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Tanya [424]
3 years ago
5

PLEASE HELP !! ILL GIVE BRAINLIEST NO LINKS OR FILES.

Biology
1 answer:
zzz [600]3 years ago
4 0

Answer:

The answer is C.

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A certain buffer is made by mixing a weak acid HA and its conjugate base A–. When HA is present at a concentration of 0.5 mM and
MAVERICK [17]

Answer:The ratio of the concentrations of HA  and A^- when the buffer has a pH of 7.02 is 0.69

Explanation:

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pH = 6.16

First we have to calculate the value of K_a.

Using Henderson Hesselbach equation :

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Now put all the given values in this expression, we get:

6.16=pK_a+\log (\frac{[0.1]}{0.5})

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To calculate the ratio of the concentrations of HA  and A^- when the buffer has a pH of 7.02.

Using Henderson Hesselbach equation :

7.02=6.86+\log \frac{[A^-]}{[HA]}

7.02=6.86+\log \frac{[A^-]}{[HA]}

\frac{[A^-]}{[HA]}=1.44

\frac{[HA]}{[A^-]}=0.69

Thus the ratio of the concentrations of HA  and A^- when the buffer has a pH of 7.02 is 0.69

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How should “free water” have been administered to the patient?
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Patient is allowed to drink water btwn meals (beginning a minimum of 30 mins after meals); oral care must be done prior to consuming water; patient should be upright and use appropriate swallowing strategies.

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