# hasselbalch equation in a sentence

- Most of them use Henderson
*Hasselbalch equation*with different pK values. - This is described by the Henderson-
*Hasselbalch equation*. - We can write two Henderson
*Hasselbalch equations*: - The Henderson-
*Hasselbalch equation*is useful for calculating blood pH, because blood is a buffer solution. - His work contributed to the Henderson
*Hasselbalch equation*, used to calculate pH as a measure of acidity. - It's difficult to find
*hasselbalch equation*in a sentence. - :At some point, though, it gets easier to work forward from the Henderson
*Hasselbalch equations*. - The pH can be calculated by the following formula ( which is a variation of the Henderson-
*Hasselbalch equation*): - In highly concentrated solutions, simple approximations such as the Henderson
*Hasselbalch equation*are no longer valid due to the variations of the activity coefficients. - However, since the carbonic acid concentration is directly proportional to the P _ _ 2 } in the extracellular fluid, the Henderson
*Hasselbalch equation*can be rewritten as follows: - This ratio and its relationship to the pH is described by the Henderson
*Hasselbalch equation*, which, when applied to the bicarbonate buffering system in the extracellular fluids, states that: - The pK a for the quinoline nitrogen of chloroquine is 8.5, meaning it is about 10 % deprotonated at physiological pH as calculated by the Henderson-
*Hasselbalch equation*. - Not that you mentioned it, but you may find Buffer solution and Henderson
*Hasselbalch equation*to be relevent reading .-- contribs 20 : 37, 8 May 2009 ( UTC) - The ratio of these determines the color of the solution and connects the color to the pH value . pH indicators that are weak protolytes, the Henderson
*Hasselbalch equation*for them can be written as: - This is just a consequence of simple equilibrium principles-the Henderson-
*Hasselbalch equation*may look magical, but it's just the talk ) 18 : 13, 2 April 2008 ( UTC) - The larger the value of p " K " a, the smaller the extent of dissociation at any given pH ( see Henderson
*Hasselbalch equation*) that is, the weaker the acid.

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