11. The ppm concentration of Cl-ion in 100 ml mixture solution of 0.01 M CaCl₂ and 0.1 M HCl is (MW of Cl = 35.45 g/mol and for Cl=35.45 g/mol ) is :- c. 355 ppm d. 9150ppm e. 850ppm b. 4254 ppm a. 243 ppm 12. The mass of AgNO(s) needed to prepare 1.0001 of 0.0500 MANO (160.97
11. The ppm concentration of Cl-ion in 100 ml mixture solution of 0.01 M CaCl₂ and 0.1 M HCl is (MW of Cl = 35.45 g/mol and for Cl=35.45 g/mol ) is :- c. 355 ppm d. 9150ppm e. 850ppm b. 4254 ppm a. 243 ppm 12. The mass of AgNO(s) needed to prepare 1.0001 of 0.0500 MANO (160.97
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Q 11 please
![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%2F94c372e6-c2ea-4239-94ae-94695bbf7f13%2Fzc1zd5_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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