1. What is equilibrium?
State of balanced rates.
2. What is physical equilibrium?
Equilibrium in physical processes.
3. Give an example of physical equilibrium.
Ice and water.
4. What is chemical equilibrium?
Equal rates of reactions.
5. Give an example of chemical equilibrium.
N 2 + 3 H 2 ⇌ 2 N H 3.
6. What is dynamic equilibrium?
Forward equals reverse rate.
7. What is a reversible reaction?
Proceeds in both directions.
8. What is an irreversible reaction?
Proceeds in one direction.
9. What is the law of mass action?
Rate proportional to concentrations.
10. What is equilibrium constant?
Ratio of product to reactant concentrations.
11. What is the symbol for equilibrium constant?
K c.
12. What is K p in equilibrium?
Equilibrium constant using pressures.
13. What is the relation between K p and K c?
K p
14. What is delta n in K p and K c relation?
Change in moles of gas.
15. What is R in K p and K c relation?
0.0831 bar L per K per mole.
16. What is the unit of K c for a reaction with equal moles?
Dimensionless.
17. What is the unit of K p for a reaction with equal moles?
18. What does a large K c indicate?
Favors products.
19. What does a small K c indicate?
Favors reactants.
20. What is Le Chatelier’s principle?
System adjusts to minimize change.
21. What happens if concentration increases?
Equilibrium shifts forward.
22. What happens if pressure increases?
Shifts to fewer moles.
23. What happens if temperature increases for exothermic reaction?
Shifts backward.
24. What is an exothermic reaction?
Releases heat.
25. What is an endothermic reaction?
Absorbs heat.
26. What is the effect of catalyst on equilibrium?
No shift, faster attainment.
27. What is homogeneous equilibrium?
Same phase reactants, products.
28. Give an example of homogeneous equilibrium.
N 2 + O 2 ⇌ 2 N O.
29. What is heterogeneous equilibrium?
Different phase reactants, products.
30. Give an example of heterogeneous equilibrium.
C a C O 3 ⇌ C a O + C O 2.
31. What is the expression for K c of H 2 + I 2 ⇌ 2 H I?
K c
32. What is the expression for K p of N 2 + 3 H 2 ⇌ 2 N H 3?
33. What is the effect of adding inert gas at constant volume?
No effect on equilibrium.
34. What is the effect of adding inert gas at constant pressure?
Shifts to more moles.
35. What is the equilibrium expression for C O + H 2 O ⇌ C O 2 + H 2?
36. What is the equilibrium expression for P C l 5 ⇌ P C l 3 + C l 2?
37. What is the value of delta n for P C l 5 ⇌ P C l 3 + C l 2?
1.
38. What is the value of delta n for N 2 + 3 H 2 ⇌ 2 N H 3?
-2.
39. What is the value of delta n for H 2 + I 2 ⇌ 2 H I?
0.
40. What is the effect of temperature on K c for endothermic reaction?
Increases with temperature.
41. What is the effect of temperature on K c for exothermic reaction?
Decreases with temperature.
42. What is an acid according to Arrhenius?
Produces H + ions.
43. What is a base according to Arrhenius?
Produces O H - ions.
44. Give an example of an Arrhenius acid.
H C l.
45. Give an example of an Arrhenius base.
N a O H.
46. What is an acid according to Bronsted-Lowry?
Proton donor.
47. What is a base according to Bronsted-Lowry?
Proton acceptor.
48. Give an example of a Bronsted-Lowry acid.
H 2 O.
49. Give an example of a Bronsted-Lowry base.
N H 3.
50. What is a conjugate acid?
Base after accepting proton.
51. What is a conjugate base?
Acid after donating proton.
52. What is the conjugate base of H C l?
C l -.
53. What is the conjugate acid of N H 3?
N H 4 +.
54. What is an acid according to Lewis?
Electron pair acceptor.
55. What is a base according to Lewis?
Electron pair donor.
56. Give an example of a Lewis acid.
B F 3.
57. Give an example of a Lewis base.
58. What is the ionisation constant of water?
K w
59. What is the value of K w at 298 K?
1.0 × 10^-14.
60. What is pH?
-log[H +].
