Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
![1. Consider the chemical reaction.
\[ 3 \text{MgCl}_2 (\text{aq}) + 2 \text{Na}_3\text{PO}_4 (\text{aq}) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (\text{s}) + 6 \text{NaCl} (\text{aq}) \]
Write the net ionic equation for the chemical reaction, including phases.
**Net ionic equation:**
[Space for the equation]
Which of these ions are considered spectator ions for this reaction?
- [ ] \( \text{PO}_4^{3-} \)
- [ ] \( \text{Na}^+ \)
- [ ] \( \text{Mg}^{2+} \)
- [ ] \( \text{Cl}^- \)](https://content.bartleby.com/qna-images/question/9985dfa2-26db-459e-98b3-af2531f0e329/a2fd28a0-8212-4c31-af3d-41871a68f655/ae651og_processed.png)
Transcribed Image Text:1. Consider the chemical reaction.
\[ 3 \text{MgCl}_2 (\text{aq}) + 2 \text{Na}_3\text{PO}_4 (\text{aq}) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (\text{s}) + 6 \text{NaCl} (\text{aq}) \]
Write the net ionic equation for the chemical reaction, including phases.
**Net ionic equation:**
[Space for the equation]
Which of these ions are considered spectator ions for this reaction?
- [ ] \( \text{PO}_4^{3-} \)
- [ ] \( \text{Na}^+ \)
- [ ] \( \text{Mg}^{2+} \)
- [ ] \( \text{Cl}^- \)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. KI+Pb(No3)2arrow_forwardA student mixes phosphoric acid and sodium hydroxide in a neutralization reaction. Write the balanced chemical equation.Write the ionic equation.List the spectator ions(s).Write the net ionic equation.arrow_forward4. Write the balanced molecular, ionic, and net ionic equations for the following reactions. Is it precipitation, gas formation, and/or neutralization? a. FeCO3 (aq) + HCl (aq) → b. AgNO3 (aq) + PbBr2 (aq) → c. Ca(OH)2(aq) + HC2H3O2(aq) → d. H₂SO4(aq) + BaCl2(aq) → e. NiSO4(s) + HCl (aq) → f. CaSO3(s) + HNO3(aq) → g. Co(PO4)(aq) + H₂SO3(aq) → →> h. BaS(s) + LiOH(aq) - i. KOH(aq) + HI(aq) →> j. CsOH(aq) + H₂S(g) →arrow_forward
- Consider the reaction between aqueous solutions of Pb(NO3)2 and KBr. Pb(NO3)2(aq) + KBr(aq) = a. Complete the balanced molecular equation by writing the chemical formulas of the products. Write the physical states of the products. b. Write the balanced total ionic equation. c. Write the net ionic equation.arrow_forwardIf a precipitate will form, enter its empirical formula in the last column.arrow_forwardA student mixed a series of aqueous solutions in an experiment and recorded the results in the table below. (ppt = precipitate formed, NR = no reaction observed). Fe2(SO3)3 Li2CO3 Na3PO4 NH4Cl Pb(NO3)2 ppt ppt ppt ppt KNO3 NR NR NR NR Using the data from the table, write a net ionic equation for the reaction of Pb(NO3)2 (aq) and Na3PO4 (aq) on a piece of paperarrow_forward
- Predict the possible products for each reaction. Use the solubility rules to predict the phase of each product. Write the phase for each product. Balance the complete chemical equation. Write the formula equation, complete ionic equation and the net ionic equation ____NaCl (aq)+ ____AgNO3 (aq) ->arrow_forwardWrite balanced ionic equations and net ionic equations for the following reactions: Part A Balanced ionic equation: a precipitate of barium sulfate forms when aqueous solutions of barium nitrate and potassium sulfate are mixed. Express your answer as a chemical equation. Identify all of the phases in your answer. Express single charges as [+], not [1+]. Part B Net ionic equation: a precipitate of barium sulfate forms when aqueous solutions of barium nitrate and potassium sulfate are mixed. Express your answer as a chemical equation. Identify all of the phases in your answer. Express single charges as [+], not [1+]. Part C Balanced ionic equation: zinc ion and hydrogen gas form when zinc metal reacts with aqueous sulfuric acid (H2SO4). Express your answer as a chemical equation. Identify all of the phases in your answer. Express single charges as [+], not [1+]. While this is not strictly correct, you can assume that…arrow_forwardHi, I was wondering if you could help me with this question. The question is asking to write out and balance the precipitation reaction. But I am a little stuck on how to balance both sides. Am I going in the right direction? How do I balance the NO3 on both sides of the reaction? Thank you!arrow_forward
- Predict the possible products for each reaction. Use the solubility rules to predict the phase of each product. Write the phase for each product. Balance the complete chemical equation. Write the formula equation, complete ionic equation and the net ionic equation ____K2SO4 (aq) + ____BaCl2 (aq) ->arrow_forwardComplete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? ? nickel(II) nitrate manganese(II) chloride yes no silver nitrate potassium sulfide olo yes no barium nitrate potassium acetate O yes no Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ........................................arrow_forwardDo not give handwriting solution.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY