Question

A barium hydroxide solution is prepared by dissolving 2.06 g of Ba(OH)2 in water to make 32.9 mL of solution. What is the concentration of the solution in units of molarity? concentration: 0.364 The barium hydroxide solution is used to titrate a perchloric acid solution of unknown concentration. Write a balanced chemical equation to represent the reaction between barium hydroxide and perchloric acid. chemical equation: 2HCIO4(a Ba(OH2(a)Ba CIO42H2o If 15.9 mL of the barium hydroxide solution was needed to neutralize a 8.50 mL aliquot of the perchloric acid solution, what is the concentration of the acid?

Answer 1

Answer:  1.36 M

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

$Molarity=\frac{n\times 1000}{V_s}$

where,

n = moles of solute

To calculate the moles, we use the equation:

moles of solute= $\frac{\text {given mass}}{\text {molar mass}}=\frac{2.06g}{171g/mol}=0.0120moles$

$Molarity=\frac{0.0120\times 1000}{32.9}=0.364M$

The balanced reaction between barium hydroxide and perchloric acid:

$2HCIO_4+Ba(OH_)2\rightarrow BaCIO_4+2H_2O$

To calculate the concentration of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $HClO_4$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is $Ba(OH)_2$

We are given:

$n_1=1\\M_1=?\\V_1=8.50mL\\n_2=2\\M_2=0.364M\\V_2=15.9mL$

Putting values in above equation, we get:

$1\times M_1\times 8.50=2\times 0.364\times 15.9\\\\M_1=1.36M$

Thus the concentration of the acid is 1.36 M

Answer 2

• The concentration of the barium hydroxide solution is 0.3647 M

• The balanced chemical equation for the reaction is

Ba(OH)₂ + 2HClO₄ → Ba(ClO₄)₂ + 2H₂O

• The concentration of the acid is 1.36 M

To determine the concentration of the barium hydroxide solution,

First, we will calculate the number of moles of Ba(OH)₂ present

From the question  

Mass of Ba(OH)₂ = 2.06g

Using the formula

$Number\ of\ moles = \frac{Mass}{Molar\ mass}$

Molar mass of Ba(OH)₂ = 171.34 g/mol

∴ Number of moles of Ba(OH)₂ = $\frac{2.06}{171.34}$

Number of moles of Ba(OH)₂ = 0.012 moles

Now, for the concentration of the barium hydroxide solution

From the formula

Number of moles = Concentration × Volume

Then,

$Concentration = \frac{Number\ of\ moles}{Volume}$

Number of moles of Ba(OH)₂ = 0.012 moles

Volume of the solution = 32.9 mL = 0.0329 L

∴ Concentration of the solution = $\frac{0.012}{0.0329}$

Concentration of the solution = 0.3647 M

The concentration of the barium hydroxide [Ba(OH)₂] solution is 0.3647 M

Now, from the question

The barium hydroxide solution is used to titrate a perchloric acid solution.

We are to write a balanced chemical equation to represent the reaction.

The balanced chemical equation for the reaction is

Ba(OH)₂ + 2HClO₄ → Ba(ClO₄)₂ + 2H₂O

Also, from the question

15.9 mL of the barium hydroxide solution was needed to neutralize a 8.50 mL aliquot of the perchloric acid solution

To determine the concentration of the acid,

We will use the formula

$\frac{C_{A}V_{A} }{C_{B}V_{B}}=\frac{n_{A}}{n_{B}}$

Where

$C_{A}$ is the concentration of acid

$C_{B}$ is the concentration of base

$V_{A}$ is the volume of acid

$V_{B}$ is the volume of base

$n_{A}$ is the mole ratio of acid

$n_{B}$ is the mole ratio of base

From the question

$V_{A} = 8.50 \ mL$

$C_{B}= 0.3647 \ M$

$V_{B} = 15.9 \ mL$

From the balanced chemical equation

$n_{A} = 2$

$n_{B}=1$

Put all the parameters into the equation

$\frac{C_{A}V_{A} }{C_{B}V_{B}}=\frac{n_{A}}{n_{B}}$

We get

$\frac{C_{A} \times 8.50}{0.3647 \times 15.9} = \frac{2}{1}$

∴ $C_{A} =\frac{2 \times 0.3647 \times 15.9}{1 \times 8.50}$

$C_{A} =\frac{11.59746}{8.50}$

$C_{A} =1.36 \ M$

Hence, the concentration of the acid is 1.36 M

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