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babymother [125]
2 years ago
8

Lactic acid has a pKa of 3.08. What is the approximate degree of dissociation of a 0.35 M solution of lactic acid?

Chemistry
1 answer:
aalyn [17]2 years ago
5 0

The approximate degree of dissociation of a 0.35 M solution of lactic acid is 4,87%

<h3>What is  degree of dissociation?</h3>

The degree of dissociation is the quantity used to express the strength of a base, that is, its ability to conduct electric current, which depends on the amount of ions released in the dissociation.

The degree of dissociation (α) is another way of determining the strength of a base. It indicates the fatty acids that were released from a base when it dissociates in water.

With that being said, C stands for concentration and α is the the degree of dissociation.

Latic Acid can be written as  C3H6O3

CH3Ch(OH)CO2H < -- > H^{+} + CH3CH(OH)CO2^{-}

Ka = \frac{[H^{+}] [CH3CH(OH)CO2^{-}]  }{CH#CH(OH)CO2H} = \frac{C^{2} \alpha^{2}  }{C(1-\alpha )} = \frac{C\alpha ^{2} }{(1-\alpha )}

As α is too small (1-α) can be neglected.

Ka = C\alpha ^{2}  \\\\\\alpha    = \sqrt[]{\frac{Ka}{C} }

Ka = 10^{-3,08}  = 8,32 .10^{-4} .10^{-4} = 0,35

\alpha = \sqrt{\frac{ka}{C} } \\\\\alpha = \sqrt{\frac{8,32.10^{-4} }{0,35} } = 0,0487

In this case, is possible to see that  approximate degree of dissociation of a 0.35 M solution of lactic acid is 4,87%

See more about pKa at: brainly.com/question/14924722

#SPJ1

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3 years ago
sodium reacts with chlorine gas to form sodium chloride. if you have 60 L of chlorine gas at STP and 30 g of sodium, how many gr
Stels [109]

Answer:

75.9 grams of salt

Explanation:

The reaction is the following:  

2Na(s) + Cl₂(g) → 2NaCl(s)   (1)

We have:

m(Na): the mass of sodium = 30 g

V(Cl₂): the volume of the chlorine gas at STP = 60 L

So, to find the mass of NaCl we need to calculate the number of moles of Na and Cl₂.

n_{Na} = \frac{m}{A_{r}} = \frac{30 g}{22.99 g/mol} = 1.30 moles

The number of moles of Cl₂ can be found by the Ideal gas law equation:

PV = n_{Cl_{2}}RT

Where:

P: is the pressure = 1 atm (at STP)

R: is the gas constant = 0.082 L*atm/(K*mol)

T: is the temperature = 273 K (at STP)

n_{Cl_{2}} = \frac{PV}{RT} = \frac{1 atm*60 L}{0.082 L*atm/(K*mol)*273 K} = 2.68 moles

Now we need to find the limiting reactant. From the stoichiometric relation between Na and Cl₂ (equation 1), we have that 2 moles of Na react with 1 mol of Cl₂, so:

n_{Na} = \frac{2 moles Na}{1 mol Cl_{2}}*2.68 moles Cl_{2} = 5.36 moles

Since we have 1.30 moles of Na, the limiting reactant is Na.  

Finally, we can find the number of moles of NaCl and its mass.

n_{NaCl} = n_{Na} = 1.30 moles

m_{NaCl} = n_{NaCl}*M = 1.30 moles*58.44 g/mol = 75.9 g

Therefore, would be formed 75.9 grams of salt.

 

I hope it helps you!                

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C. it explained the odds of finding the position of an electron.

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