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hammer [34]
1 year ago
14

calculate the ratio of [sodium acetate] to [acetic acid] in a buffer solution that has a ph of 4.25. the ka for acetic acid at 2

5 °c is 1.7 × 10−5. please choose the correct answer from the following choices, and then select the submit answer button. answer choices
Chemistry
1 answer:
const2013 [10]1 year ago
5 0

The ratio of [sodium acetate] to [acetic acid] in a buffer solution is 0.30.

Henderson–Hasselbalch equation: pH = pKa + log(cs/ck)

pH = 4.25; pH of buffer solution

pKa = -log(1.7 × 10−5) = 4.77

4.25 = 4.77 + log(cs/ck)

log(cs/ck) =4.25 - 4.77 = -0.52

cs/ck = 10∧(-0.52) = 0.30; ratio of sodium acetate to acetic acid

A buffer can be defined as a substance that prevents the pH of a solution from changing by either releasing or absorbing H⁺ in a solution.

Buffer is a solution that can resist pH change upon the addition of an acidic or basic components and it is able to neutralize small amounts of added acid or base, pH of the solution is relatively stable.

More about sodium acetate: brainly.com/question/24671704

#SPJ4

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How much mass defect is required to release 5.5 x 1020 J of energy?
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Explanation :

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Now put all the given values in above equation, we get:

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6 0
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4 0
3 years ago
10) In order to make spaghetti cook faster, a chef adds salt to water. How many moles of salt would he need to add to 1.0 kg wat
Vadim26 [7]
The answer is 4.9 moles.
Solution: 
Using the equation for boiling point elevation Δt,
     Δt = i Kb m 
we can rearrange the expression to solve for the molality m of the solution:
     m = Δt / i Kb 

Since we know that pure water boils at 100 °C, and the Ebullioscopic constant Kb for water is 0.512 °C·kg/mol, 
     m = (105°C - 100°C) / (2 * 0.512 °C·kg/mol)
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From the molality m of the solution of salt added in a kilogram of water, we can now find the number of moles of salt: 
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                                  = (4.883 mol/kg) * (1.0kg)
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3 years ago
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