What are the net ionic equations for these reactions?

  • Thread starter Thread starter Zachalmighty
  • Start date Start date
  • Tags Tags
    Ionic Net
Click For Summary

Discussion Overview

The discussion revolves around determining net ionic equations for two chemical reactions, one involving aluminum nitrate and potassium carbonate, and the other involving hydroiodic acid and methylamine. Participants explore concepts related to solubility rules, dissociation of compounds, and the interpretation of concentration in the context of these reactions.

Discussion Character

  • Homework-related
  • Exploratory
  • Technical explanation

Main Points Raised

  • One participant presents a homework question asking for the net ionic equation, formula equation, complete ionic equation, and net ionic equation for two reactions.
  • Another participant suggests checking solubility rules in textbooks or online resources, indicating that the second reaction is an acid-base reaction with no precipitate.
  • There is a question regarding the meaning of "dissociates," with participants discussing whether it refers to breaking down into individual atoms or remaining as complete ions like NO3.
  • Clarification is provided that dissociation of aluminum nitrate results in Al3+ and NO3- ions.
  • Participants discuss the meaning of concentration, with one noting that it refers to the amount per volume and does not depend on charge, while another confirms that concentration is interpreted as molarity.
  • One participant acknowledges a misunderstanding regarding concentration and thanks another for clarification.

Areas of Agreement / Disagreement

Participants express differing views on the presence of a precipitate in the second reaction and the interpretation of dissociation and concentration. The discussion remains unresolved regarding the net ionic equations and the specifics of the reactions.

Contextual Notes

Participants have not reached a consensus on the net ionic equations, and there are assumptions regarding solubility rules and the nature of the reactions that remain unverified.

Zachalmighty
Messages
3
Reaction score
0

Homework Statement


1) You mix a 45.0 mL solution of 0.250 M Al(NO3)3* with a 30.0 mL solution of 0.600 M K2C)3. (a) Give the net ionic equation. (b) How many grams of the precipitate forms? (c) After the reaction, what is the concentration of the excess ions?

*All of the numbers in the listed molecules are subscripts.

2. Give the formula equation, the complete ionic equation, and the net ionic equation of the reaction in water between hydroiodic acid and CH3NH2*.

*the numbers here are subscript as well.

Homework Equations


The Attempt at a Solution


a) Al(NO3)3 + K2CO3 ----> AlK2 + NO3 ?
 
Last edited:
Physics news on Phys.org
Well, if you know that you are assumed to use solubility rules, I suppose you may check them in your textbook. You may also try to google them:

http://www.google.com/search?q=solubility+rules

In the second reaction there will be no precipitate, this is acid base reaction.
 
Is it safe to assume that when it says dissociates it means that a compound like NO3would turn into N and 03 or does it simply mean that it breaks with whatever else it is bonded to as the complete compound NO3?

By concentration of the remaining Ions it means whether they are negative or positively charged, right?
 
Zachalmighty said:
Is it safe to assume that when it says dissociates it means that a compound like NO3would turn into N and 03 or does it simply mean that it breaks with whatever else it is bonded to as the complete compound NO3?

Dissociates into Al3+ and NO3-.

By concentration of the remaining Ions it means whether they are negative or positively charged, right?

No, concentration is amount per volume, charge doesn't matter. For example you may have solution that contains 0.1M (mol/L) Na+.

This is just a limiting reagent question.
 
Borek said:
Dissociates into Al3+ and NO3-.



No, concentration is amount per volume, charge doesn't matter. For example you may have solution that contains 0.1M (mol/L) Na+.

This is just a limiting reagent question.

Ah, ok. So by concentration they mean Molarity! I should have noticed that. Thank you.
 

Similar threads

Understanding Ionic Equations: Pb2+ & I- Reactants
  • · Replies 6 ·
Replies
6
Views
3K
Balancing acid equation-net ionic equation
  • · Replies 16 ·
Replies
16
Views
3K
Complete and Net Ionic Equations
  • · Replies 3 ·
Replies
3
Views
8K
Net Ionic Lab Question (the lab procedure)
  • · Replies 6 ·
Replies
6
Views
2K
Net Ionic Equation of Four Solutions
  • · Replies 1 ·
Replies
1
Views
1K
Acid-Base Reactions: Did the Solutions Neutralize Each Other? | Homework Help
  • · Replies 2 ·
Replies
2
Views
3K
Net Ionic Equation for HC2H3O2 + NH3 Reaction
  • · Replies 1 ·
Replies
1
Views
3K
What is the net ionic equation for the reaction between HF and KOH?
  • · Replies 2 ·
Replies
2
Views
25K
Finding balanced net ionic equation of reaction with three reactants
  • · Replies 1 ·
Replies
1
Views
12K
Net Ionic Equations: Solutions & Examples
  • · Replies 2 ·
Replies
2
Views
2K