3js (a) 6.s0 ).3 623 (13.19 35. A solution has a hydroside-ion concentration of

Question

3js (a) 6.s0 ).3 623 (13.19 35. A solution has a hydroside-ion concentration of 0 0040 M What is the post of the wohtin ay (a) 11.60 (b) 2.40 (0) 7.00 ()8.48 ()5.52 36. What is the pOH of a 0.011 M HI solution? 3)* (a) 4.51 () 12.04 ()9.49 (d) 15.96 ()1.96 37. Which aqueous solution has the lowest pH? (2) a.o.30 MHCI b. 0.30 MNaOH c. 0.30 MNH, d. 0.30 MBa(OH), e. 0.30 MH,so. 38. What is the pOH of a 0.0017 M Ba(OH), solution? 3) a. 8.78 b. 12.43 c. 1.73 d. 2.47 e.2.77 39. A solution has a pH of 10.20 at 25°C. What is the hydroxide-ion concentration at 25°C? 3)* a. 3.8M b. 2.2x102 M c. 1.8x104M d. 6.3x101 M e.1.0x10? M 40. The pH of a solution of a strong base is 11.32 a concentration? (2) t 25°C. What is its hydronium-ion, HsO c. 4.87x 10+ M d. 4.78x 10-13 M e. 478 x 10"2 M a. 2.09 x 10-2 M b. 2.09 × 10-5 M

Explanation / Answer

35) {OH-] = 0.0040M

Thus pOH = - log (0.004)

=2.3979

option B

36)The solution is of a strong acid HI with concentration 0.011M

Thus [H+] = 0.011M

pH = -log (0.011)

= 1.9586

and pOH = 14 - pH

= 14-1.9586

= 12.0414

option b

37) Among the gven options NaOH, NH3 and Ba(OH)2 are bases , hence their pH > 7 .

The remaining two are aids HCl and H2SO4

pH of 0.30M HCl

pH = -log (0.3)

=0.5228

and pH of 0.3M H2 So4

In H2SO4 the [H+] = 2 x0.3 = 0.6 M as it is dibasic acid.

Thus pH = -log (0.6)

= 0.2218

Thus option e is right answer

38) Ba(OH)2 gives two hydroxide ions or it is diacidic base

Thus [OH-] = 2 x 0.0017M

and pOH= -log (2x0.0017)

= 2.4685

Thus option D is correct.

39) pH = 10.20

then [H+] = antilog (-10.20)

= 6.31x10-11 M

we know in any solution [H+] [OH-] = 1.0x10-14 (ionic product 0f water)

Thus [OH-] in the given solution = 1.0x10-14 /6.31x10-11

=1.584x10-4 M

option C

40)

pH = 11.32

then [H+] or [H3O+] = antilog (-11.32)

= 4.786 x 10-12 M

option e

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