61. What is pOH?
-log[O H -].
62. What is the relation between pH and pOH?
pH + pOH
63. What is the pH of a neutral solution at 298 K?
7.
64. What is the pH of an acidic solution?
Less than 7.
65. What is the pH of a basic solution?
More than 7.
66. What is the pH of 0.1 M H C l?
67. What is the pH of 0.01 M N a O H?
12.
68. What is a strong acid?
Fully ionises in water.
69. Give an example of a strong acid.
H N O 3.
70. What is a weak acid?
Partially ionises in water.
71. Give an example of a weak acid.
C H 3 C O O H.
72. What is a strong base?
73. Give an example of a strong base.
K O H.
74. What is a weak base?
75. Give an example of a weak base.
N H 4 O H.
76. What is the ionisation constant of a weak acid?
K a
77. What is the ionisation constant of a weak base?
K b
78. What is pK a?
-log K a.
79. What is pK b?
-log K b.
80. What is the relation between K a and K b for conjugate pairs?
K a × K b
81. What is the relation between pK a and pK b?
pK a + pK b
82. What is a buffer solution?
Resists pH change.
83. What is an acidic buffer?
Weak acid and its salt.
84. Give an example of an acidic buffer.
C H 3 C O O H + C H 3 C O O N a.
85. What is a basic buffer?
Weak base and its salt.
86. Give an example of a basic buffer.
N H 4 O H + N H 4 C l.
87. What is the Henderson-Hasselbalch equation for acidic buffer?
pH
88. What is the Henderson-Hasselbalch equation for basic buffer?
pOH
89. What is the pH of a buffer with equal acid and salt concentrations?
90. What is the solubility product?
K sp
91. What is the K sp expression for A g C l?
92. What is the K sp expression for C a F 2?
93. What happens if ionic product exceeds K sp?
Precipitation occurs.
94. What is the common ion effect?
Reduces solubility by common ion.
95. Give an example of the common ion effect.
A g C l with N a C l.
96. What is the effect of temperature on K w?
97. What is the pH of 0.001 M H 2 S O 4?
2.
98. What is the pH of 0.02 M C H 3 C O O H (K a
3.37.
99. What is the pOH of 0.01 M N H 4 O H (K b
2.74.
100. What is the degree of ionisation of 0.1 M H C O O H (K a
0.042.
101. What is the K a of a weak acid with pK a
1.58 × 10^-5.
102. What is the K sp of A g 2 C r O 4 if solubility is 2 × 10^-5 M?
3.2 × 10^-14.
103. What is the solubility of B a S O 4 (K sp
1.05 × 10^-5 M.
104. What is the pH of a solution with [H +]
8.
105. What is the pOH of a solution with [O H -]
6.
106. What is the effect of dilution on weak acid ionisation?
Increases ionisation.
107. What is the conjugate base of H 2 O?
O H -.
108. What is the conjugate acid of O H -?
109. What is the conjugate base of H 2 S O 4?
H S O 4 -.
110. What is the conjugate acid of H S O 4 -?
H 2 S O 4.
111. What is the conjugate base of N H 4 +?
112. What is the conjugate acid of C H 3 C O O -?
113. What is the pH of 0.05 M H N O 3?
1.3.
114. What is the pH of 0.002 M K O H?
11.3.
115. What is the K b of N H 3 if K a of N H 4 + is 5.6 × 10^-10?
1.79 × 10^-5.
116. What is the pH of a buffer with 0.1 M C H 3 C O O H and 0.2 M C H 3 C O O N a (pK a
5.04.
117. What is the solubility of A g C l (K sp
1.34 × 10^-5 M.
118. What is the effect of adding N H 4 C l to N H 4 O H solution?
Decreases pH.
119. What is the effect of adding N a C l to A g C l solution?
Decreases solubility.
120. What is the pH of 10^-7 M H C l?
7 (neutral due to water).
121. What is the K sp expression for A l ( O H ) 3?
122. What is the K sp expression for B a 3 ( P O 4 ) 2?
123. What is the degree of ionisation of 0.01 M N H 4 O H (K b
124. What is the pH of 0.1 M N H 4 C l (K b of N H 3
5.13.
