questions Pre-Lab Questions: Complete the following equations, writing balanced chemical equation, balanced ionic equation, and net ionic equation for each equation. Note that precipitates are insoluble and are followed by (s). Species in solution are followed by (aq). Note the list of insoluble salts. These are precipitates. Note the list of polyatomic ions. These atoms always stay together as a unit. 1. Ba(NO3)2 (aq) + K₂SO4 (aq) 2. AgNO3(aq) + NaBr (aq)

questions Pre-Lab Questions: Complete the following equations, writing balanced chemical equation, balanced ionic equation, and net ionic equation for each equation. Note that precipitates are insoluble and are followed by (s). Species in solution are followed by (aq). Note the list of insoluble salts. These are precipitates. Note the list of polyatomic ions. These atoms always stay together as a unit. 1. Ba(NO3)2 (aq) + K₂SO4 (aq) 2. AgNO3(aq) + NaBr (aq)

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 108A: Apply Students conducted a lab to investigate limiting and excess reactants. The students added...

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Show all work please.. answer both questions I. Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide. Below is an unbalanced net ionic equation of the reaction: Pb2+ (aq) + I-1 (aq) → PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 45.0 g of Pb(NO3)2 (aq) to completely precipitate the lead? II. Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.86 g of magnesium ribbon burns with 155ml of oxygen at 1.0 atm and 275 K , a bright, white light and a white, powdery product is formed, magnesium oxide. How many grams of excess reactant remain?
Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.
Based on the general solubility rules given in Table 7.1, propose five combinations of aqueous ionic reagents that likely would form a precipitate when they are mixed. Write the balanced full molecular equation and the balanced net ionic equation for each of your choices.
This series demonstrates a drop-by-drop addition of 0.5 M potassium chromate solution (? ??? ) to 0.5 M barium chloride solution (???? ). What observations indicate that a chemical reaction has occurred Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. Write the complete ionic equation for this reaction. Write the net ionic equation for this reaction. What is the precipitate?
A chemist wishes to precipitate iron ions out of a solution of iron (III) nitrate. Provide complete balanced equation, total ionic equation and a net ionic equation that describes how this can be done. Complete Balanced Chemical Equation (2 marks) ________________________________________ ? __________________________________________ Total Ionic Equation (2 marks) ________________________________________ ? __________________________________________ Net Ionic Equation (1 mark) ________________________________________ ? __________________________________________
Write the objectives IN YOUR OWN WORDS: Obiective:To predict the products of some displacement reactions and write net ionic equations.Note-the (aq) has been eliminated from all equations below while (s), (I) and (g) have been used to represent phases. When you write chemical reactions in your lab reports youmust show all phases including (aq).
For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together.Note: Leave the answer blank if no precipitate will form. (Express your answer as a chemical formula.)
This series demonstrates a drop-by-drop addition of 0.5 M barium chloride solution (???? ) to 0.5 M sodium carbonate solution (?? ?? ) 1. What observations indicate that a chemical reaction has occurred? 2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?
Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct? Both NaCl and CuS precipitate from solution. No reaction will occur. CuS will precipitate from solution. NaCl will precipitate from solution. Cu2S will precipitate from solution. Why would number 3 be correct and not number 1? This is where I need help-I assumed whenever a solid is produced as products in a reaction, then both (in this case) precipitate. Please clarify, thanks.
B.This series demonstrates the addition of 0.5 M potassium chromate solution (? ??? ) drop-by-drop to 0.25 M iron(III) chloride solution (???? ) What observations indicate that a chemical reaction has occurred. 2.Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3.Write the complete ionic equation for this reaction. 4.Write the net ionic equation for this reaction. 5.What is the precipitate?
This is my second time submitting this question, please help write out equations even if it is just for the 1st sample so I can apply the values for 2 and 3. Please help me understand the equations for this table. How do I calculate the moles of NaOH and acetic acid? How do I calculate the mass of acetic acid? How do I calculate the molarity and % mass of acetic acid. Thanks! moles of NaOH = 1.0 M x 6.2 mL x 1 L/1,000mL = 0.0062 moles NaOH - from lab manual the experimental data is in the picture with blue answers, the second part of the table I need help with.
Analytical chemists are trying to determine the identity of an unknown solution. They have narrowed it down to two possibilities, silver nitrate or potassium nitrate. You have been assigned the task of determining how to finish testing the solution to reveal its identity. Use your knowledge of double displacement reactions, and the solubility table to come up with a laboratory procedure which will identify the unknown solution. Be sure to include a purpose, hypothesis, materials and procedure.