If 2.0 ml of 6.0m hcl is used to make a 500.0-ml aqueous solution, what is the molarity of the dilute solution?

2 answers:

4 0

Make sure that you understand what they are asking you from this question, as it can be confusing, but the solution is quite simple. They are stating that they want you to calculate the final concentration of 6.0M HCl once a dilution has been made from 2.0 mL to 500.0 mL. They have given us three values, the initial concentration, initial volume and the final volume. So, we are able to employ the following equation:

C1V1 = C2V2
(6.0M)(2.0mL) = C2(500.0mL)
Therefore, the final concentration, C2 = 0.024M.

natita [175]3 years ago

4 0

Answer:

0.024M

Explanation:

You might be interested in

2. A rock occupies a volume of 20 cm and has a mass of 54 grams. Find the density of<br> this rock.

vredina [299]

The answer is 2.7gm/cm^3 . Density is mass divided by volume .

6 0

2 years ago

Where does lava in volcanoes come from?

Stella [2.4K]

Magma can push through holes or cracks in the crust of the volcano, causing a volcanic eruption. Which is when magma flows or erupts onto earth's surface, which is what you call lava (whenever it goes onto the earths surface).

4 0

3 years ago

The ΔHcomb value for anethole is -5539 kJ/mol. Assume 0.840 g of anethole is combusted in a calorimeter whose heat capacity (Cal

bonufazy [111]

Answer:

Final temperature of calorimeter is 25.36^{0}\textrm{C}

Explanation:

Molar mass of anethole = 148.2 g/mol

So, 0.840 g of anethole = $\frac{0.840}{148.2}moles$ of anethole = 0.00567 moles of anethole