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3 years ago

What is the molarity of a solution made by mixing 75.0 mL of 3.00 M NH₄OH with enough water to give 250. mL of solution?

Chemistry

2 answers:

enyata [817]3 years ago

7 0

Answer:

Mass 1=3M

Mass 2=?

Volume1=75mL

Volume2=250mL

By using molarity formula:

<u>mass1*volume 1=mass2*volume 2</u>

3M*75=mass2*250

mass2=225/250

mass2:0.9M

<h3>the molarity of a solution is 0.9M.</h3>

strojnjashka [21]3 years ago

4 0

M1=3M
M2=?
V1=75mL
V2=250mL

We know

$\boxed{\Large{\sf M_1V_1=M_2V_2}}$

$\\ \Large\sf\longmapsto M_2=\dfrac{M_1V_1}{V_2}$

$\\ \Large\sf\longmapsto M_2=\dfrac{3(75)}{250}$

$\\ \Large\sf\longmapsto M_2=\dfrac{225}{250}$

$\\ \Large\sf\longmapsto M_2=0.9M$

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2.61 kilograms of water in a container have a pressure of 200 kPa and temperature of 200°C . What is the volume of this containe

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<u>Answer:</u> The volume of the container is $2.8497m^3$

<u>Explanation:</u>

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T = temperature of container = $200^oC=[200+273]K=473K$

Putting values in above equation, we get:

$200kPa\times V=\frac{2610g}{18g/mol}\times 8.31\text{L kPa }\times 473K\\\\V=2849.7L$

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