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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Watch this video of a double displacement experiment:
https://www.youtube.com/watch?v=mph8Hq_75vU
-
Write the balanced
chemical reactions , includingstate of the matter -
What is the precipitate that forms, and which color is it?
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- In the laboratory you are given the task of separating Ba2+ and Pb²+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. Na₂CO3 2. 3. NaOH Na₂Sarrow_forwardFor the following reaction, do the following: 1. Write the correct formulas for the products, assuming a metathesis/exchange/double replacement/double displacement reaction is occurring 2. Using a solubility table, predict whether the reaction would produce a precipitate and fill in the phase subscripts for each product 3. Balance the equation, giving the correct balanced molecular equation 4. Write the total ionic equation 5. Write the net ionic equation FeCl3 (aq) + K2S (aq) →arrow_forwardIn the laboratory, you are given the task of separating Ba2+ and Co2+ ions in an aqueous solution. For each reagent listed below, indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES HCl Na2S K2CO3arrow_forward
- 12arrow_forwardFor each of the following balanced chemical reactions, identify the type of chemical reaction. If you need to review this concept, select here. Choose... 2 Na(s) + Cl,(g) 2 NaC((s) simple decomposition V simple formation complete combustion 4 PCI(g) + P,(s) + 10 Cl,(g) double replacement 3Cuso,(aq) + 2Fe(s) → Fe,(so,),(aq) + 3Cu single replacement AGNO,(aq) + NaCI(aq) → AgCl(s) + NaNO,(aq) double replacement + 2 C,H2o(g) + 13 02(g) - 8 CO,(g) + 10 H,0(g) complete combustion +arrow_forward[Review Topics] [References] Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. The following molecular equation represents the reaction that occurs when aqueous solutions of silver(I) nitrate and iron(III) iodide are combined. 3AGNO3 (aq) + Fel3 (aq) →3AgI (s) + Fe(NO3)3 (aq) Write the balanced net ionic equation for the reaction. + + Submit Answer Retry Entire Group 4 more group attempts remaining Previous Next Save and Exi Email Instructorarrow_forward
- In the laboratory you are given the task of separating Ca2+ and Fe2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the lons, give the formula of the precipitate. If it cannot, type "No" Y or N 1. 12. 3 Reagent Formula of Precipitate if YES ка K₂SO4 Na COarrow_forwardNormally, the amount of silver nitrate required to precipitate all of the chloride in the sample is found by a trial and error process. However, to speed up the experiment, assume a sample mass of 0.1431 g, and that sample contains approximately 55.0% chloride ion by mass. From these assumptions, calculate the volume of 0.100 M AgNO3(aq) that needs to be added to precipitate all of the chloride ion. Please answer in mL. (Note: You are calculating the exact amount required and not adding 5mL in excess. In the experiment, you'd be adding an additional 5mL in excess since the chloride value of the salt may exceed 55%. Pay attention to the sig. figs. in your calculation; keep three sig. figs. in the answer.)arrow_forwardWrite total ionic and net ionic equations for the following reactions. Be sure to include the states for each species. Note: Reference the Solubility of ionic compounds in water table for additional information. Part 1 of 2 MnI₂(aq) + Hg(NO3)₂(aq) → Total ionic: Net ionic: Part 2 of 2 Mg(NO3)₂ (aq) + 2NaOH(aq) - → Total ionic: ID Net ionic: X X Darrow_forward
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