Q5. Calculate the molar mass of the acid when 0.625 g sample of H₂X acid is completely neutralized with 45.2 ml. of 0.106 M NaOH. A. 246.8 g/mol B. 505.2 g/mol C. 260.9 g/mol D. 82.9 g/mol
Q5. Calculate the molar mass of the acid when 0.625 g sample of H₂X acid is completely neutralized with 45.2 ml. of 0.106 M NaOH. A. 246.8 g/mol B. 505.2 g/mol C. 260.9 g/mol D. 82.9 g/mol
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 98AP
Related questions
Question
Q 5 please
![Q1. What mass of Li3PO4 is needed to prepare 500 ml. of a solution having a lithium ion concentration of
0.175 M?
A. 6.75 g
B. 10.1 g
C. 3.36 g
D. 19.3 g
Q2. A 47.27 g of Ca(OH)2 is dissolved in water to make 1.0 liters of solution. How many mL of this solution
must be diluted with water to make 1.0 L of 0.10 M Ca(OH)2?
A. 538.4 ml.
B. 658 ml.
Q3. Arrange the following in order of increasing first ionization energy
A. Rb<Ca<S<P
C. Rb< Ca<P<S
C. 156.7 ml.
Q4. Which pair of ions will form a precipitate (insoluble) when their solutions are mixed?
A. AP³+, NO,¹
B. K¹, S²
C. Na, PO¹
Q10. Which of the following is paired correctly?
A. H₂SO4 nonelectrolyte
C. BaCl₂ weak electrolyte
B. Rb<P<Ca<S
D. P<S<Ca<Rb
D. Ca²+, CO₂-²
Q5. Calculate the molar mass of the acid when 0.625 g sample of H₂X acid is completely neutralized with 45.2
ml. of 0.106 M NaOH.
A. 246.8 g/mol
B. 505.2 g/mol
C. 260.9 g/mol
D. 82.9 g/mol
Q6. Calculate of the light emitted by a H atom if an electron falls from n=7 to n=2 principal energy
level.
A. 3.97 × 10² nm
B. 101mm
C. 445nm
D. 2.16 x 10 m
Q7. The electron configuration for the iodine ion (1¹) is?
A. [Kr]5s²4d¹05p
B. [Xe]6s²
D. [Kr]4s3d¹04p
D. (6. 2, -3,-1/2)
C) 1s 2s 2p 3s 3p 4s²
Q8. The correct set of quantum numbers (n, 1, mi, m.) for an electron in a 6f orbital is?
A. (6, 2, 1, 1/2)
B. (6, 3, -2, -1/2)
C. (5, 2, 2, 1/2)
Q9. Which one of the following is the correct order for atomic radius? (largest to smallest)
A. K> F > P
B.K>P>F
C.F> P> K
A. 14, 2, 3
D. 3.34 mL
Q11. Which of the following frequencies corresponds to light with the shortest wavelength?
A. 3.00 × 10¹3 S-1
B. 4.12 x 10³ s
X
C. 8.50 × 1020 S-¹
Q12. What are the reacting ions in the following reaction?
Pb(NO3)2 + 2NaCl-PbCl₂ + 2NaNO3
B. Pb²+, C1¹
B. 7, 2, 3
B. HNO, weak electrolyte
D. HCI strong electrolyte
C. Pb². Na¹+
D. P> K>F
Cr₂O7² (aq) +1¹(aq) → Cr+³(aq) + 12 (aq)
1
C. 6, 2, 2
A. Na¹*, NO,¹-
D. Pb²+, NO3¹
Q13. When the following equation is balanced in acidic solution the coefficients for, H¹, Cr3, and Iz
respectively are?
D.9.12 × 1021 1
D. 14, 3, 2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F73756e6a-601d-4e3a-a6d7-35b2b5f0e6cb%2F7358d5c9-2359-4fd3-9d40-02029ad7c530%2Fg7i69ab_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Q1. What mass of Li3PO4 is needed to prepare 500 ml. of a solution having a lithium ion concentration of
0.175 M?
A. 6.75 g
B. 10.1 g
C. 3.36 g
D. 19.3 g
Q2. A 47.27 g of Ca(OH)2 is dissolved in water to make 1.0 liters of solution. How many mL of this solution
must be diluted with water to make 1.0 L of 0.10 M Ca(OH)2?
A. 538.4 ml.
B. 658 ml.
Q3. Arrange the following in order of increasing first ionization energy
A. Rb<Ca<S<P
C. Rb< Ca<P<S
C. 156.7 ml.
Q4. Which pair of ions will form a precipitate (insoluble) when their solutions are mixed?
A. AP³+, NO,¹
B. K¹, S²
C. Na, PO¹
Q10. Which of the following is paired correctly?
A. H₂SO4 nonelectrolyte
C. BaCl₂ weak electrolyte
B. Rb<P<Ca<S
D. P<S<Ca<Rb
D. Ca²+, CO₂-²
Q5. Calculate the molar mass of the acid when 0.625 g sample of H₂X acid is completely neutralized with 45.2
ml. of 0.106 M NaOH.
A. 246.8 g/mol
B. 505.2 g/mol
C. 260.9 g/mol
D. 82.9 g/mol
Q6. Calculate of the light emitted by a H atom if an electron falls from n=7 to n=2 principal energy
level.
A. 3.97 × 10² nm
B. 101mm
C. 445nm
D. 2.16 x 10 m
Q7. The electron configuration for the iodine ion (1¹) is?
A. [Kr]5s²4d¹05p
B. [Xe]6s²
D. [Kr]4s3d¹04p
D. (6. 2, -3,-1/2)
C) 1s 2s 2p 3s 3p 4s²
Q8. The correct set of quantum numbers (n, 1, mi, m.) for an electron in a 6f orbital is?
A. (6, 2, 1, 1/2)
B. (6, 3, -2, -1/2)
C. (5, 2, 2, 1/2)
Q9. Which one of the following is the correct order for atomic radius? (largest to smallest)
A. K> F > P
B.K>P>F
C.F> P> K
A. 14, 2, 3
D. 3.34 mL
Q11. Which of the following frequencies corresponds to light with the shortest wavelength?
A. 3.00 × 10¹3 S-1
B. 4.12 x 10³ s
X
C. 8.50 × 1020 S-¹
Q12. What are the reacting ions in the following reaction?
Pb(NO3)2 + 2NaCl-PbCl₂ + 2NaNO3
B. Pb²+, C1¹
B. 7, 2, 3
B. HNO, weak electrolyte
D. HCI strong electrolyte
C. Pb². Na¹+
D. P> K>F
Cr₂O7² (aq) +1¹(aq) → Cr+³(aq) + 12 (aq)
1
C. 6, 2, 2
A. Na¹*, NO,¹-
D. Pb²+, NO3¹
Q13. When the following equation is balanced in acidic solution the coefficients for, H¹, Cr3, and Iz
respectively are?
D.9.12 × 1021 1
D. 14, 3, 2
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