
Concentrated HCl solution is 37.0% HCl and has a density of 1.19 g/mL. A dilute solution of HCl is prepared by diluting 4.50mL of this concentrated HCl solution to 100mL with water. Then 10mL of this dilute HCl solution reacts with an solution. Calculate the volume of 0.108M solution required to precipitate all the chloride as .
Answer
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Hint: The formula to find molarity and molarity of dilute solution obtained from concentrated solution are as below.
Complete Step-by-Step Solution:
We will first calculate the molarity of concentrated HCl solution. From that, we will find the molarity of dilute HCl solution and finally from it, we will find the volume of solution required to complete precipitation.
- We are given that the concentrated HCl solution is 37%. So, we can say that if the solution is of 100 g, then the weight of dissolved HCl will be 37g.
- Density of the solution is given 1.19 g/mL. Now, we will use the formula of the density given below.
So,
Thus, we can write that Volume =
We know that Molecular weight of HCl = Atomic weight of H + Atomic weight of Cl
So, Molecular weight of HCl = 1 + 35.5 = 36.5 g/mol
Now, we will find the molarity of the solution.
So,
Now, we will find the molarity of diluted solution of HCl using the equation given below.
where = Molarity of con. HCl solution = 12.06M
= volume of cone. HCl solution taken to make dilute solution = 4.50 mL
=Molarity of diluted solution
=Volume of diluted solution of HCl = 100mL
So, we can write that
So,
Now, we will take a look at the reaction between HCl and .
- Now, we are given that 10mL of this 0.5427M solution is allowed to react with 0.108M solution.
- From the definition of molarity, we can say that 1000mL of 0.5427M solution will contain 0.5427 moles of HCl. So, 10mL of 0.5427M solution will contain 0.005427 moles.
- Now, we will require 0.005427 moles of to have complete precipitation.
- From the definition of molarity, we can say that 0.108 moles of will be obtained from 1000mL of 0.108M solution. So, 0.005427 moles of can be obtained from
Thus, we found that we will require 50.25mL of 0.108M solution to ensure complete precipitation.
Note: Remember that whenever we make a solution from another solution of known concentration, then we can use the formula to find the volume or molarity whichever is unknown. If we are given normality, then we can use normality of both the solutions in the same formula.
Complete Step-by-Step Solution:
We will first calculate the molarity of concentrated HCl solution. From that, we will find the molarity of dilute HCl solution and finally from it, we will find the volume of
- We are given that the concentrated HCl solution is 37%. So, we can say that if the solution is of 100 g, then the weight of dissolved HCl will be 37g.
- Density of the solution is given 1.19 g/mL. Now, we will use the formula of the density given below.
So,
Thus, we can write that Volume =
We know that Molecular weight of HCl = Atomic weight of H + Atomic weight of Cl
So, Molecular weight of HCl = 1 + 35.5 = 36.5 g/mol
Now, we will find the molarity of the solution.
So,
Now, we will find the molarity of diluted solution of HCl using the equation given below.
where
So, we can write that
So,
Now, we will take a look at the reaction between HCl and
- Now, we are given that 10mL of this 0.5427M solution is allowed to react with 0.108M
- From the definition of molarity, we can say that 1000mL of 0.5427M solution will contain 0.5427 moles of HCl. So, 10mL of 0.5427M solution will contain 0.005427 moles.
- Now, we will require 0.005427 moles of
- From the definition of molarity, we can say that 0.108 moles of
Thus, we found that we will require 50.25mL of 0.108M
Note: Remember that whenever we make a solution from another solution of known concentration, then we can use the formula
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