HCO3- as a Buffer

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• prepare a liter of "carbonate buffer" at a pH of 10.10

  To make a "carbonate buffer" at pH 10.10, do we want to have a mixture of H2CO3 (carbonic acid) and HCO3- (bicarbonate), OR do we want a mixture of HCO3- (bicarbonate) and CO3-2(carbonate)? That's the question, isn't it?

• pH calculations for buffers, mixtures of acids and bases

  PART FOUR: Answer this question in exactly the same way as part three, above. NaOH is a strong base, so it will react with the weak acid (HCO3(1-)). Answer: pH = 10.25.

• Biochemistry Questions

  Solution: The carbonic acid buffer is H2CO3 + H2O → H3O+ + HCO3- Let's assume we want the total buffer concentration to be 0.1M.

• Chemistry/Buffer Systems: Metabolic Acidosis

  14445 Chemistry/Buffer Systems: Metabolic Acidosis If, during a metabolic acidosis the pH falls to 7.1, and the (HCO3) falls to 12 meq/L, the total conc. of H+ ions neutralized by the (HCO3)/(CO2) buffer system as the metabolic acid is titrated is approx

• Acid-base Equilibrium and High Altitude Disease

  H2CO3(aq) H+(aq) + HCO3-(aq) This buffer functions in exactly the same way as the phosphate buffer. Additional H+ is consumed by HCO3- and additional OH- is consumed by H2CO3.

• bicarbonate-carbonic acid buffer system

  45567 Bicarbonate-Carbonic Acid Buffer System Preparing a Buffer. The pH of blood is 7.40. Calculate the [HCO3-] / [H2CO3] ratio of a bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40.

• Buffers and Buffer Type Solutions

  as needed.

• Calculating the pH of a buffer

  is the bicarbonate ion, HCO3, and the conjugate base [A-] is the OH-.

• Finding chemical equations in a phosphate buffer system

  Hence, in your buffer H2PO4- will react as an acid and HPO42- as a base. This is illustrated in your problem: 1. Since H2SO4 is a strong acid it will react with a basic component of the buffer i.e. HPO42-.