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3 years ago

15

When viewing a cork through his homemade microscope, Robert Hook discovered small compartments that he called

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Hoochie [10]3 years ago

6 0

Answer:

Answer: cells

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2 years ago

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2 years ago

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:

The dissociation constant for formic acid = $K_a=1.8\times 10^{-4}$

Concentration of HA= 0.5 mM

Concentration of $A^-$ = 0.1 mM

pH = 6.16

First we have to calculate the value of $K_a$ .

Using Henderson Hesselbach equation :

$pH=pK_a+\log \frac{[A^-}{[HA]}$

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

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

$pK_a=6.86$

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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2 years ago