# Net ionic equation questions.

## 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.

## The Attempt at a Solution

a) Al(NO3)3 + K2CO3 ----> AlK2 + NO3 ?

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Borek
Mentor
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:

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?

Borek
Mentor
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.

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.