Q 1 please Choose the best answer.Q1. What mass of K₂CO3 is needed to prepare 200 mL of a solution having a potassium ion concentration c0.150 M?A. 2.07B. 4.15 gC. 10.4 gD. 1.49gQ2. A 47.27 g of Ca(OH)2 is dissolved in water to make 2.5 L of solution. How many mL of this solution mube diluted with water to make 1.0 L of 0.10 M Ca(OH)₂?B. 658 mLD. 3.34 mlA. 392.1 mLQ3. Arrange the following in order of increasing first ionization energy.A. Ca

Answered: Image /qna-images/answer/1b44476f-cbd8-439f-947d-10f2c732f9c7.jpg

Choose the best answer. Q1. What mass of K₂CO3 is needed to prepare 200 mL of a solution having a potassium ion concentration c 0.150 M? C. 10.4 g D. 1.49 g A. 2.07 B. 4.15 g Q2. A 47.27 g of Ca(OH) is dissolved in water to make [ C

Choose the best answer. Q1. What mass of K₂CO3 is needed to prepare 200 mL of a solution having a potassium ion concentration c 0.150 M? C. 10.4 g D. 1.49 g A. 2.07 B. 4.15 g Q2. A 47.27 g of Ca(OH) is dissolved in water to make [ C

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 16QAP

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Q 1 please

Choose the best answer.
Q1. What mass of K₂CO3 is needed to prepare 200 mL of a solution having a potassium ion concentration c
0.150 M?
A. 2.07
B. 4.15 g
C. 10.4 g
D. 1.49g
Q2. A 47.27 g of Ca(OH)2 is dissolved in water to make 2.5 L of solution. How many mL of this solution mu
be diluted with water to make 1.0 L of 0.10 M Ca(OH)₂?
B. 658 mL
D. 3.34 ml
A. 392.1 mL
Q3. Arrange the following in order of increasing first ionization energy.
A. Ca<Ba<P<S
B. Ca<Ba<S<P
C. Ba<Ca<S<P
D. Ba<Ca<P<S
Which pair of ions will not form a precipitate (soluble) when their solutions are mixed?
A. Ca²+, SO4²-
B. Ag+, NO3
C. AP¹+, PO¹
D. Pb, OH
5. Calculate the molar mass of the acid when 0.425 g sample of H₂X acid is completely neutralized with
34.6 mL of 0.151 M NaOH.
A. 162.8 g/mol
B. 246.8 g/mol
C) 173 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-4 principal energy level.
B. 1.010 10³ nm
A. 4.450 x 10-22 nm
C. 9.180 10-20 nm
D.2.166 10's
C. 18.5 mL
Q7. The electron configuration for the sulfur ion (S²) is?
A. 1s 2s 2p 3s 3p²
B. 1s²2s²2p 3s²3p
(n, 1, m, m.) for an electron in a 5f orbital
B. (5, 2, 3, 1/2)
Q8. The correct set of quantum numbers
A. (4, 2, 1, 1/2)
C. (5, 2, 0, 1/2)
Q9. Which one of the following is the correct order for atomic radius? (Smallest to largest)
B. F<Ca<P
A. Ca<P <F
C. Ca < F<P
incorrectly?
Q10. Which of the following is paired
A. C6H12O6 nonelectrolyte
C. Na(OH) strong electrolyte
C. [Ne]3s 3p 4s
Q11. Which of the following frequencies corresponds to light with the longest wavelength?
B. 4.12 x 10³ s¹
A..3.00 × 10¹3 ¹
C. 8.50 100 ¹
A. 1, 1, 1
B. HNO, weak electrolyte
D. HCI strong electrolyte
D. [Ne]3s 3p
D. (5, 3,-1,-1/2)
D. F<P <Ca
Q12. The spectator ions in the following reaction are? Pb(NO3)2+ 2NaC1→ PbCl₂ + 2NaNO,
B. Pb2+, NO3-
A. Na²+, NO3-
C. NO, CH-
D. 9.12 - 102
D. Pb, C1-
Q13. When the following equation is balanced in acidic solution, the coefficients for Cr₂O, I and Cr
respectively are?
r
Cr₂O72 (aq) +1¹(q) →→ Cr+ (aq) + 10) (q)
C. 1, 1,2
B. 1, 1,2
D. 2, 1, 1

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