125. What is the pH of 0.1 M N a C N (K a of H C N
11.15.
126. What is hydrolysis of a salt?
Reaction with water forming ions.
127. What is the pH of a salt of strong acid and weak base?
128. What is the pH of a salt of weak acid and strong base?
129. What is the pH of a salt of strong acid and strong base?
130. What is the hydrolysis constant of N H 4 C l?
K h
131. What is the hydrolysis constant of N a C H 3 C O O?
132. What is the pH of 0.1 M N a H C O 3 (pK a1
8.34.
133. What is the K a1 of H 2 C O 3?
4.5 × 10^-7.
134. What is the K a2 of H 2 C O 3?
4.7 × 10^-11.
135. What is the pH of 0.01 M H 3 P O 4 (K a1
2.12.
136. What is the K sp of C a C O 3 if solubility is 5 × 10^-5 M?
2.5 × 10^-9.
137. What is the solubility of P b C l 2 (K sp
1.62 × 10^-2 M.
138. What is the effect of increasing [H +] on C a F 2 solubility?
Increases solubility.
139. What is the pH of a saturated solution of M g ( O H ) 2 (K sp
10.35.
140. What is the K c expression for 2 S O 2 + O 2 ⇌ 2 S O 3?
141. What is the K p expression for 2 S O 2 + O 2 ⇌ 2 S O 3?
142. What is the value of delta n for 2 S O 2 + O 2 ⇌ 2 S O 3?
-1.
143. What is the effect of increasing pressure on N 2 O 4 ⇌ 2 N O 2?
144. What is the effect of decreasing temperature on N 2 O 4 ⇌ 2 N O 2 (endothermic)?
145. What is the K c expression for C O C l 2 ⇌ C O + C l 2?
146. What is the K p expression for C a C O 3 ⇌ C a O + C O 2?
147. What is the effect of adding C a O to C a C O 3 ⇌ C a O + C O 2?
No effect (solid).
148. What is the pH of 0.001 M C a ( O H ) 2?
149. What is the pH of 0.05 M N H 4 O H (K b
11.13.
150. What is the K a of H F if pK a
6.76 × 10^-4.
151. What is the pH of 0.1 M H F (K a
2.08.
152. What is the solubility of A g 2 S O 4 (K sp
1.52 × 10^-2 M.
153. What is the K sp of Z n S if solubility is 3 × 10^-12 M?
9 × 10^-24.
154. What is the pH of a buffer with 0.2 M H C O O H and 0.1 M H C O O N a (pK a
3.47.
155. What is the pOH of a buffer with 0.1 M N H 4 O H and 0.2 M N H 4 C l (pK b
156. What is the degree of ionisation of 0.05 M H C N (K a
3.13 × 10^-4.
157. What is the pH of 0.01 M N a 2 C O 3 (pK a2
11.66.
158. What is the K sp expression for P b I 2?
159. What is the solubility of P b I 2 (K sp
1.26 × 10^-3 M.
160. What is the effect of adding N a F to C a F 2 solution?
161. What is the pH of 0.1 M H 2 C 2 O 4 (K a1
1.28.
162. What is the K a1 of H 2 S?
9.5 × 10^-8.
163. What is the K a2 of H 2 S?
1 × 10^-19.
164. What is the pH of 0.1 M H 2 S (K a1
4.02.
165. What is the K sp of M g C O 3 if solubility is 1.8 × 10^-4 M?
3.24 × 10^-8.
166. What is the solubility of C u S (K sp
7.94 × 10^-18 M.
167. What is the pH of a saturated solution of C a ( O H ) 2 (K sp
12.37.
168. What is the K c expression for N H 4 H S ⇌ N H 3 + H 2 S?
169. What is the K p expression for N H 4 H S ⇌ N H 3 + H 2 S?
170. What is the value of delta n for N H 4 H S ⇌ N H 3 + H 2 S?
171. What is the effect of increasing temperature on H 2 + I 2 ⇌ 2 H I (exothermic)?
172. What is the effect of increasing pressure on H 2 + I 2 ⇌ 2 H I?
No effect.
