the molar mass of the compound is equal to:
a) g/mol b) g/mol c) g/mol d) 100 g/mol

20. a) Si2F6 b) SiF3 c) Si3F9 d) Si3F 1- we change from % to g
Final Exam/ Exercises
15- What is the molecular formula of the compound in the above question if you know that it contained 33.0 percent Si and 67.0 percent F by mass?
a) Si2F b) SiF c) Si3F d) Si3F
1- we change from % to g
33 g of Si, 67 g of F
2- change from g to mole using
Divided by the smallest number
of mole which is 1.18
Thus the empirical formula is SiF3
254.68 85
= 3 33 28
= 1.18 mol of Si
Ratio =
nSi =
molecular formula = ratio x empirical formula
= 3 x SiF3 = Si3F9 67 19
= 3.53 mol of F
nF =
1.18
= 1
3.53
1.18
= 3 F:
Si:

21. Final Exam/ Exercises
15- What is the molecular formula of the compound in the above question if you know that it contained 33.0 percent Si and 67.0 percent F by mass?
a) Si2F b) SiF c) Si3F d) Si3F
16-The element 'X' does not usually form compounds with atoms of other elements. Which one of the following could be the electron configuration of 'X'?
a) 1s22s b) 1s22s22p c) 1s22s22p6 d)1s22s22p1
17-''The energy required to remove an electron from a gaseous atom in its ground state" is known as: 
a) Electron affinity b) Electronegativity.
c) Ionization energy d) Ionic radius.

22. Final Exam/ Exercises
18-If the energy (E) of radiation is 6.63 x J, what is the frequency (υ) of this radiation?
a) 1X1010 Hz b) 1X108 Hz c) 1X10-34 Hz d) 1X10-8 Hz

23. Final Exam/ Exercises
18-If the energy (E) of radiation is 6.63 x J, what is the frequency (υ) of this radiation?
a) 1X1010 Hz b) 1X108 Hz c) 1X10-34 Hz d) 1X10-8 Hz
19-How many total valance electrons are available in SO2 ?
a) b) c) d) 24
S=6, O=6
TOTAL = 6 + (6X2)=18

24. Final Exam/ Exercises
18-If the energy (E) of radiation is 6.63 x J, what is the frequency (υ) of this radiation?
a) 1X1010 Hz b) 1X108 Hz c) 1X10-34 Hz d) 1X10-8 Hz
19-How many total valance electrons are available in SO2 ?
a) b) c) d) 24
20-What is the volume of 4.35×10-3 mol gas at 21.2 °C and 0.83 atm?
a) 0.13 L b) 0.2 L c) 0.1L d) 0.3 L
n= 4.35×10-3 mole, T= 21.2 °C= =294.2 K, P= 0.83 atm, V= ?
PV=nRT
V= nRT/P
= 4.35×10-3 x x / 0.83
= 0.13L

25. Final Exam/ Exercises
18-If the energy (E) of radiation is 6.63 x J, what is the frequency (υ) of this radiation?
a) 1X1010 Hz b) 1X108 Hz c) 1X10-34 Hz d) 1X10-8 Hz
19-How many total valance electrons are available in SO2 ?
a) b) c) d) 24
20-What is the volume of 4.35×10-3 mol gas at 21.2 °C and 0.83 atm?
a) 0.13 L b) 0.2 L c) 0.1L d) 0.3 L
21-Calculate the pH of 0.05 M ammonium hydroxide (Kb= 1.8x10-5 at 25°C).
NH4OH (aq) NH4+ (aq) + OH- (aq)
a) b) c) d) 13

26. Final Exam/ Exercises
21-Calculate the pH of 0.05 M ammonium hydroxide (Kb= 1.8x10-5 at 25°C).
NH4OH (aq) NH4+ (aq) + OH- (aq)
a) b) c) d) 13

27. Final Exam/ Exercises
18-If the energy (E) of radiation is 6.63 x J, what is the frequency (υ) of this radiation?
a) 1X1010 Hz b) 1X108 Hz c) 1X10-34 Hz d) 1X10-8 Hz
19-How many total valance electrons are available in SO2 ?
a) b) c) d) 24
20-What is the volume of 4.35×10-3 mol gas at 21.2 °C and 0.83 atm?
a) 0.13 L b) 0.2 L c) 0.1L d) 0.3 L
21-Calculate the pH of 0.05 M ammonium hydroxide (Kb= 1.8x10-5 at 25°C).
NH4OH (aq) NH4+ (aq) + OH- (aq)
a) b) c) d) 13

