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Otrada [13]
3 years ago
14

What volume of 0.235 M H2SO4 is needed to titrate 40.0 mL of 0.0500 M Na2CO M NaCO3 solution?

Chemistry
1 answer:
Andreyy893 years ago
5 0

Answer: The volume of 0.235 M H_2SO_4 needed to titrate 40.0 mL of 0.0500 M Na_2CO_3 is 8.51 ml

Explanation:

To calculate the volume 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 H_2SO_4

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is Na_2CO_3

We are given:

n_1=2\\M_1=0.235M\\V_1=?mL\\n_2=2\\M_2=0.0500M\\V_2=40.0mL

Putting values in above equation, we get:

2\times 0.235\times V_1=2\times 0.0500\times 40.0\\\\V_1=8.51mL

Thus volume of 0.235 M H_2SO_4 needed to titrate 40.0 mL of 0.0500 M Na_2CO_3 is 8.51 ml

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You have 16.7 grams of hydrogen and 15.4 grams of oxygen in a synthesis rxn. Which is the limiting reagent?
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Explanation:

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Limiting reactant = ?

Solution:

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2H₂ + O₂   →   2H₂O

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Number of moles = mass/ molar mass

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Now we will compare the moles of both reactant with product,

                 

                             H₂           :          H₂O

                              2            :            2

                             8.35        :            8.35

                             O₂           :          H₂O

                               1            :            2

                             0.48        :        2×0.48 = 0.96 mol

The number of moles of water produced by oxygen are less so it will limiting reactant.

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3 years ago
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