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Marina86 [1]
3 years ago
10

8.00ml of 1.25M lithiukm hydroxide is reacted with sulfuric acid. It is found that 52.87mL of the sulfuric acid is required to c

ompletely neutralize the lithium hydroxide. What is the approximate molarity of sulfuric acid?
Chemistry
1 answer:
BabaBlast [244]3 years ago
8 0

<u>Answer:</u> The molarity of sulfuric acid is 0.0946 M

<u>Explanation:</u>

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 H_2SO_4

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

We are given:

n_1=2\\M_1=?M\\V_1=52.87mL\\n_2=1\\M_2=1.25M\\V_2=8.00mL

Putting values in above equation, we get:

2\times M_1\times 52.87=1\times 1.25\times 8.00\\\\M_1=\frac{1\times 1.25\times 8.00}{2\times 52.87}=0.0946M

Hence, the molarity of sulfuric acid is 0.0946 M

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