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4.44 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Potassium carbonate + barium hydroxide (b) Aluminum nitrate + sodium phosphate

4.44 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Potassium carbonate + barium hydroxide (b) Aluminum nitrate + sodium phosphate

Chemistry
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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question 44 please
4.42 Complete the following precipitation reactions with bal- anced molecular, total ionic, and net ionic equations: (a) CaCl,(aq) + CS3PO4(aq) – (b) Na,S(aq) + ZNSO«(aq) 4.43 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium nitrate + copper(II) sulfate (b) Ammonium bromide + silver nitrate 4.44 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Potassium carbonate + barium hydroxide (b) Aluminum nitrate + sodium phosphate 45 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations. (a) Potassium chloride + iron(III) nitrate (b) Ammonium sulfate + barium chloride 4.46 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium sulfide + nickel(II) sulfate (b) Lead(II) nitrate + potassium bromide 4.47 If 38.5 mL of lead(II) nitrate solution reacts completely with excess sodium iodide solution to yield 0.628 g of precipitate, what is the molarity of lead(II) ion in the original solution? 4.48 If 25.0 mL of silver nitrate solution reacts with excess potas- sium chloride solution to yield 0.842 g of precipitate, what is the molarity of silver ion in the original solution?
Transcribed Image Text:4.42 Complete the following precipitation reactions with bal- anced molecular, total ionic, and net ionic equations: (a) CaCl,(aq) + CS3PO4(aq) – (b) Na,S(aq) + ZNSO«(aq) 4.43 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium nitrate + copper(II) sulfate (b) Ammonium bromide + silver nitrate 4.44 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Potassium carbonate + barium hydroxide (b) Aluminum nitrate + sodium phosphate 45 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations. (a) Potassium chloride + iron(III) nitrate (b) Ammonium sulfate + barium chloride 4.46 When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium sulfide + nickel(II) sulfate (b) Lead(II) nitrate + potassium bromide 4.47 If 38.5 mL of lead(II) nitrate solution reacts completely with excess sodium iodide solution to yield 0.628 g of precipitate, what is the molarity of lead(II) ion in the original solution? 4.48 If 25.0 mL of silver nitrate solution reacts with excess potas- sium chloride solution to yield 0.842 g of precipitate, what is the molarity of silver ion in the original solution?
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