It is a solution commonly used in biological research. It is a buffer solution commonly used in biological research.
(Redirected from Phosphate buffered saline). Phosphate-buffered saline (abbreviated PBS) is a buffer solution commonly used in biological research. It is a water-based salt solution containing sodium phosphate, sodium chloride and, in some formulations, potassium chloride and potassium phosphate. The simplest way to prepare a PBS solution is to use PBS buffer tablets or pouches. They are formulated to give a ready-to-use PBS solution upon dissolution in a specified quantity of distilled water. They are available in the standard volumes: 100, 200, 500 and 1000 mL, and 10, 25, 50 and 100 L. Sodium phosphate. 1 M sodium phosphate buffer (pH 6.0–7.2). Mixing 1 M NaH 2 PO 4 (monobasic) and 1 M Na 2 HPO 4 (dibasic) stock solutions in the volumes designated in the table below results in 1 L of 1 M sodium phosphate buffer of the desired pH. To prepare the stock solutions, dissolve 138 g of NaH 2 PO 4 •H 2 O (monobasic; m.w. The phosphate buffer system operates in the internal fluid of all cells. This buffer system consists of dihydrogen phosphate ions (H2PO4-) as hydrogen-ion donor (acid) and hydrogen phosphate ions (HPO42-) as hydrogen-ion acceptor (base). These two ions are in equilibrium with each other as indicated by the chemical equation below. 1 This pH should be within one pH unit from the pKa of the acid/conjugate base. 2  So, you can prepare a buffer at pH 2 or pH 7, for example, but pH 9 would be pushing it. 3  Use the Henderson-Hasselbach equation to calculate how much acid and base you need. 4  You can simplify the calculation if you make 1 liter of buffer. 1 Use the Henderson-Hasselbach equation to calculate how much acid and base you need. 2  You can simplify the calculation if you make 1 liter of buffer. 3  Select the pKa value that is closest to the pH of your buffer. 0.1 M sodium phosphate buffer (pH 7.4). Add 3.1 g of NaH 2 PO 4 •H 2 O and 10.9 g of Na 2 HPO 4 (anhydrous) to distilled H 2 O to make a volume of 1 L. The pH of the final solution will be 7.4. This buffer can be stored for up to 1 mo at 4°C. Mixing 1 M NaH 2 PO 4 (monobasic) and 1 M Na 2 HPO 4 (dibasic) stock solutions in the volumes designated in the table below results in 1 L of 1 M sodium phosphate buffer of the desired pH. To prepare the stock solutions, dissolve 138 g of NaH 2 PO 4 •H 2 O (monobasic; m.w. Experimental Procedures: 1. Prepare 10 mL of a 0.01 M phosphate buffer, pH 7.70, from stock solutions of 0.1 M K 2 HPO 4 and 0.2 M KH 2 PO 4. (pKa for the weak acid = 7.20). A. Use the Henderson-Hasselbalch equation to calculate the volume of each stock solution needed.  1 So, you can prepare a buffer at pH 2 or pH 7, for example, but pH 9 would be pushing it. 2  Use the Henderson-Hasselbach equation to calculate how much acid and base you need. 3  You can simplify the calculation if you make 1 liter of buffer. 4  Select the pKa value that is closest to the pH of your buffer. 1 Use the Henderson-Hasselbach equation to calculate how much acid and base you need. 2  You can simplify the calculation if you make 1 liter of buffer. 3 Introduction. Phosphate buffered saline (abbreviated as PBS) is a buffer solution commonly used in biological research. It is a salty solution containing sodium chloride, sodium phosphate, and (in some formulations) potassium chloride and potassium phosphate. The buffer helps to maintain a constant pH
https://en.wikipedia.org/wiki/Phosphate_buffered_saline http://cshprotocols.cshlp.org/content/2006/1/pdb.rec8303.full?text_only=true http://scifun.chem.wisc.edu/chemweek/BioBuff/BioBuffers.html http://chemistry.about.com/od/acidsbases/a/phosphatebutter.htm http://cshprotocols.cshlp.org/content/2006/1/pdb.rec8303.full?text_only=true http://www.xula.edu/chemistry/documents/biolab/Carroll%20lab%20Chap%203.pdf http://chemistry.about.com/od/acidsbases/a/phosphatebutter.htm http://www.protocolsonline.com/recipes/phosphate-buffered-saline-pbs/
what is phosphate buffer