-
- Posts: 2
- Joined: Sun Aug 16, 2015 3:07 pm
Advertisement
Broad peak in urine but not in water
Discussions about HPLC, CE, TLC, SFC, and other "liquid phase" separation techniques.
2 posts
Page 1 of 1
Why do I get a broad peak for D-serine during chiral separations in urine but not in standard solutions when eluting using the same basic mobile phase gradient (10mM ammonium bicarbonate with acetonitrile) on the Xevo TQS in +ESI mode? This is true for both unlabelled and deuterium labelled D-serine.
-
- Posts: 69
- Joined: Tue Jul 31, 2012 9:36 pm
Off the cuff, assuming you're using RP or HILIC, but some information about your column and chromatography modes might be helpful.
Try a few pH adjustments in your MP (1 around 4.0-4.2, another around 7, and another around 8.5-9 -- column willing) and see if one of those pH ranges helps. I have a feeling the low pH might make the difference. Start with using 0.1% Ammonium Formate + 0.1% Formic Acid (1g/L in water of each) and rerun it.
Another thing, ammonium bicarbonate is inherently unstable in aqueous solution. I doubt your mobile phase is good after even 24 hours. I had problems with aqueous Ammonium Acetate's pH changing slowly over time, and the only thing we could figure was ammonia was evolving out of solution. When we changed the cation to potassium, the problem went away. (Granted we weren't using LCMS, so we could get away with using K.)
Food for thought:
Ammonium Bicarbonate -> Ammonia(g) + Carbonic Acid(aq) -> Ammonia(g) + Carbon Dioxide(g) + Water
Room temperature is enough to slowly push this reaction forward.
Try a few pH adjustments in your MP (1 around 4.0-4.2, another around 7, and another around 8.5-9 -- column willing) and see if one of those pH ranges helps. I have a feeling the low pH might make the difference. Start with using 0.1% Ammonium Formate + 0.1% Formic Acid (1g/L in water of each) and rerun it.
Another thing, ammonium bicarbonate is inherently unstable in aqueous solution. I doubt your mobile phase is good after even 24 hours. I had problems with aqueous Ammonium Acetate's pH changing slowly over time, and the only thing we could figure was ammonia was evolving out of solution. When we changed the cation to potassium, the problem went away. (Granted we weren't using LCMS, so we could get away with using K.)
Food for thought:
Ammonium Bicarbonate -> Ammonia(g) + Carbonic Acid(aq) -> Ammonia(g) + Carbon Dioxide(g) + Water
Room temperature is enough to slowly push this reaction forward.
2 posts
Page 1 of 1
Who is online
In total there are 51 users online :: 0 registered, 0 hidden and 51 guests (based on users active over the past 5 minutes)
Most users ever online was 4374 on Fri Oct 03, 2025 12:41 am
Users browsing this forum: No registered users and 51 guests
Most users ever online was 4374 on Fri Oct 03, 2025 12:41 am
Users browsing this forum: No registered users and 51 guests
Latest Blog Posts from Separation Science
Separation Science offers free learning from the experts covering methods, applications, webinars, eSeminars, videos, tutorials for users of liquid chromatography, gas chromatography, mass spectrometry, sample preparation and related analytical techniques.
Subscribe to our eNewsletter with daily, weekly or monthly updates: Food & Beverage, Environmental, (Bio)Pharmaceutical, Bioclinical, Liquid Chromatography, Gas Chromatography and Mass Spectrometry.
- Follow us on Twitter: @Sep_Science
- Follow us on Linkedin: Separation Science