1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? a.4.2 x 10 M b. 1.6 x 105 M c. 3.6 x 10-12 M d. 6.3 x 10-10 M 2 the pH of a 0.50 M solution of NaNO₂. Ka for HNO₂ is 4× 10-5 a 12.1 b. 5.48 c. 1.82 e. 2.0 x 10- M c. 8.90 d 8.52 3- What was the pH of the solution that result from titration of 25.0 ml of 0.5 M solution of weak base (Kb - 9.74×10) wi 30 ml of 0.1 M hydrochloric acid, HCL.? a. 5.10 b. 4.92 d. 9.1 e.7.00 4-Which of the following combinations cannot produce a buffer solution? a. HNO₂ and NaNO₂ b. HCN and NaCN c. HCIO4 and NaCIO4 d. NH3 and (NH4)2SO4 d. 5.5 e. 9.5 e. NH3 and NH4Br 5- What is the pH at the equivalence point in the titration of 100.0 mL of 0.20 M ammonia (NH3) with 0.10 M hydrochloric acid (HCI)? Kb for NH31.8x 10-5 a. 4.6 b. 5.2 c. 7.0 e. 4.9 6- If 10.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in ppm is: [M.wt. of HNO3= 63 g/mol] e. 25.77 x10³ ppm b.14.70 x10³ ppm c. 6.30 × 10¹ ppm a. 9.45×10³ ppm d. 18.77 x 10¹ ppm
1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? a.4.2 x 10 M b. 1.6 x 105 M c. 3.6 x 10-12 M d. 6.3 x 10-10 M 2 the pH of a 0.50 M solution of NaNO₂. Ka for HNO₂ is 4× 10-5 a 12.1 b. 5.48 c. 1.82 e. 2.0 x 10- M c. 8.90 d 8.52 3- What was the pH of the solution that result from titration of 25.0 ml of 0.5 M solution of weak base (Kb - 9.74×10) wi 30 ml of 0.1 M hydrochloric acid, HCL.? a. 5.10 b. 4.92 d. 9.1 e.7.00 4-Which of the following combinations cannot produce a buffer solution? a. HNO₂ and NaNO₂ b. HCN and NaCN c. HCIO4 and NaCIO4 d. NH3 and (NH4)2SO4 d. 5.5 e. 9.5 e. NH3 and NH4Br 5- What is the pH at the equivalence point in the titration of 100.0 mL of 0.20 M ammonia (NH3) with 0.10 M hydrochloric acid (HCI)? Kb for NH31.8x 10-5 a. 4.6 b. 5.2 c. 7.0 e. 4.9 6- If 10.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in ppm is: [M.wt. of HNO3= 63 g/mol] e. 25.77 x10³ ppm b.14.70 x10³ ppm c. 6.30 × 10¹ ppm a. 9.45×10³ ppm d. 18.77 x 10¹ ppm
Chapter14: Acids And Bases
Section: Chapter Questions
Problem 104E: Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution having...
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![1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution?
a.4.2 x 10 M b. 1.6 x 105 M
c. 3.6 x 10-12 M
d. 6.3 x 10-10 M
2 the pH of a 0.50 M solution of NaNO₂. Ka for HNO₂ is 4×10-5
a 12.1
b. 5.48
c. 1.82
c. 8.90
d 8.52
3- What was the pH of the solution that result from titration of 25.0 ml of 0.5 M solution of weak base (Kb - 9.74×10) wi
30 ml of 0.1 M hydrochloric acid, HCI.?
a. 5.10
b. 4.92
d. 9.1
4-Which of the following combinations cannot produce a buffer solution?
a. HNO₂ and NaNO₂ b. HCN and NaCN c. HCIO4 and NaClO4 d. NH3 and (NH4)2SO4
e. 2.0 x 10-8 M
d. 5.5
e. NH3 and NH4Br
5- What is the pH at the equivalence point in the titration of 100.0 mL of 0.20 M ammonia (NH3) with 0.10 M
hydrochloric acid (HCI)? Kb for NH31.8x 10-5
a. 4.6
b. 5.2
c. 7.0
e. 4.9
e.7.00
9. what will happened to the pH of buffer system when it diluted
a. ApH=0
b. pH will increased c. pH will decrease
6- If 10.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in
ppm is: [M.wt. of HNO3= 63 g/mol]
e. 25.77 x 10³ ppm
a. 9.45×10³ ppm
b.14.70 x10³ ppm
c. 6.30 × 10³ ppm
d. 18.77 × 10¹ ppm
7. A 0.6745-gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the
molarity of the KOH solution? (Molecular weight of KHP = 204 g/mol. KHP has one acidic hydrogen.)
a. 0.158 M
c. 0.139 M
b. 0.099 M
d. 0.079 M
e. 0.061 M
8. Which of the following combinations would give a pH =7.00 at the "equivalence point" (when equal moles of each have
been added)?
a. HCI + KF
b. HCN + NaOH
c. HF + HCI
d. HCI + KOH
13. The molar analytical concentration of NO
were added to 20.0 ml of 0. 82 M Fe (NO3)2
a.1.09M
b. 2.53 M
d. pH >7 e.
