The henderson-hasselbalch equation relates the ph of a buffer solution to the pka of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. the equation is important in laboratory work that makes use of buffered solutions, in industrial processes where ph needs to be controlled, and in medicine, where understanding the henderson-hasselbalch equation is critical for the control of blood ph.
(a)-as a technician in a large pharmaceutical research firm, you need to produce 250.ml of 1.00 m a phosphate buffer solution of ph = 7.18. the pka of h2po4? is 7.21. you have 2.00 l of 1.00 m kh2po4 solution and 1.50 l of 1.00 m k2hpo4 solution, as well as a carboy of pure distilled h2o. how much 1.00 m kh2po4 will you need to make this solution? express your answer numerically in milliliters to three significant figures.
(b)-if the normal physiological concentration of hco3- is 24 mm, what is the ph of blood if pco2 drops to 35.0mmhg? express your answer numerically using one decimal place.