173. What is the K c expression for 2 N O + O 2 ⇌ 2 N O 2?
174. What is the K p expression for 2 N O + O 2 ⇌ 2 N O 2?
175. What is the value of delta n for 2 N O + O 2 ⇌ 2 N O 2?
176. What is the effect of adding H e at constant volume to P C l 5 ⇌ P C l 3 + C l 2?
177. What is the pH of 0.02 M B a ( O H ) 2?
12.6.
178. What is the pH of 0.005 M H 2 S O 4?
179. What is the K b of C H 3 N H 2 if pK b
4.17 × 10^-4.
180. What is the pH of 0.1 M C H 3 N H 2 (K b
11.62.
181. What is the solubility of A g 2 C O 3 (K sp
1.27 × 10^-4 M.
182. What is the K sp of C u C O 3 if solubility is 1.4 × 10^-5 M?
1.96 × 10^-10.
183. What is the pH of a buffer with 0.05 M H 3 P O 4 and 0.1 M N a H 2 P O 4 (pK a1
2.44.
184. What is the pOH of a buffer with 0.2 M N H 4 O H and 0.1 M N H 4 C l (pK b
4.44.
185. What is the degree of ionisation of 0.02 M H 3 B O 3 (K a
5.38 × 10^-4.
186. What is the pH of 0.1 M N a 2 H P O 4 (pK a2
9.61.
187. What is the K sp expression for F e ( O H ) 3?
188. What is the solubility of F e ( O H ) 3 (K sp
1.9 × 10^-10 M.
189. What is the effect of adding N H 4 C l to N H 4 H S ⇌ N H 3 + H 2 S?
190. What is the pH of 0.05 M H 3 P O 3 (K a1
1.59.
191. What is the K a1 of H 3 P O 3?
1.6 × 10^-2.
192. What is the K a2 of H 3 P O 3?
7 × 10^-7.
193. What is the pH of 0.01 M H 3 P O 3 (K a1
2.09.
194. What is the K sp of Z n C O 3 if solubility is 3.8 × 10^-5 M?
1.44 × 10^-9.
195. What is the solubility of H g S (K sp
4 × 10^-26 M.
196. What is the pH of a saturated solution of S r ( O H ) 2 (K sp
12.52.
197. What is the K c expression for C H 3 C O O H ⇌ C H 3 C O O - + H +?
198. What is the K p expression for N 2 O 4 ⇌ 2 N O 2?
199. What is the value of delta n for N 2 O 4 ⇌ 2 N O 2?
200. What is the effect of decreasing volume on C O C l 2 ⇌ C O + C l 2?
201. What is the effect of adding C l 2 to C O C l 2 ⇌ C O + C l 2?
202. What is the K c expression for H 2 S ⇌ H + + H S -?
203. What is the K p expression for 2 H 2 O ⇌ 2 H 2 + O 2?
204. What is the value of delta n for 2 H 2 O ⇌ 2 H 2 + O 2?
205. What is the effect of adding A r at constant pressure to N 2 + 3 H 2 ⇌ 2 N H 3?
Shifts forward.
206. What is the pH of 0.001 M S r ( O H ) 2?
207. What is the pH of 0.02 M H C O O H (K a
2.72.
208. What is the K a of H C N if pK a
4.9 × 10^-10.
209. What is the pH of 0.05 M H C N (K a
5.34.
210. What is the solubility of C a 3 ( P O 4 ) 2 (K sp
1.4 × 10^-7 M.
211. What is the K sp of N i S if solubility is 3.2 × 10^-10 M?
1.02 × 10^-19.
212. What is the pH of a buffer with 0.1 M H 2 C O 3 and 0.2 M N a H C O 3 (pK a1
6.65.
213. What is the pOH of a buffer with 0.05 M N H 4 O H and 0.1 M N H 4 C l (pK b
214. What is the degree of ionisation of 0.1 M H F (K a
0.082.
215. What is the pH of 0.1 M N a H 2 P O 4 (pK a1
4.67.
216. What is the K sp expression for A g 3 P O 4?
217. What is the solubility of A g 3 P O 4 (K sp
1.3 × 10^-4 M.
218. What is the effect of adding N a 2 S O 4 to B a S O 4 solution?
219. What is the pH of 0.02 M H 2 C O 3 (K a1
220. What is the K a1 of H 2 C 2 O 4?
5.9 × 10^-2.