pH = 7
10. the pH for Acidic buffer system with highest capacity if the Ka for the weak Acid 1.8 104 is
a. 4.3
b.5.3
c.3.77
d.6.8
e. 8.3
e. 9.5
c.0.73 M
11.The ppm concentration of Cl-ion in 100 ml mixture solution of 0.01 M CaCl2 and 0.1 M HCI is (MW of Cl =
35.45 g/mol and for Cl =35.45 g/mol ) is :-
b. 4254 ppm
c. 355 ppm
d. 9150ppm
a. 243 ppm
e. 850ppm
from the primary-
12. The mass of AgNO3(s) needed to prepare 1.000 L of 0.0500 M AgNO3 (169.87 g/mol) solution
standard-grade solid is
a. 18.548g
b. 16.987 g
c. 16.139 g
d. 9.843g
e. 10.36 g
ions in the solution produced when 25.0 ml of Distilled water
d. 0.11 M
14. Standard solution of EDTA (0.100 M) is being used to titrate 25.00 ml of (0.0100) M of Zn²+ solution (buffered
at pH =10, 04-0.36 and kMY = 3.2x10¹6) the pZn after the addition of 25 ml EDTA solution is (at equivalent
point)
a. 8.68
b. 9.03
d. 9.79
c. 3.76
e. 0.13 M
e. 6.89](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ef3182-b77b-4d5e-aa39-bd37ce4fcd02%2Fec727acb-c045-4781-ae8c-f55a0015705b%2F4lk8128_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution?
a.4.2 x 10 M b. 1.6 x 105 M
c. 3.6 x 10-12 M
d. 6.3 x 10-10 M
2 the pH of a 0.50 M solution of NaNO₂. Ka for HNO₂ is 4×10-5
a 12.1
b. 5.48
c. 1.82
c. 8.90
d 8.52
3- What was the pH of the solution that result from titration of 25.0 ml of 0.5 M solution of weak base (Kb - 9.74×10) wi
30 ml of 0.1 M hydrochloric acid, HCI.?
a. 5.10
b. 4.92
d. 9.1
4-Which of the following combinations cannot produce a buffer solution?
a. HNO₂ and NaNO₂ b. HCN and NaCN c. HCIO4 and NaClO4 d. NH3 and (NH4)2SO4
e. 2.0 x 10-8 M
d. 5.5
e. NH3 and NH4Br
5- What is the pH at the equivalence point in the titration of 100.0 mL of 0.20 M ammonia (NH3) with 0.10 M
hydrochloric acid (HCI)? Kb for NH31.8x 10-5
a. 4.6
b. 5.2
c. 7.0
e. 4.9
e.7.00
9. what will happened to the pH of buffer system when it diluted
a. ApH=0
b. pH will increased c. pH will decrease
6- If 10.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in
ppm is: [M.wt. of HNO3= 63 g/mol]
e. 25.77 x 10³ ppm
a. 9.45×10³ ppm
b.14.70 x10³ ppm
c. 6.30 × 10³ ppm
d. 18.77 × 10¹ ppm
7. A 0.6745-gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the
molarity of the KOH solution? (Molecular weight of KHP = 204 g/mol. KHP has one acidic hydrogen.)
a. 0.158 M
c. 0.139 M
b. 0.099 M
d. 0.079 M
e. 0.061 M
8. Which of the following combinations would give a pH =7.00 at the "equivalence point" (when equal moles of each have
been added)?
a. HCI + KF
b. HCN + NaOH
c. HF + HCI
d. HCI + KOH
13. The molar analytical concentration of NO
were added to 20.0 ml of 0. 82 M Fe (NO3)2
a.1.09M
b. 2.53 M
d. pH >7 e.
pH = 7
10. the pH for Acidic buffer system with highest capacity if the Ka for the weak Acid 1.8 104 is
a. 4.3
b.5.3
c.3.77
d.6.8
e. 8.3
e. 9.5
c.0.73 M
11.The ppm concentration of Cl-ion in 100 ml mixture solution of 0.01 M CaCl2 and 0.1 M HCI is (MW of Cl =
35.45 g/mol and for Cl =35.45 g/mol ) is :-
b. 4254 ppm
c. 355 ppm
d. 9150ppm
a. 243 ppm
e. 850ppm
from the primary-
12. The mass of AgNO3(s) needed to prepare 1.000 L of 0.0500 M AgNO3 (169.87 g/mol) solution
standard-grade solid is
a. 18.548g
b. 16.987 g
c. 16.139 g
d. 9.843g
e. 10.36 g
ions in the solution produced when 25.0 ml of Distilled water
d. 0.11 M
14. Standard solution of EDTA (0.100 M) is being used to titrate 25.00 ml of (0.0100) M of Zn²+ solution (buffered
at pH =10, 04-0.36 and kMY = 3.2x10¹6) the pZn after the addition of 25 ml EDTA solution is (at equivalent
point)
a. 8.68
b. 9.03
d. 9.79
c. 3.76
e. 0.13 M
e. 6.89
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