All categories

3 years ago

How many moles are in a solution with a concentration of 5 M and a volume of 0.25 L?

Chemistry

1 answer:

Otrada [13]3 years ago

5 0

Answer:

160 mL

Explanation:

You might be interested in

Kobotan [32]

Don’t know this oneeeeeeeeeeeee

4 0

3 years ago

To measure the solubility product of lead (II) iodide (PbI2) at 25°C, you constructed a galvanic cell that is similar to what yo

Veronika [31]

Answer:

0.2320V

Explanation:

Voltage can be defined as the amount of potential energy available (work to be done) per unit charge, to move charges through a conductor.

Voltage can be generated by means other than rubbing certain types of materials against each other.

Please look at attached file for solution to the problem.

8 0

4 years ago

In a chemical equation, the sum of the masses ______.

Readme [11.4K]

C. Of the products is equal to the reactants.

Good luck out there! :)

5 0

3 years ago

Read 2 more answers

The critical pressure of carbon dioxide is 72.7 atm what is this value in units of pascals

NeTakaya

Answer:

7366.328 kPa.

Explanation:

The critical pressure of carbon dioxide is 72.7 atm.

To convert from atm to kPa, we use the relation that:

1.0 atm = 101.325 kPa.

Applying conversion factor:

<em>The conversion factor = (101.325 kPa/1.0 atm)</em>

∴ The critical pressure of carbon dioxide (in kPa) = (72.7 atm)(101.325 kPa/1.0 atm) = 7366.328 kPa.

3 0

4 years ago

A 1.87 L aqueous solution of KOH contains 155 g of KOH . The solution has a density of 1.29 g/mL . Calculate the molarity ( M ),

lbvjy [14]

Answer:

[KOH] = 1.47 M

[KOH] = 1.22 m

KOH = 6.86 % m/m

Explanation:

Let's analyse the data

1.87 L is the volume of solution

Density is 1.29 g/mL → Solution density

155 g of KOH → Mass of solute

Moles of solute is (mass / molar mass) = 2.76 moles.

Molarity is mol/L → 2.76 mol / 1.87 L = 1.47 M

Let's determine, the mass of solvent.

Molality is mol of solute / 1kg of solvent

We can use density to find out the mass of solution

Mass of solution - Mass of solute = Mass of solvent

Density = Mass / volume

1.29 g/mL = Mass / 1870 mL

Notice, we had to convert L to mL, cause the units of density.

1.29 g/mL . 1870 mL = Mass → 2412.3 g

2412.3 g - 155 g = 2257.3 g of solvent

Let's convert the mass of solvent to kg

2257.3 g / 1000 = 2.25kg

2.76 mol / 2.25kg = 1.22 m (molality)

% percent by mass = mass of solute in 100g of solution.

(155 g / 2257.3 g) . 100g = 6.86 % m/m

5 0

3 years ago