221. What is the K a2 of H 2 C 2 O 4?
6.4 × 10^-5.
222. What is the pH of 0.05 M H 2 C 2 O 4 (K a1
223. What is the K sp of P b C O 3 if solubility is 1.1 × 10^-7 M?
1.21 × 10^-14.
224. What is the solubility of A g 2 S (K sp
1.16 × 10^-16 M.
225. What is the pH of a saturated solution of B a ( O H ) 2 (K sp
13.1.
226. What is the K c expression for C H 4 + 2 O 2 ⇌ C O 2 + 2 H 2 O?
Not applicable (irreversible).
227. What is the K p expression for 2 N H 3 ⇌ N 2 + 3 H 2?
228. What is the value of delta n for 2 N H 3 ⇌ N 2 + 3 H 2?
229. What is the effect of increasing temperature on 2 N O 2 ⇌ N 2 O 4 (exothermic)?
230. What is the effect of adding N 2 to N 2 + 3 H 2 ⇌ 2 N H 3?
231. What is the K c expression for H C O O H ⇌ H + + H C O O -?
232. What is the K p expression for 2 S O 3 ⇌ 2 S O 2 + O 2?
233. What is the value of delta n for 2 S O 3 ⇌ 2 S O 2 + O 2?
234. What is the effect of decreasing pressure on P C l 5 ⇌ P C l 3 + C l 2?
235. What is the pH of 0.005 M M g ( O H ) 2?
11.7.
236. What is the pH of 0.01 M C H 3 C O O H (K a
237. What is the K b of N H 2 O H if pK b
1.1 × 10^-6.
238. What is the pH of 0.02 M N H 2 O H (K b
10.17.
239. What is the solubility of C a S O 4 (K sp
3.02 × 10^-3 M.
240. What is the K sp of C d S if solubility is 1.4 × 10^-15 M?
1.96 × 10^-30.
241. What is the pH of a buffer with 0.1 M H 3 P O 3 and 0.05 M N a H 2 P O 3 (pK a1
1.5.
242. What is the pOH of a buffer with 0.1 M N H 4 O H and 0.05 M N H 4 C l (pK b
243. What is the degree of ionisation of 0.05 M H C O O H (K a
0.06.
244. What is the pH of 0.1 M N a 3 P O 4 (pK a3
12.34.
245. What is the K sp expression for H g 2 C l 2?
246. What is the solubility of H g 2 C l 2 (K sp
6.9 × 10^-7 M.
247. What is the effect of adding N a C l to A g C l solution?
248. What is the pH of 0.01 M H 3 P O 4 (K a1
249. What is the K a1 of H 3 P O 4?
7.5 × 10^-3.
250. What is the K a2 of H 3 P O 4?
6.2 × 10^-8.
251. What is the pH of 0.05 M H 3 P O 4 (K a1
1.62.
252. What is the K sp of S r C O 3 if solubility is 7 × 10^-6 M?
4.9 × 10^-11.
253. What is the solubility of M n S (K sp
5 × 10^-7 M.
254. What is the pH of a saturated solution of Z n ( O H ) 2 (K sp
8.88.
255. What is the K c expression for N H 4 O H ⇌ N H 4 + + O H -?
256. What is the K p expression for 2 H I ⇌ H 2 + I 2?
257. What is the value of delta n for 2 H I ⇌ H 2 + I 2?
258. What is the effect of increasing volume on N 2 O 4 ⇌ 2 N O 2?
259. What is the effect of adding S O 2 to 2 S O 2 + O 2 ⇌ 2 S O 3?
260. What is the K c expression for H 3 B O 3 ⇌ H + + H 2 B O 3 -?
261. What is the K p expression for C O 2 + H 2 ⇌ C O + H 2 O?
262. What is the value of delta n for C O 2 + H 2 ⇌ C O + H 2 O?
263. What is the effect of increasing temperature on C O C l 2 ⇌ C O + C l 2 (endothermic)?
264. What is the pH of 0.002 M C a ( O H ) 2?
11.6.
265. What is the pH of 0.05 M H N O 2 (K a
2.17.
