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Veseljchak [2.6K]
3 years ago
15

A solution of hydrochloric acid of unknown concentration was titrated with 0.10 M NaOH. If a 100.-mL sample of the HCl solution

required exactly 1.0 mL of the NaOH solution to reach the equivalence point, what was the initial pH of the HCl solution
Chemistry
1 answer:
madam [21]3 years ago
6 0

<u>Answer:</u> The initial pH of the HCl solution is 3

<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 HCl

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

We are given:

n_1=1\\M_1=?M\\V_1=100mL\\n_2=1\\M_2=0.10M\\V_2=1mL

Putting values in above equation, we get:

1\times M_1\times 100=1\times 0.10\times 1\\\\M_1=\frac{1\times 0.10\times 1}{1\times 100}=10M

1 mole of HCl produces 1 mole of H^+ ions and 1 mole of Cl^- ions

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

pH=-\log[H^+]

We are given:

[H^+]=0.001M

Putting values in above equation, we get:

pH=-\log (0.001)\\\\pH=3

Hence, the initial pH of the HCl solution is 3

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Explanation:

2HI(g)\rightarrow H_2(g)+I_2(g)&#10;

Rate Law: k[HI]^2&#10;

Rate constant of the reaction = k = 6.4\times 10^{-9} L/mol s

Order of the reaction = 2

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