All categories

4 years ago

A. 1.0 liter of a 1.0 M mercury (II) chloride (HgCl2) solution IMO)

Chemistry

1 answer:

insens350 [35]4 years ago

4 0

What mass of the following chemicals is needed to make the solutions indicated?

Answer:

271.6g

Explanation:

The mass of the chemicals need to make the needed solution can be derived by obtaining the number of moles first.

Given parameters:

Volume of solution = 1L

Molarity of HgCl₂ = 1M

number of moles of HgCl₂ = molarity of solution x volume

= 1 x 1

= 1 mole

From;

Mass of a substance = number of moles x molar mass;

we can find mass;

Molar mass of HgCl₂ = 200.6 + 2(35.5) = 271.6g/mol

Mass of the substance = 1 x 271.6 = 271.6g

You might be interested in

PLZZZZZZZ HELP MEEEEEE!!!!!!!!!!

nikitadnepr [17]

Answer:

Its Obviously Dinosaurs

Explanation: They died 65 million years ago

7 0

3 years ago

In a chromatography experiment, chlorophyll pigments are separated using paper. What is the stationary phase in this experiment?

Bond [772]

Answer:
The stationary phase in chromatography experiment is paper.

Explanation:
In chromatography experiment, the stationary phase is defined as the fixed substance that is necessary to start chromatography. In our case, this fixed substance is paper, so that makes paper our stationary phase.

Hope this helps :)

4 0

3 years ago

Read 2 more answers

Suppose you see a crescent Moon. How do you know if it is waxing or waning?

nasty-shy [4]

Answer:

waxing is in the evening and waning is in the morning if you cant see the moon in the evening it is waning if you can see it in the evening it is waxing

5 0

3 years ago

If 2.60 g of NaBr are dissolved in enough water to make 160. mL of solution, what is the molar concentration of

navik [9.2K]

This problem has two parts; the first one asking for the concentration of NaBr given both its mass and volume and the second one asking for its volume given both mass and concentration. The answers turn out to be 0.158 M and 211 mL.

<h3>Molarity</h3>

In chemistry, the use of units of concentration depends on both the substances to analyze and their amounts. In such a way, for molarity, one needs the following relationship between the moles of solute and volume of solution:

$M=\frac{n}{V}$

Thus, for the first part of the problem we first calculate the moles in 2.60 g of NaBr via its molar mass:

$2.60g*\frac{1mol}{102.89g} =0.0253mol$

Next, we convert the 160. mL to L by dividing by 1000 in order to obtain 0.160 L to subsequently calculate the molarity:

$M=\frac{0.0253mol}{0.160L}=0.158M$

Next, since the moles remain the same and for the second part we are asked for the volume given the concentration, one can solve for the volume so as to obtain:

$V=\frac{n}{M} =\frac{0.158M}{0.120mol/L}\\ \\V=0.211L$