266. What is the K a of H O C l if pK a
3.47 × 10^-8.
267. What is the pH of 0.1 M H O C l (K a
4.76.
268. What is the solubility of P b S O 4 (K sp
1.26 × 10^-4 M.
269. What is the K sp of F e S if solubility is 6 × 10^-10 M?
3.6 × 10^-19.
270. What is the pH of a buffer with 0.2 M H F and 0.1 M N a F (pK a
2.87.
271. What is the pOH of a buffer with 0.1 M N H 4 O H and 0.2 M N H 4 C l (pK b
272. What is the degree of ionisation of 0.01 M H N O 2 (K a
0.2.
273. What is the pH of 0.1 M N a H C O 3 (pK a1
274. What is the K sp expression for C u ( I O 3 ) 2?
275. What is the solubility of C u ( I O 3 ) 2 (K sp
2.6 × 10^-3 M.
276. What is the effect of adding N a 2 C O 3 to C a C O 3 solution?
277. What is the pH of 0.05 M H 3 B O 3 (K a
5.77.
278. What is the K a of H 3 B O 3?
5.8 × 10^-10.
279. What is the pH of 0.01 M H 3 B O 3 (K a
6.12.
280. What is the K sp of B a C O 3 if solubility is 4 × 10^-5 M?
1.6 × 10^-9.
281. What is the solubility of C d C O 3 (K sp
3.16 × 10^-7 M.
282. What is the pH of a saturated solution of F e ( O H ) 2 (K sp
9.83.
283. What is the K c expression for H F ⇌ H + + F -?
284. What is the K p expression for 2 N O 2 ⇌ 2 N O + O 2?
285. What is the value of delta n for 2 N O 2 ⇌ 2 N O + O 2?
286. What is the effect of decreasing temperature on N 2 + 3 H 2 ⇌ 2 N H 3 (exothermic)?
287. What is the effect of adding H 2 to C O + H 2 ⇌ C O + H 2 O?
288. What is the K c expression for H C N ⇌ H + + C N -?
289. What is the K p expression for C O + 2 H 2 ⇌ C H 3 O H?
290. What is the value of delta n for C O + 2 H 2 ⇌ C H 3 O H?
291. What is the effect of increasing pressure on C O + 2 H 2 ⇌ C H 3 O H?
292. What is the pH of 0.01 M B a ( O H ) 2?
12.3.
293. What is the pH of 0.02 M H O C l (K a
5.08.
294. What is the K b of C 2 H 5 N H 2 if pK b
6.46 × 10^-4.
295. What is the pH of 0.1 M C 2 H 5 N H 2 (K b
11.67.
296. What is the solubility of S r S O 4 (K sp
5.83 × 10^-4 M.
297. What is the K sp of P b S if solubility is 3.4 × 10^-14 M?
1.16 × 10^-27.
298. What is the pH of a buffer with 0.05 M H N O 2 and 0.1 M N a N O 2 (pK a
3.65.
299. What is the pOH of a buffer with 0.2 M N H 4 O H and 0.05 M N H 4 C l (pK b
4.14.
300. What is the degree of ionisation of 0.05 M H C l O (K a
2.45 × 10^-3.
301. What is the pH of 0.1 M N a 2 C 2 O 4 (pK a2
8.60.
302. What is the K sp expression for Z n 3 ( P O 4 ) 2?
303. What is the solubility of Z n 3 ( P O 4 ) 2 (K sp
1.5 × 10^-7 M.
304. What is the effect of adding N a I to P b I 2 solution?
305. What is the pH of 0.01 M H 2 S O 3 (K a1
2.07.
306. What is the K a1 of H 2 S O 3?
1.7 × 10^-2.
307. What is the K a2 of H 2 S O 3?
308. What is the pH of 0.05 M H 2 S O 3 (K a1
1.57.
309. What is the K sp of C u C O 3 if solubility is 1.4 × 10^-5 M?
310. What is the solubility of N i C O 3 (K sp
3.6 × 10^-4 M.
311. What is the pH of a saturated solution of C u ( O H ) 2 (K sp
9.42.
