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aksik [14]
3 years ago
14

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The end point was obtained at abou

t 24.8 mL. The concentration of the monoprotic acid is about ........ mol/L.
A) 25.0

B) 0.0600

C) 0.240

D) 0.120

E) None of the above
Chemistry
1 answer:
kati45 [8]3 years ago
5 0

Answer:

The concentration of the acid is about 0.114 M (option E)

Explanation:

Step 1: Data given

Volume of the monoprotic acid = 25.0 mL = 0.025 L

Molarity of the monoprotic acid = ?

Molarity of the NaOH solution = 0.115 M

Volume NaOH = 24.8 mL = 0.0248 L

Step 2: Calculate the concentration

a*Cb * Vb = b * Ca * Va

⇒ a = the coeficient of NaOH = 1

⇒ Cb = the molarity of the acid = TO BE DETERMINED

⇒ Vb = the volume of the acid = 0.025 L

⇒ b = the coefficient of the acid = monoprotic = 1

⇒ Ca = the moalrity of NaOH = 0.115 M

⇒ Va = the volume of NaOH = 0.0248 L

1 * Cb * 0.025 = 1 * 0.115 * 0.0248

0.025 Cb = 0.002852

Cb = 0.11408 M

The concentration of the acid is about 0.114 M

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<u>Answer:</u> The mass of HCl present in 500 mL of acid solution is 36.5 grams

<u>Explanation:</u>

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

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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=50.00mL\\n_2=1\\M_2=0.500M\\V_2=200.mL

Putting values in above equation, we get:

1\times M_1\times 50.00=1\times 0.500\times 200\\\\M_1=\frac{1\times 0.500\times 200}{1\times 50.00}=2M

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2mol/L=\frac{\text{Mass of solute}\times 1000}{36.5g/mol\times 500}\\\\\text{Mass of solute}=\frac{2\times 36.5\times 500}{1000}=36.5g

Hence, the mass of HCl present in 500 mL of acid solution is 36.5 grams

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