Q. Is there any logic why ammonium magnesium phosphate stone precipitates at increased PH or alkalized urine?I surfed and came to know that ammonium is an acid and its conjugate base is ammonia but still I am not able to understand the reason for the above question.Can anyone help. Thanks.
why AMP stone precipitate at inc PH?
- Thread starter sgsh
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It's just a natural way that a bug like Proteus Mirabalis works.
It's urease +, so it makes an alkaline environment - by converting urea to CO2 and Ammonia (base - as you described).
By doing that, struvite can more readily precipitate and form a stone (AMP stone/struvite stone/staghorn caliculi).
EDIT: After re-reading your question --> AMP stones are more soluble in acidic environments. Thus, when you have an alkaline environment, it will precipitate more readily.
It's urease +, so it makes an alkaline environment - by converting urea to CO2 and Ammonia (base - as you described).
By doing that, struvite can more readily precipitate and form a stone (AMP stone/struvite stone/staghorn caliculi).
EDIT: After re-reading your question --> AMP stones are more soluble in acidic environments. Thus, when you have an alkaline environment, it will precipitate more readily.
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Well think of it in terms of the Henderson hasselbalch equation,,PH=PKa+log base/conjugate acid,,for NH3/NH4+ base/conjugate acid complex ,,the higher the PH for a given PKa constant,,u wud have an increased NH3 @ de xpense of decreasing NH4+,,making the AMP stone less polar with decreased solubility in water nd increased precipitation,,