312. What is the K c expression for C H 3 N H 2 + H 2 O ⇌ C H 3 N H 3 + + O H -?
313. What is the K p expression for C H 3 O H ⇌ C O + 2 H 2?
314. What is the value of delta n for C H 3 O H ⇌ C O + 2 H 2?
315. What is the effect of increasing volume on C O + 2 H 2 ⇌ C H 3 O H?
316. What is the effect of adding C O to C O + 2 H 2 ⇌ C H 3 O H?
317. What is the K c expression for H 2 C O 3 ⇌ H + + H C O 3 -?
318. What is the K p expression for 2 C O 2 ⇌ 2 C O + O 2?
319. What is the value of delta n for 2 C O 2 ⇌ 2 C O + O 2?
320. What is the effect of decreasing pressure on C O + 2 H 2 ⇌ C H 3 O H?
321. What is the pH of 0.001 M M g ( O H ) 2?
322. What is the pH of 0.01 M H C l O (K a
4.77.
323. What is the K b of ( C H 3 ) 2 N H if pK b
5.37 × 10^-4.
324. What is the pH of 0.1 M ( C H 3 ) 2 N H (K b
11.64.
325. What is the solubility of B a F 2 (K sp
3.56 × 10^-3 M.
326. What is the K sp of A g I if solubility is 9.1 × 10^-9 M?
8.28 × 10^-17.
327. What is the pH of a buffer with 0.1 M H 2 S O 3 and 0.2 M N a H S O 3 (pK a1
328. What is the pOH of a buffer with 0.05 M N H 4 O H and 0.2 M N H 4 C l (pK b
329. What is the degree of ionisation of 0.02 M H C O O H (K a
0.094.
330. What is the pH of 0.1 M N a 2 S O 3 (pK a2
10.10.
331. What is the K sp expression for C a 3 ( A s O 4 ) 2?
332. What is the solubility of C a 3 ( A s O 4 ) 2 (K sp
2.3 × 10^-4 M.
333. What is the effect of adding N a 2 S O 4 to P b S O 4 solution?
334. What is the pH of 0.05 M H C O O H (K a
2.37.
335. What is the K a1 of H 2 S O 4?
Very large (strong acid).
336. What is the K a2 of H 2 S O 4?
1.2 × 10^-2.
337. What is the pH of 0.01 M H 2 S O 4 (K a2
1.96.
338. What is the K sp of M n C O 3 if solubility is 6.5 × 10^-6 M?
4.23 × 10^-11.
339. What is the solubility of C u S (K sp
340. What is the pH of a saturated solution of N i ( O H ) 2 (K sp
9.74.
341. What is the K c expression for ( C H 3 ) 2 N H + H 2 O ⇌ ( C H 3 ) 2 N H 2 + + O H -?
342. What is the K p expression for 2 C H 4 ⇌ C 2 H 4 + H 2?
343. What is the value of delta n for 2 C H 4 ⇌ C 2 H 4 + H 2?
344. What is the effect of increasing pressure on 2 C H 4 ⇌ C 2 H 4 + H 2?
345. What is the effect of adding H 2 to C H 3 O H ⇌ C O + 2 H 2?
346. What is the K c expression for H 2 C 2 O 4 ⇌ H + + H C 2 O 4 -?
347. What is the K p expression for C O C l 2 ⇌ C O + C l 2?
348. What is the value of delta n for C O C l 2 ⇌ C O + C l 2?
349. What is the effect of increasing temperature on 2 H 2 + O 2 ⇌ 2 H 2 O (exothermic)?
350. What is the pH of 0.005 M S r ( O H ) 2?
351. What is the pH of 0.01 M H 3 P O 3 (K a1
352. What is the K b of C 6 H 5 N H 2 if pK b
3.98 × 10^-10.
353. What is the pH of 0.1 M C 6 H 5 N H 2 (K b
8.80.
354. What is the solubility of A g 2 C r O 4 (K sp
6.5 × 10^-5 M.
355. What is the K sp of Z n S if solubility is 3 × 10^-12 M?
356. What is the pH of a buffer with 0.1 M H 3 P O 4 and 0.2 M N a H 2 P O 4 (pK a1
357. What is the pOH of a buffer with 0.2 M N H 4 O H and 0.1 M N H 4 C l (pK b
358. What is the degree of ionisation of 0.05 M H 2 C 2 O 4 (K a1
0.72.
