Team:Oxford/how much can we degrade
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As one of the products of our reaction is HCl, we have been able to calculate the pH change of the system. However, since a deviation of neutral pH is unfavourable for the bacteria we are working with, we have investigated the effect of using buffers in the aqueous part of our system. | As one of the products of our reaction is HCl, we have been able to calculate the pH change of the system. However, since a deviation of neutral pH is unfavourable for the bacteria we are working with, we have investigated the effect of using buffers in the aqueous part of our system. | ||
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- | + | Derivation of the Van Slyke eqn: | |
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- | <img src="https://static.igem.org/mediawiki/2014/ | + | To simplify calculations, assumptions that HCl completely dissociates, and that the system volume = 1L (allowing concentration and number of moles to be treated interchangeably) are made. |
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+ | Electro-neutrality condition for a system of two substances, HA and BOH: (1.1) | ||
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+ | <img src="https://static.igem.org/mediawiki/2014/1/1c/Oxford_Jack_eqn1.png" style="float:left;position:relative; width:40%; margin-left:0%; margin-right:60%;margin-bottom:2%;" /> | ||
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+ | Total concentration of buffer: | ||
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+ | <img src="https://static.igem.org/mediawiki/2014/1/13/Oxford_Jack_eqn2.png" style="float:left;position:relative; width:35%; margin-left:0%; margin-right:65%;margin-bottom:2%;" /> | ||
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Upon solving the equation in Matlab, it was clear that only a relatively low concentration (0.05 M) of buffer was needed to significantly reduce the pH change of the solution: | Upon solving the equation in Matlab, it was clear that only a relatively low concentration (0.05 M) of buffer was needed to significantly reduce the pH change of the solution: |
Revision as of 14:36, 8 October 2014
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