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3 years ago

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A volume of 0.550 L of gas is contained at 23.0°C. What is the new volume of the gas if it is heated to 57.°C. Assume that the p

ressure of the gas remains constant. Work must be shown to earn credit.

1 answer:

dezoksy [38]3 years ago

7 0

Answer:

0.61 L

Explanation:

T1 = 23.0 +273 = 296K

T2 = 57+273 = 330 K

V2 = (V1×T2)/T1

V2 = (0.55 × 330)/296

V2 = 0.61 L

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g A chemist must prepare of hydrochloric acid solution with a pH of at . He will do this in three steps: Fill a volumetric flask

klemol [59]

The question is incomplete, here is the complete question:

A chemist must prepare 550.0 mL of hydrochloric acid solution with a pH of 1.60 at $25^oC$ . He will do this in three steps: Fill a 550.0 mL volumetric flask about halfway with distilled water. Measure out a small volume of concentrated (8.0M) stock hydrochloric acid solution and add it to the flask. Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits.

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<u>Explanation:</u>

To calculate the hydrogen ion concentration, we use the formula:

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To calculate the volume of concentrated solution, we use the equation:

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$M_1\text{ and }V_1$ = molarity and volume of concentrated acid solution

$M_2\text{ and }V_2$ = molarity and volume of diluted acid solution

We are given:

$M_1=8.0M\\V_1=?mL\\M_2=0.0251M\\V_2=550mL$

Putting values in above equation, we get:

$8.0\times V_1=0.0251\times 550\\\\V_1=\frac{0.0251\times 550}{8.0}=1.7mL$

Hence, the volume of concentrated hydrochloric acid solution is 1.7 mL.

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