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serg [7]
3 years ago
5

Calculate the ph of a buffer that is 0.13m in lactic acid and 0.10m in sodium lactate.

Chemistry
1 answer:
Alona [7]3 years ago
3 0
According to Henderson–Hasselbalch Equation,

                                       pH  =  pKa + log [Lactate] / [Lactic Acid]
As,
      Ka of Lactic Acid  =  1.38 × 10⁻⁴

           pKa  = -log Ka
           pKa  = -log 1.38 × 10⁻⁴
           pKa  =  3.86
So,
                                  pH  =  3.86 + log [0.10] / [0.13]

                                  pH  =  4.74 + log 0.769

                                  pH  =  4.74 - 0.11

                                  pH  =  4.63
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Answer:

D) 2-methylpent-2-ene

Explanation:

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2-methylpent-1-ene is minor product since double bond form with secondary Carbon rather than primary Carbon.

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3 years ago
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3. Discuss the difference between molarity and molality, state the units of each, state the symbol for each, and give an example
dangina [55]

<span>Molality(m) or molal concentration is a measure of concentration and it refers to amount of substance in a specified amount of mass of the solvent. Used unit for molality is mol/kg which is also sometimes denoted as 1 molal. It is equal to the moles of solute (the substance being dissolved) divided by the kilograms of solvent (the substance used to dissolve).</span>

Molarity(M) or molar concentration is also a measure of concentration and represents the amount of substance per unit volume of solution(number of moles per litre of solution. Used unit for molarity is mol/L or M. A solution with a concentration of 1 mol/L is equivalent to 1 molar (1 M).

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4 0
3 years ago
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3 years ago
Solution made up of a
Vadim26 [7]

Answer:

solute and solvent

Explanation:

Because solutes dissolves in solvent to form a solution

5 0
3 years ago
Which of the following gases effuses the fastest at a given temperature?
Sholpan [36]

Answer: -

H₂ will diffuse the fastest.

Explanation: -

According to Graham's Law of Diffusion

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Molar mass of Ne = 20 g / mol

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Thus H₂ will diffuse the fastest.

7 0
3 years ago
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