28. Final Exam/ Exercises
22-Calculate pH of final solution after diluting 10 mL of 0.1 M HCl with 90 mL water.
a) b) c) d) 1.0
First calculate the new concentration of HCl
M1 V1 = M2 V2
0.1 X 10 =M2 X (90+10)
M2= 0.01 M

29. Final Exam/ Exercises
22-Calculate pH of final solution after diluting 10 mL of 0.1 M HCl with 90 mL water.
a) b) c) d) 1.0
23-Arrange the following salts according to increasing of solubility: AgCl (Ksp=1.6x10-10), AgI (Ksp=8.3x10-17), and AgBr (Ksp=7.7x10-13).
a) AgCl >AgI> AgBr b) AgI<AgBr<AgCl
c) AgI>AgBr>AgCl d) AgCl <AgI< AgBr
24-If the solubility of BaSO4 is 1.05x10-5 M at 25 °C, the Ksp of this salt is:
BaSO4 (s) Ba+2 (aq) + SO4-2 (aq)
a) 1.1x b) 2.5x c) 1.05x d) 5x10-20

30. BaSO4 (s) Ba+2 (aq) + SO4-2 (aq)
Final Exam/ Exercises
24-If the solubility of BaSO4 is 1.05x10-5 M at 25 °C, the Ksp of this salt is:
BaSO4 (s) Ba+2 (aq) + SO4-2 (aq)
a) 1.1x b) 2.5x c) 1.05x d) 5x10-20
[Ba+2] = s [SO4-2] = s
Ksp = [Ba+2][SO4-2]
Ksp = s2
s = 1.05x 10 -5mol/L
Ksp = [Ba+2][SO4-2]
Ksp = (1.05x )(1.05x )
Ksp = 1.1x10-10

31. Final Exam/ Exercises
22-Calculate pH of final solution after diluting 10 mL of 0.1 M HCl with 90 mL water.
a) b) c) d) 1.0
23-Arrange the following salts according to increasing of solubility: AgCl (Ksp=1.6x10-10), AgI (Ksp=8.3x10-17), and AgBr (Ksp=7.7x10-13).
a) AgCl >AgI> AgBr b) AgI<AgBr<AgCl
c) AgI>AgBr>AgCl d) AgCl <AgI< AgBr
24-If the solubility of BaSO4 is 1.05x10-5 M at 25 °C, the Ksp of this salt is:
BaSO4 (s) Ba+2 (aq) + SO4-2 (aq)
a) 1.1x b) 2.5x c) 1.05x d) 5x10-20

32. Final Exam/ Exercises
25-For the reaction at equilibrium; N2 (g) + 3 H2 (g) NH3 (g)
If [N2] = 0.1 M, [H2] = 0.2 M and [NH3] = 0.2 M, the equilibrium constant (Kc) is:
a) b) c) d) 200

33. Final Exam/ Exercises
25-For the reaction at equilibrium; N2 (g) + 3 H2 (g) NH3 (g)
If [N2] = 0.1 M, [H2] = 0.2 M and [NH3] = 0.2 M, the equilibrium constant (Kc) is:
a) b) c) d) 200
26-The equilibrium constant for the following reaction at definite temperature is;
H2 (g) + I2 (g) HI (g) K1 = 15
What is the value of the equilibrium constant for the following reaction?
2 HI (g) H2 (g) + I2 (g)
a) b) 6.6x c) 6.6x d) 5x10-3
K2=1/K1
=1/15 =0.066

