Strontium Nitrate and Ammonium Hydroxide Reaction: Formation of Precipitate

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Discussion Overview

The discussion revolves around the reaction between strontium nitrate and ammonium hydroxide, specifically focusing on the formation of a precipitate and the conditions affecting solubility. Participants explore the implications of solubility and concentration in the context of a laboratory experiment.

Discussion Character

  • Homework-related
  • Experimental/applied
  • Debate/contested

Main Points Raised

  • Some participants present a balanced equation for the reaction, suggesting that no precipitate forms under certain conditions.
  • Others note that not all hydroxides are water-soluble, referencing strontium hydroxide's solubility.
  • One participant mentions that the formation of a precipitate may depend on the concentration of strontium hydroxide produced and the amount of water present.
  • Another participant provides estimates for the pH and hydroxide concentration in a 1 M ammonia solution, suggesting that a higher concentration of strontium ions is needed to observe a precipitate.
  • It is proposed that stronger bases like NaOH or KOH may be necessary to achieve visible precipitation.

Areas of Agreement / Disagreement

Participants express differing views on whether a precipitate forms in the reaction, with some asserting that it does not while others suggest that conditions such as concentration play a critical role. The discussion remains unresolved regarding the specific conditions required for precipitate formation.

Contextual Notes

There are varying solubility product values for strontium hydroxide mentioned, and the discussion highlights the dependence on concentration and pH, which are not fully resolved.

Sace Ver
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Homework Statement


Strontium Nitrate + Ammonium Hydroxide =

Homework Equations


Finding net ionic equation

The Attempt at a Solution


Balanced Equation:
Sr(NO3)2(aq) + NH4OH (aq) = Sr(OH)2(aq) + NH4NO3 there is no precipitate correct? I will not need to find the net-ionic equation.
 
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Sace Ver said:

Homework Statement


Strontium Nitrate + Ammonium Hydroxide =

Homework Equations


Finding net ionic equation

The Attempt at a Solution


Balanced Equation:
Sr(NO3)2(aq) + NH4OH (aq) = Sr(OH)2(aq) + NH4NO3 there is no precipitate correct? I will not need to find the net-ionic equation.
Not all hydroxides are water-soluble:

https://en.wikipedia.org/wiki/Strontium_hydroxide
 
Sace Ver said:
I was doing a lab today and no precipitate formed.
Well, it all depends on how much Sr hydroxide you made and how much water there is.

The solubility figures for Sr hydroxide are given in the Wiki article.

You can contrast those solubility figures with comparable ones for ammonium nitrate:

https://en.wikipedia.org/wiki/Ammonium_nitrate
 
It is rather easy to estimate.

pH of a 1 M ammonia solution is around 11.2, so [OH-] = 4.2×10-3

Different sources list different values for solubility product of Sr(OH)2, but apparently it is around 10-4.

That means using 1 M ammonia you should not expect precipitate unless concentration of the Sr2+ is around 6 M.

Using more concentrated ammonia (3 M) will shift the required Sr2+ concentration down to 1.9 M, still quite high.

No wonder you couldn't see any precipitate. For that you would need a strong base like NaOH or KOH.
 

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