6. A solution of potassium sulfide reacts with a solution of lead (II) nitrate to produce aqueous potassium nitrate and solid lead (II) sulfide. 7. Iron(III) oxide reacts with carbon to produce iron and carbon dioxide. 8. A solution of lithium phosphate reacts with a solution of magnesium sulfate to produce magnesium phosphate and aqueous lithium sulfate.

6. A solution of potassium sulfide reacts with a solution of lead (II) nitrate to produce aqueous potassium nitrate and solid lead (II) sulfide. 7. Iron(III) oxide reacts with carbon to produce iron and carbon dioxide. 8. A solution of lithium phosphate reacts with a solution of magnesium sulfate to produce magnesium phosphate and aqueous lithium sulfate.

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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31) You have 500 mL of a 1.25 M Pb(NO3)2 solution. How much solid sodium chloride do you need to add to react all of the lead? ? (HINT: react lead (II) nitrate with sodium chloride) а. 54.6 g b. 44.3 g с. 146 g d. 73.1 g
. For each reaction scenario below, predict the products of the reaction, and write a complete balanced chemical equation. If you predict that no reaction will occur, write the reactants, then write NR after the arrow. а. Water undergoes decomposition by electrolysis. b. A table salt (sodium chloride) solution is poured into an aluminum can. с. A copper (II) nitrate solution is combined with an ammonium chromate solution.
3. A solution contains silver nitrate, lead (II) nitrate, and calcium nitrate. What reagent could be added to this solution that would separate the calcium nitrate from the other three compounds? Write the formula of the resulting precipitates after the addition of this reagent.
Classify each chemical reaction: Reaction Cl₂(g) + 2KI (aq) → 2KCl(aq) + 1₂ (s) H₂SO₂ (aq) H₂O(l) + SO₂ (g) PbCl₂ (aq) + FeSO (aq) → FeCl₂ (aq) + PbSO₂ (s) Mg(s) + F₂ (g) → MgF₂ (s) Type choose one choose one choose one choose one X Ś
A student weighs out 4.16 g of magnesium chloride and adds enough water to make 125.0 mL of solution. The student then weighs out 8.82 g of sodium phosphate and adds enough water to make 250.0 mL of solution. 25.0 mL of the magnesium chloride solution is combined with 25.0 mL of the sodium phosphate solution. a. Write a balanced equation for the reaction that occurs (remember to include phases). b. If a precipitate forms, write the name of the precipitate and calculate the theoretical yield for the precipitate. If no precipitate forms, calculate the limiting reactant. c. If the temperature of the solution decreases, is this reaction exothermic or endothermic?
13. A chemistry student offers a possible improvement to this lab. Since one goal of this lab is to determine the mass of the precipitate produced, wouldn't it be possible to measure the mass of an empty beaker, mix the solutions, and boil off the water until it is entirely evaporated, leaving only solid behind? Then the beaker with the precipitate could be weighed, and the difference between this mass and that of the empty beaker would be the mass of the precipitate. This would eliminate the need for the filtration step. Explain why this is a poor suggestion. Remember to check your reasoning on this question and all other questions with your instructor.
3. For each reaction below, (f) write a balanced reaction equation, including proper state symbols, and (ii) name the type of reaction that occurs. Note: More than one type of reaction may apply to the same reaction equation. a. zinc metal reacts with aqueous copper(II) sulfate to form copper metal and aqueous zinc(II) sulfate b. aqueous sodium sulfide and aqueous lead(II) acetate form aqueous sodium acetate and solid lead(II) sulfide C. solid sodium bicarbonate is heated to form carbon dioxide gas, liquid water, and solid sodium carbonate d. solid magnesium and diatomic nitrogen gas react to form solid magnesium nitride e. sulfuric acid and aqueous potassium hydroxide react to form aqueous potassium sulfate and liqud water
6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)
What happens when potassium iodide is added to a solution of lead nitrate? Potassium nitrate precipitates out. Lead iodide precipitates out. Gaseous lead iodide forms. Nothing - there is no reaction between potassium iodide and lead nitrate.
Two experiments are performed as described below:i. Aluminum foil (Al) is placed into a solution of nickel(II) chloride.ii. A piece of gold metal (Au) was added to an aqueous solution of Zn(NO3)2.In which experiment does a reaction occur, and in which experiment does a reaction not occur?
4. Write an equation for the reaction of aqueous sulfuric acid and aqueous barium hydroxide. Indicate the physical states of all reactants and products. 5. Write an equation for the reaction of aqueous phosphoric acid and magnesium metal. Indicate the physical states of all reactants and products. 6. Write an equation for the reaction of aqueous phosphoric acid and aqueous sodium bicarbonate. Indicate the physical states of all reactants and products.
Write the formulas of the reactants and products - including the symbols for the state - (s), (l), (g), (aq) - then balance the equations. Use the WIRIS editor to appropriately represent formulas and symbols.