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3 years ago

You have 87.0mL of a 0.500M stock solution that must be diluted to 0.100M. What is the final volume g

Chemistry

1 answer:

IgorLugansk [536]3 years ago

8 0

Answer:

435 mL

Explanation:

Step 1: Given data

Initial volume (V₁): 87.0 mL

Initial concentration (C₁): 0.500 M

Final volume (V₂): ?

Final concentration (C₂): 0.100 M

Step 2: Calculate the final volume of the solution

We want to prepare a diluted solution from a concentrated one. We can calculate the final volume of the solution using the dilution rule.

C₁ × V₁ = C₂ × V₂

V₂ = C₁ × V₁ / C₂

V₂ = 0.500 M × 87.0 mL / 0.100 M

V₂ = 435 mL

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A solution is made using 200.0 mL of methanol (density 0.792 g/mL) and 985.1 mL of water (density 1.000 g/mL). What is the mass

DaniilM [7]

Answer: The mass percent of methanol in solution is 13.85 %

Explanation:

To calculate the mass of water, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

For water:

Density of water = 1.000 g/mL

Volume of water = 985.1 mL

Putting values in above equation, we get:

$1.000g/mL=\frac{\text{Mass of water}}{985.1mL}\\\\\text{Mass of water}=(1.000g/mL\times 985.1mL)=985.1g$

For methanol:

Density of methanol = 0.792 g/mL

Volume of methanol = 200.0 mL

Putting values in above equation, we get:

$0.792g/mL=\frac{\text{Mass of methanol}}{200.0mL}\\\\\text{Mass of methanol}=(0.792g/mL\times 200.0mL)=158.4g$

To calculate the mass percent of methanol, we use the equation:

$\text{Mass percent of methanol}=\frac{\text{Mass of methanol}}{\text{Mass of solution}}\times 100$

Mass of solution = [158.4 + 985.1] g = 1143.5 g

Mass of methanol = 158.4 g

Putting values in above equation, we get:

$\text{Mass percent of methanol}=\frac{158.4g}{1143.5g}\times 100=13.85\%$

Hence, the mass percent of methanol in solution is 13.85 %

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Which has the greater mass 10.0 g or 1000 mg

Natalka [10]

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A gas sample enclosed in a rigid metal container at room temperature (20.0∘C) has an absolute pressure p1. The container is imme

Vlad [161]

Answer : The new absolute pressure is, $1.068\times P_1$

Explanation :

Gay-Lussac's Law : It is defined as the pressure of the gas is directly proportional to the temperature of the gas at constant volume and number of moles.

$P\propto T$

or,

$\frac{P_2}{P_1}=\frac{T_2}{T_1}$

where,

$P_1$ = initial pressure of gas

$P_2$ = final pressure of gas

$T_1$ = initial temperature of gas = $20.0^oC=273+20.0=293.0K$

$T_2$ = final temperature of gas = $40.0^oC=273+40.0=313.0K$

Now put all the given values in the above equation, we get:

$\frac{P_2}{P_1}=\frac{313.0K}{293.0K}$

$\frac{P_2}{P_1}=1.068$

$P_2=1.068\times P_1$

Therefore, the new absolute pressure is, $1.068\times P_1$

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