34. Final Exam/ Exercises
25-For the reaction at equilibrium; N2 (g) + 3 H2 (g) NH3 (g)
If [N2] = 0.1 M, [H2] = 0.2 M and [NH3] = 0.2 M, the equilibrium constant (Kc) is:
a) b) c) d) 200
26-The equilibrium constant for the following reaction at definite temperature is;
H2 (g) + I2 (g) HI (g) K1 = 15
What is the value of the equilibrium constant for the following reaction?
2 HI (g) H2 (g) + I2 (g)
a) b) 6.6x c) 6.6x d) 5x10-3
27-At equilibrium, the total gas pressure was found to be atm. Calculate the equilibrium constant KP for the following decomposition;
NH4CO2NH2 (s) NH3 (g) + CO2 (g)
a) 5.32x b) 5.55x c) 2.22x d) 5.0x10-3

35. Final Exam/ Exercises
27-At equilibrium, the total gas pressure was found to be atm. Calculate the equilibrium constant KP for the following decomposition;
NH4CO2NH2 (s) NH3 (g) + CO2 (g)
a) 5.32x b) 5.55x c) 2.22x d) 5.0x10-3
Pt = P(NH3)+ P(CO2)
= 2P + P
= 3P
0.033 = 3P P= 0.033/3= 0.011
THEN
P(CO2)= 0.011, P(NH3)= 2X0.011=0.022

36. Final Exam/ Exercises
25-For the reaction at equilibrium; N2 (g) + 3 H2 (g) NH3 (g)
If [N2] = 0.1 M, [H2] = 0.2 M and [NH3] = 0.2 M, the equilibrium constant (Kc) is:
a) b) c) d) 200
26-The equilibrium constant for the following reaction at definite temperature is;
H2 (g) + I2 (g) HI (g) K1 = 15
What is the value of the equilibrium constant for the following reaction?
2 HI (g) H2 (g) + I2 (g)
a) b) 6.6x c) 6.6x d) 5x10-3
27-At equilibrium, the total gas pressure was found to be atm. Calculate the equilibrium constant KP for the following decomposition;
NH4CO2NH2 (s) NH3 (g) + CO2 (g)
a) 5.32x b) 5.55x c) 2.22x d) 5.0x10-3

37. Final Exam/ Exercises
28-For the reaction at equilibrium;
Cl2 (g) F2 (g) ClF3 (g)
KC= 3.0x10-2 at 25 °C, the KP of this reaction is:
a) 4.86x b) 2.28x c) 5.0x d) 1.33x10-5
Δn= 2-(1+3)= -2

38. Final Exam/ Exercises
28-For the reaction at equilibrium;
Cl2 (g) F2 (g) ClF3 (g)
KC= 3.0x10-2 at 25 °C, the KP of this reaction is:
a) 4.86x b) 2.28x c) 5.0x d) 1.33x10-5
29-Which of the following is the correct form of the equilibrium constant expression for the reaction;
Cu(s) + 2Ag+(aq) Cu2+ (aq) + 2 Ag(s)
a) Kc = [Cu2+] [2Ag] b) Kc = [Ag]2 [Cu+2] / [Cu] [ Ag]2
c) Kc = [Cu] [2Ag+] / [Cu+2] [2Ag] d) Kc = [Cu2+] / [Ag+]2
30-For the following reaction, at equilibrium which choice gives a change that will shift the position of equilibrium to favor formation of NO?
2NOBr (g)    2NO (g) + Br2 (g), Hº = 30 kJ/mol
a) Increase the total pressure b) Increasing the temperature.
c) Decreasing the temperature d) Removing NOBr selectively.

39. Final Exam/ Exercises
31-The correct name for the following compound is :
a) o-methyltoluene b) m-methyltoluene
c) o-ethyltoluene d) m- ethyltoluene
32-The right systematic name for the following organic molecule is :
a) 5-methyl-3-hexene b) 5-methylhexane
c) 2-methylhexane d) 3-methylhexene
33-HF/NaF system is used as buffer solution. What is the pH if it has [HF] = 0.1M and [NaF] = 0.15M? (Ka= 7.1x10-4 at 25 °C).
HF(aq) H+ (aq) + F-(aq)
NaF(s) Na+ (aq) + F-(aq)
a) b) c) d) 1.4

40. NaF(s) Na+ (aq) + F-(aq) a) 2.12 b) 3.33 c) 0.83 d) 1.4
Final Exam/ Exercises
33-HF/NaF system is used as buffer solution. What is the pH if it has [HF] = 0.1M and [NaF] = 0.15M? (Ka= 7.1x10-4 at 25 °C).
HF(aq) H+ (aq) + F-(aq)
NaF(s) Na+ (aq) + F-(aq)
a) b) c) d) 1.4
pH = pKa + log
[A-]
[HA]
pH = -log 7.1 x log
0.15
0.1
pH = 3.33

