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2 years ago

4) What is the IUPAC name of this compound?

Chemistry

1 answer:

zheka24 [161]2 years ago

8 0

Answer:

1,3- dichlorobutane

Explanation:

The IUPAC name of given compound is 1,3- dichlorobutane.

First of all we will select the longest chain.

The given compound is straight chain. So the compound have four carbon atoms means parent name will butane.

Then we will see the position of functional group. Gives the lowest possible number to the functional group attached.

In given compound one chlorine atom is attached on left side and other is on right side. we will start the numbering from left because in this way chlorine will get lowest possible number which 1 and 3.

As we start the numbering from left the one chlorine atom get number one and other is attached on carbon 3 will have number 3.

There are two chlorine atoms so we will give name "dichloro"

The name will be,

⁴CH₃-³CHCl-²CH₂-¹CH₂Cl

1,3- dichlorobutane.

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Answer:

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Explanation:

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2 years ago

In a titration of 47.41 mL of 0.3764 M ammonia with 0.3838 M aqueous nitric acid, what is the pH of the solution when 47.41 mL +

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Answer: The pH of the solution is 1.136

Explanation:

To calculate the moles from molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

For ammonia:

Molarity of ammonia = 0.3764 M

Volume of ammonia = 47.41 mL = 0.04741 L (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

$0.3764mol/L=\frac{\text{Moles of ammonia}}{0.04741L}\\\\\text{Moles of ammonia}=0.01784mol$

For nitric acid:

Molarity of nitric acid = 0.3838 M

Volume of ammonia = (47.41 + 10.00) mL = 57.41 mL= 0.05741 L

Putting values in above equation, we get:

$0.3838mol/L=\frac{\text{Moles of nitric acid}}{0.05741L}\\\\\text{Moles of nitric acid}=0.02203mol$

After the completion of reaction, amount of nitric acid remained = 0.022 - 0.0178 = 0.0042 mol

For the reaction of ammonia with nitric acid, the equation follows:

$NH_3+HNO_3\rightarrow NH_4NO_3$

At $t=0$ 0.0178 0.022

Completion 0 0.0042 0.0178

As, the solution of the reaction is made from strong acid which is nitric acid and the conjugate acid of weak base which is ammonia. So, the pH of the reaction will be based totally on the concentration of nitric acid.

To calculate the pH of the reaction, we use the equation:

$pH=-\log[H^+]$

where,

$[H^+]=\frac{0.0042mol}{0.05741L}=0.0731M$

Putting values in above equation, we get:

$pH=-\log(0.0731)\\\\pH=1.136$

Hence, the pH of the solution is 1.136

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