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Alex787 [66]
3 years ago
12

What is the buffer component ratio, (bro-)/(hbro) of a bromate buffer that has a ph of 8.08. ka of hbro is 2.3 x 10-9?

Chemistry
1 answer:
Alla [95]3 years ago
3 0

pKa= -log(ka)

= -log(2.3*10^-9)

= 8.64

Now pH can be calculated using equation:

pH=pka+log(BrO-)/(HBrO)

8.08 =8.64+log(BrO-)/(HBrO)

log(BrO-)/(HBrO)=8.08-8.64

= -0.56

(BrO-)/(HBrO)= 10^-0.56

=0.275

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What is the boiling point of a solution of 12.0 g of urea in 165.0 g of water
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Answer:

T = 100.63 °C

Explanation:

To solve this question, we need to know what are we talking about here. In this case, we want to know the boiling point of a solution with Urea in water. This is a colligative property, so, the expression to use to calculate that is the following:

ΔT = m * K / MM * kg water (1)

Where:

ΔT: difference of temperatures (Tb of solution - Tb water)

m: mass of the urea

K: ebulloscopic constant of the water (0.52 ° C / m)

MM: molecular mass of urea

The boiling point of water is 100 °C, we have the mass of the urea, but not the molar mass. The urea has the formula CH₄N₂O, so the molar mass can be calculated using the atomic mass of the elements (I will use a rounded number for this):

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Now, we can calculate the ΔT and then, the boiling point of the solution:

ΔT = 12 * 0.52 / 60 * 0.165

ΔT = 6.24 / 9.9

ΔT = 0.63 °C

the value of ΔT is a difference between the boling point of water and the solution so:

ΔT = Ts - Tw

Ts = ΔT + Tw

Replacing we have:

Ts = 100 + 0.63

<h2>Ts = 100.63 ° C</h2>
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