41. Final Exam/ Exercises
31-The correct name for the following compound is :
a) o-methyltoluene b) m-methyltoluene
c) o-ethyltoluene d) m- ethyltoluene
32-The right systematic name for the following organic molecule is :
a) 5-methyl-3-hexene b) 5-methylhexane
c) 2-methylhexane d) 3-methylhexene
33-HF/NaF system is used as buffer solution. What is the pH if it has [HF] = 0.1M and [NaF] = 0.15M? (Ka= 7.1x10-4 at 25 °C).
HF(aq) H+ (aq) + F-(aq)
NaF(s) Na+ (aq) + F-(aq)
a) b) c) d) 1.4

42. Ionized acid concentration at equilibrium
Final Exam/ Exercises
34-The percent ionization of hydrofluoric acid (HF) at the concentrations of M ( Ka= 7.1x10-4) is:
HF(aq) H+ (aq) + F-(aq)
a) 3.8% b) 0.6% c) 0.011% d) 2.83%
Ionized acid concentration at equilibrium
Initial concentration of acid
x 100%
percent ionization =
0.19
0.5
x 100%
percent ionization =
= 3.8%

43. Final Exam/ Exercises
34-The percent ionization of hydrofluoric acid (HF) at the concentrations of M ( Ka= 7.1x10-4) is:
HF(aq) H+ (aq) + F-(aq)
a) 3.8% b) 0.6% c) 0.011% d) 2.83%
35-The general molecular formula of alkynes is:
a) CnH2n b) CnH2n c) CnH2n d) CnH2n+1
36-The concentration of hydroxide ion [OH-] in an aqueous solution is 3.5x10-9M.What is the concentration of hydrogen ion [H+]?
a) 2.86 x 10-6M b) 2.86 x 106M c) 3.5 x 10-5M d) 3.5 x 105M

44. Final Exam/ Exercises
34-The percent ionization of hydrofluoric acid (HF) at the concentrations of M ( Ka= 7.1x10-4) is:
HF(aq) H+ (aq) + F-(aq)
a) 3.8% b) 0.6% c) 0.011% d) 2.83%
35-The general molecular formula of alkynes is:
a) CnH2n b) CnH2n c) CnH2n d) CnH2n+1
36-The concentration of hydroxide ion [OH-] in an aqueous solution is 3.5x10-9M.What is the concentration of hydrogen ion [H+]?
a) 2.86 x 10-6M b) 2.86 x 106M c) 3.5 x 10-5M d) 3.5 x 105M

45. Final Exam/ Exercises
37-Which of the following compounds has geometrical isomer?
a) b)
c) d)
38-The right name for the following molecule is:
CH3-CH2-CH2-CO-CH3
a) propyl methyl alchol b) 1-methyl-2-propanal
c) 2-pentanone d) methyl propyl ester
39-Calculate the H+ ion concentration in lemon juice having a pH= 2. 
a) M b) 2.5x10-4 M c) 10.0 M d) 3 M

46. Final Exam/ Exercises
39-Calculate the H+ ion concentration in lemon juice having a pH= 2. 
a) M b) 2.5x10-4 M c) 10.0 M d) 3 M

47. Final Exam/ Exercises
37-Which of the following compounds has geometrical isomer?
a) b)
c) d)
38-The right name for the following molecule is:
CH3-CH2-CH2-CO-CH3
a) propyl methyl alchol b) 1-methyl-2-propanal
c) 2-pentanone d) methyl propyl ester
39-Calculate the H+ ion concentration in lemon juice having a pH= 2. 
a) M b) 2.5x10-4 M c) 10.0 M d) 3 M

48. Final Exam/ Exercises
40-Which expression correctly relates Kp to Kc for the reaction;
2A (g) + B (g) C (g)
a) Kp = Kc(RT)-1 b) Kp = Kc(RT)-2 c) Kp = Kc(RT) d) Kp = Kc

49. Thank you for listening