How Many Milliliters of 0.400 M Naoh Are Required to Completely Neutralize 20.0 Ml of 0.200 M Hcl?
1
Aqueous Equilibria: Buffers & Titrations
AMHS AP Chemistry Name__________________
Multiple Choice questions
Common-Ion Effect
1) The pH of a solution that contains 0.818 M acetic acid (K
a
= 1.77x10
-5
) and 0.172 M sodium acetate is ___. A) 4.077 B) 5.434 C) 8.571 D) 8.370 E) 9.922 2) Calculate the pH of a solution prepared by dissolving 0.37 mol of formic acid (HCO
2
H) and 0.23 mol of sodium formate (NaCO
2
H) in water sufficient to yield 1.00 L of solution. The K
a
of formic acid is 1.77x10
4
. A) 2.1 B) 10.46 C) 3.55 D) 2.31 E) 3.95 3) Calculate the pH of a solution prepared by dissolving 0.25 mol of benzoic acid (C
7
H
5
O
2
H) and 0.15 of sodium benzoate (NaC
7
H
5
O
2
) in water sufficient to yield 1.00 L of solution. The K
a
of benzoic acid is 6.50x10
-5
. A) 4.41 B) 2.40 C) 3.97 D) 10.08 E) 4.19 4) Calculate the pH of a solution prepared by dissolving 0.15 mol of benzoic acid (HBz) and 0.30 mol of sodium benzoate in water sufficient to yield 1.00L of solution. The K
a
of benzoic acid is 6.50x10
-5
. A) 2.52 B) 3.89 C) 4.49 D) 10.16 E) 4.20 5) Calculate the pH of a solution prepared by dissolving 0.750 mol of NH
3
and 0.250 mol of NH
4
Cl in water sufficient to yield 1.00 L of solution. The K
b
of ammonia is 1.77x10
-5
. A) 5.22 B) 4.27 C) 9.73 D) 8.78 E) 0.89 6) The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH
3
NH
3
Cl) in 1.00L of 1.10M methylamine (CH
3
NH
2
) is __________. The K
b
for methylamine is 4.4 x 10
-4
. (Assume the final volume is 1.00 L.) A) 1.86 B) 2.66 C) 10.15 D) 11.14 E) 10.64
Buffers
7) What does a buffer do? a) Keeps the pH of a solution constant b) Keeps the salt concentration of a solution constant c) Keeps the cation concentration constant d) Keeps the anion concentration constant 8) What substances are present in a buffer? a) A weak base or acid and its salt b) A hydrolyzing salt only c) A weak base or acid only d) A salt only 9) The addition of hydrofluoric acid and __________ to water produces a buffer solution. A) HCl B) NaNO
3
C) NaF D) NaCl E) NaBr
5
40) A 25.0 mL sample of 0.723 M HClO
4
is titrated with a 0.273 M KOH solution. What is the [H
+
] (molarity) before any base is added? A) 0.439 B) 1.00 x 10
-7
C) 0.723 D) 2.81 X 10
-13
E) 0.273 41) A 25.0 mL sample of 0.723 M formic acid is titrated with a 0.273 M KOH solution. The K
a
of formic acid is 1.77 x 10
-4
. What is the pH of the acid before any base is added? A) 0.14 B ) 1.95 C) 3.89 D) 7.00 E) 8.19 42) A 25.0 mL sample of 0.22 M hydrazoic acid (HN
3
; K
a
= 2.6 x 10-5) is titrated with a 0.30 M KOH solution. What is the pH of the solution before any base is added? A) 2.62 B) 5.42 C) 7.00 D) 8.97 E) 11.22 43) The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is ______. A) 6.29 B) 7.00 C) 8.11 D) 5.78 E) 0.00 44) What is the pH of a solution resulting from 65 mL of 0.15 M HClO
3
titrated with 45 mL of 0.18 M NaOH? A) 0.65 B) 1.45 C) 1.82 D) 7.95 E) 8.21 45) A 25.0 mL sample of 0.22 M hydrazoic acid (HN
3
; K
a
= 2.6 x 10-5) is titrated with a 0.30 M KOH solution. What is the pH of the solution after 16.0 mL of base is added? A) 2.62 B) 5.42 C) 7.00 D) 8.97 E) 11.22 46) A 25.0 mL sample of 0.800 M HClO
4
is titrated with a 0.300 M KOH solution. The H
3
O
+
concentration after the addition of 10.0 mL of KOH is __________ M. A) 0.486 B) 1.00 x 10
-7
C) 0.723 D) 2.81 X 10
-13
E) 0.273 47) A 30.0 mL sample of 0.50 M HClO
4
is titrated with a 0.25 M KOH solution. The H
3
O
+
concentration after the addition of 5.0 mL of KOH is __________ M. A) 0.00125 B) 0.0138 C) 0.0150 D) 0.393 E) 0.439 48) A 30.0 mL sample of 0.72 M HClO
4
is titrated with a 0.27 M KOH solution. What is the H
3
O
+
concentration after the addition of 80.0 mL of KOH? A) 1.00 x 10
-7
B) 0.0216 C) 0.196 D) 0.27 E) 0.72 49) What volume (mL) of 0.5M HNO
3
is necessary to titrate 25 mL of 0.05M KOH solution to the endpoint? A) 2.5 B) 5.0 C) 10 D) 25 E) 50 50) What volume (mL) of 0.5M HNO
3
is necessary to titrate 25 mL of 0.05M Ca(OH)
2
solution to the endpoint? A) 2.5 B) 5.0 C) 10 D) 25 E) 50 51) How much 1.5 M NaOH is necessary to exactly neutralize 20.0 mL of 2.5 M H
3
PO
4
? A) 20 B) 33 C) 40 D) 60 E) 100 52) A 25.0 mL sample of an HCl solution is titrated with a 0.15 M NaOH solution. The equivalence point is reached with 75.0 mL of base. The concentration of HCl is _________ M. A) 11.7 B) 0.00214 C) 0.450 D) 0.267 E) 0.139 53) A 50.0 mL sample of an aqueous H
2
SO
4
solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached with 100 mL of NaOH solution. The concentration of H
2
SO
4
is __________ M. A) 0.050 B) 0.100 C) 0.150 D) 0.200 E) 0.400
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18) The point at which the moles of the added strong base are equal to the moles of the weak acid initially present 19) The point at which the pH is closest to that of the strong base being added 20) The point at which the concentrations of the weak acid and its conjugate base are approximately equal The graph below shows the titration curve that results when 100 ml of 0.25M acetic acid is titrated with 0.10M NaOH. Answer questions 27-29 is based on the curve below.
How Many Milliliters of 0.400 M Naoh Are Required to Completely Neutralize 20.0 Ml of 0.200 M Hcl?
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