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I am Lyosha [343]
3 years ago
11

A certain weak acid, ha, has a ka value of 6.0×10−7. calculate the percent ionization of ha in a 0.10 m solution.

Chemistry
1 answer:
joja [24]3 years ago
5 0
For the purpose, we will use the equation for determining the dissociation constant from concentration and <span>percent of ionization:

Kd = c </span>× α²

α = √(Kd/c) × 100%

Kd = 6.0×10⁻⁷

c(HA) = 0.1M

α = √(6.0×10⁻⁷/0.1)  × 100% =  0.23%

So, in the solution, the acid <span>percent of ionization will be just 0.23%.</span>

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Which has the greater concentration of hydrogen ions, a substance with a pH of 5 or a substance with a pH of 4?
evablogger [386]

Answer:

pH 4

Explanation:

Firstly, we define pH as the negative logarithm to base 10 of the concentration of hydrogen ions.

Mathematically, we express this as:

pH = -log[H+]

Now let’s us calculate the concentration of hydrogen in each of the pH

For pH 4, we have:

4 = -log[H+]

[H+] = -Antilog(4)

[H+] = 0.0001M

For pH 5,

[H+] = -Antilog(5)

[H+] = 0.00001M

We can see that 0.0001 is greater than 0.00001 and thus it has a greater concentration of hydrogen ions

4 0
3 years ago
What are some substances that from ion-ion forces?
Anika [276]

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The three major types of intermolecular interactions are dipole–dipole interactions, London dispersion forces (these two are often referred to collectively as van der Waals forces), and hydrogen bonds.

6 0
3 years ago
Given that an E2 reaction proceeds with anti periplanar stereochemistry, draw the products of each elimination. The alkyl halide
serg [7]

Answer:

See explanation below

Explanation:

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In the case of reaction b) we have the same reaction, with the difference that we have changed the CH3 and phenyl group of positions. This will cause that the reaction will proceed the same but the stereochemistry of the final product will be changed too. In this case, and according to the picture 3 attached, we can see that the product formed is a cis product. So we can conclude that the relation of product a) and b) is that they are isomers, the trans and cis isomers respectively. See picture below for mechanism and products

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Answer:

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4 0
2 years ago
Calculate the ph of a buffer that is 0.13m in lactic acid and 0.10m in sodium lactate.
Alona [7]
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
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So,
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                                  pH  =  4.74 + log 0.769

                                  pH  =  4.74 - 0.11

                                  pH  =  4.63
3 0
3 years ago
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