NOM NOM NOM
Which concentration units make it possible to determine a titration calculation without a balanced equation?
Normality
A 50 mL sample of a solution containing sulfuric acid
(H2SO4) is titrated with 0.1 M sodium hydroxide (NaOH). It takes 30 mL of the NaOH solution to reach the equivalence point. What is the molarity of the sulfuric acid solution?
0.1 M NaOH = 0.1 N
Na = 0.06
0.06 N H2SO4 = 0.06 M
What is the concentration of OH- ions in a solution with a pH of 9.00?
pOH = 5.00
OH = 1.0 x 10-5
Calculate the pH of a buffer solution that contains 0.1 M acetic acid (Ka = 1.8 x 10-5) and 0.1 M sodium acetate.
pKa = 4.7447
pH = 5
When lead-210 undergoes beta decay, a beta particle is emitted and a new element is produced. What is that element?
210 Bi
83
If you have 250.00 ml of a 0.25 M solution of iron (III) sulfate, Fe2(SO4)3 you would have a solution that is what molarity in sulfate ions?
0.75 M
A 50 mL sample of a solution containing acetic acid (CH3COOH) is titrated with 0.1 M sodium hydroxide (NaOH). It takes 40 mL of the NaOH solution to reach the equivalence point. What is the molarity of the acetic acid solution?
0.1 M NaOH = 0.1 N
Na = 0.08
0.08 N CH3COOH = 0.08 M
Calculate the pH of a solution with [OH-] = 1.0 × 10-10 M
pOH = 10
pH = 4.0
Calculate the pH of a buffer solution that contains 0.1 M NH3 (Ka = 1.8 x 10-5) and 0.05 M NH4Cl
pKa = 4.7447
pH = 4
Ra 222 undergoes beta decay to produce a daughter isotope. What is it?
22 Ac
89
What is the osmolarity of a solution that contains 54.9 g of Sr(OH)2 (FW = 122 g/mol) in 900 ml of solution?
1.50 Osm
A sample of vinegar is titrated with 0.100 M NaOH solution. It takes 35.00 mL of NaOH solution to reach the equivalence point. If the volume of vinegar is 25.00 mL, what is the concentration of acetic acid?
0.100 M NaOH = 0.100 N
Na = 0.140 N Vinegar
A 1.1 x 10-2 M HC2H3O2, acetic acid, solution has a [H+] of? (Ka = 1.8 x 10-5)
A) 1.1 x 10-2
B) 1.3 x 10-3
C) 4.4 x 10-4
D) 1.8 x 10-5
C) 4.4 x 10-4
What is the pH of a buffer solution that contains 0.1 M
H2CO3 (Ka = 4.5 x 10-7) and 0.1 M NaHCO3?
pKa = 6.3467
pH = 6
If you ingest 20.0 mg of 99Tc with a half-life of 6 hours, how many mg are left in your body after 18 hours?
18/6 = 3
20 -> 10 -> 5 -> 3.5
What is the normality of a solution of sulfuric acid that
contains 5.0 moles of H2SO4 in 2 L of solution?
5 N
A 25.00 mL sample of NaOH solution requires 35.56 mL of 0.200 M HCl to reach the endpoint of the titration. What is the molarity of the NaOH solution?
0.200M HCl = 0.200 N
Nb = 0.28448
0.28448 N = 0.284 M NaOH
Which one of the following 0.1 M solutions will have the LOWEST pH?
A) Hydrofluoric acid (Ka = 3.5 x 10-4)
B) Propanoic acid (Ka = 1.3 x 10-5)
C) Formic acid (Ka = 1.8 x 10-4)
D) Ascorbic acid (Ka = 7.9 x 10-5)
Most H+ ions = largest Ka
A) Hydrofluoric acid (Ka = 3.5 x 10-4)
A buffer is made by dissolving 0.5 mol of acetic acid (Ka = 3.3 x 10-2) and 0.9 mol of sodium acetate in 1 L of water. What is the pH of the buffer?
pKa = 1.4814
pH = 1.7
Radium 226 undergoes alpha decay followed by emission of a gamma ray. What is the following product of this decay?
226 Rn
86
What is the normality of 0.15 M Al(OH)3?
What is the normality of 0.5 M NaOH?
What is the normality of 0.25 M H2SO4?
What is the normality of 0.4 M HNO3?
N = 0.15 M ×3 =0 .45N
N = 0.5 M ×1 = 0.5N
N = 0.25 M ×2 = 0.5N
N = 0.4 M ×1 = 0.4N
A 25.00 mL sample of HCl solution requires 38.57 mL of 0.250 M NaOH to reach the endpoint of the titration. What is the molarity of the HCl solution?
0.250 M NaOH = 0.250 N
Na = 0.3857
0.3857 N = 0.386 M HCl
Calculate the [H+] and [OH-] of a solution with pH = 4.5
H+ = 3.2 x 10-5
OH- = 3.2 x 10-10
What is the pH of a buffer solution containing 5.0 x 10-2 M potassium nitrite and 8.0 x 10-2 M nitrous acid?
Ka = 4.6 x 10-4
pKa = 3.34
pH = 3.132
The half-life of technetium 99 is 6.0 hours. If 15 microcuries are injected into a patient, what is active after 24 hours, assuming no technetium is excreted?
24/6 = 4
15 -> 7.5 -> 3.75 -> 1.875 -> 0.9375