359. What is the pH of 0.1 M N a 2 C O 3 (pK a2
360. What is the K sp expression for P b 3 ( P O 4 ) 2?
361. What is the solubility of P b 3 ( P O 4 ) 2 (K sp
1.6 × 10^-9 M.
362. What is the effect of adding N a F to C a F 2 solution?
363. What is the pH of 0.02 M H 3 P O 4 (K a1
364. What is the K a1 of H 3 P O 4?
365. What is the K a2 of H 3 P O 4?
366. What is the pH of 0.1 M H 3 P O 4 (K a1
1.52.
367. What is the K sp of A g 2 C O 3 if solubility is 1.3 × 10^-4 M?
8.79 × 10^-12.
368. What is the solubility of F e C O 3 (K sp
5.57 × 10^-6 M.
369. What is the pH of a saturated solution of A g 2 C O 3 (K sp
10.33 (with hydrolysis).
370. What is the K c expression for C 6 H 5 N H 2 + H 2 O ⇌ C 6 H 5 N H 3 + + O H -?
371. What is the K p expression for 2 H 2 S ⇌ 2 H 2 + S 2?
372. What is the value of delta n for 2 H 2 S ⇌ 2 H 2 + S 2?
373. What is the effect of increasing pressure on 2 H 2 S ⇌ 2 H 2 + S 2?
374. What is the effect of adding C l 2 to P C l 3 + C l 2 ⇌ P C l 5?
375. What is the K c expression for H 2 S O 3 ⇌ H + + H S O 3 -?
376. What is the K p expression for 2 N O C l ⇌ 2 N O + C l 2?
377. What is the value of delta n for 2 N O C l ⇌ 2 N O + C l 2?
378. What is the effect of decreasing volume on 2 N O C l ⇌ 2 N O + C l 2?
379. What is the pH of 0.002 M B a ( O H ) 2?
380. What is the pH of 0.05 M H 2 C O 3 (K a1
3.67.
381. What is the K a of C H 3 C H 2 C O O H if pK a
1.35 × 10^-5.
382. What is the pH of 0.1 M C H 3 C H 2 C O O H (K a
2.94.
383. What is the solubility of C a C O 3 (K sp
6.16 × 10^-5 M.
384. What is the K sp of C u I if solubility is 1.1 × 10^-6 M?
1.21 × 10^-12.
385. What is the pH of a buffer with 0.2 M H C O O H and 0.1 M H C O O N a (pK a
386. What is the pOH of a buffer with 0.1 M N H 4 O H and 0.05 M N H 4 C l (pK b
387. What is the degree of ionisation of 0.01 M C H 3 C H 2 C O O H (K a
0.036.
388. What is the pH of 0.1 M N a H S O 3 (pK a1
4.48.
389. What is the K sp expression for F e 2 ( S O 4 ) 3?
390. What is the solubility of F e 2 ( S O 4 ) 3 (K sp
2.5 × 10^-4 M.
391. What is the effect of adding N a 2 S to C u S solution?
392. What is the pH of 0.01 M C H 3 C H 2 C O O H (K a
3.44.
393. What is the K a1 of H 2 S O 4?
394. What is the K a2 of H 2 S O 4?
395. What is the pH of 0.05 M H 2 S O 4 (K a2
1.39.
396. What is the K sp of S r C O 3 if solubility is 7 × 10^-6 M?
397. What is the solubility of Z n C O 3 (K sp
3.74 × 10^-6 M.
398. What is the pH of a saturated solution of M g ( O H ) 2 (K sp
399. What is the K c expression for C H 3 C H 2 C O O H ⇌ H + + C H 3 C H 2 C O O -?
400. What is the K p expression for 2 C O + O 2 ⇌ 2 C O 2?
401. What is the value of delta n for 2 C O + O 2 ⇌ 2 C O 2?
402. What is the effect of increasing pressure on 2 C O + O 2 ⇌ 2 C O 2?
403. What is the effect of adding C O 2 to 2 C O + O 2 ⇌ 2 C O 2?
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