1. Which one of the following combinations would NOT form a precipitate in aqueous solution? A) Li(NO₃)₂ and NaOH B) AgNO₃ and KBr C) Zn(C₂H₃O₂)₂ and Na₂S D) Pb(NO₃)₂ and Na₂SO₄ E) All of the combinations will form precipitates.
1. Which one of the following combinations would NOT form a precipitate in aqueous solution? A) Li(NO₃)₂ and NaOH B) AgNO₃ and KBr C) Zn(C₂H₃O₂)₂ and Na₂S D) Pb(NO₃)₂ and Na₂SO₄ E) All of the combinations will form precipitates.
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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1. Which one of the following combinations would NOT form a precipitate in aqueous solution?
A) Li(NO₃)₂ and NaOH
B) AgNO₃ and KBr
C) Zn(C₂H₃O₂)₂ and Na₂S
D) Pb(NO₃)₂ and Na₂SO₄
E) All of the combinations will form precipitates.
2. What volume (in L) of 1.5 M Na₂CO₃ would be required to obtain 0.65 moles of Na⁺ ions?
3. What volume (in L) of 1.3 M FeBr₃ would be required to obtain 0.80 moles of Br⁻ ions?
4. To what volume (in mL) would you need to dilute 35.0 mL of a 1.30 M solution of KBr to make a 0.0600 M solution of KBr?
5. What volume, in L, of 1.1 M FeCl₃ would be required to obtain 0.70 moles of Cl⁻ ions?
A) 1.9 L
B) 0.21 L
C) 0.64 L
D) 0.77 L
6.If 0.25 L of a 6.0 M HNO₃ solution is diluted to 2.0 L, what is the molarity of the new solution?
7. What is the concentration of a solution made with 0.150 moles of KOH in 400.0 mL of solution?
8. How many moles of NaOH are there in 225.0 mL of 2.50 M NaOH?
9. How many moles of NaOH are there in 125.0 mL of 0.190 M NaOH?
10. How many moles of HCl are there in 35.0 mL of 0.350 M HCl?
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