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It depends a bit on what information you are given. However, the principle is the same in all cases, although how you do the specific calculation may vary a bit.

As an example, let's say we have a mixture of 5.00 grams of water and 10.0 grams of ethanol (C2H5OH). What is the mole fraction of the two components?

The first thing we must do is convert the number of grams of each substance into moles. To do that, see the Related Question below:

How do you convert from grams to moles and also from moles to grams?

For water, we have:

5.00 grams ÷ 18.015 grams/mole = 0.2775 moles H2O

For ethanol, we have:

10.0 grams ÷ 46.068 grams/mole = 0.2171 moles C2H5OH

Now we can find the mole ratio, which is defined as follows:

Moles ratio of compound X = number of moles of X ÷ total number of moles in mixture

So the mole ratio of water is: 0.2775 ÷ (0.2775 + 0.2171) = 0.561 or 56.1%

and the mole ratio of ethanol is: 0.2171 ÷ ((0.2775 + 0.2171) = 0.439 or 43.9%

Check your answer! The total mole ratio for all components MUST add up to 1.00:

0.561 + 0.439 = 1.00 Yes!

Note that the weight ratio was 1-to-2 (twice as much ethanol as water by weight), but the mole ratio was completely different.

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The molality of this solution is 1,905; to calculate the molarity you need the density of the solution.

Increasing the amount of the solute in the solution the molarity and the density of this solution increases.

6M

The density is 1,0075 g/cm3 at 20 0C.

Not enough information. To calculate mass, you would need volume and density (mass = volume x density).

Density is the weight per volume of a solution, while the concentration is the amount of particles/molarity per volume.

Is the makeup of the solution expressed as "percent by mass"? If so, to calculate molarity (or normality), you have to also know the density of the solution Step 1. Lets say the solution is 14%, and the density is 1.09 g/mL. We can write the following: (14 grams solute/100 grams solution) (1.09 grams solution/ mL solution) Step 2. Multiplying and cancelling from step 1 gives you 15.26 grams solute / 100 mL solution. Multiplying top and bottom by 10 gives you 152.6 grams solute per liter. Step 3. Molarity is number of moles per liter. Divide the 152.6 grams of the solute by the forumua weight (or molecular weight) of the solute, and you have the number of moles of solute. This number is therefore the molarity of the solution. If the solution is "percent by volume", the number you have is number of grams per 100 mL. Multiply by 10, and you have grams per liter. Then divide by the formula weight, and you have the molarity.

For starters, in analytical science, when trying to make up a certain molarity of solution, you can be given the density of a liquid. from that and the molecular weight of the liquid, you can figure out the volume needed to be taken to make the certain molarity.

13M of HCl

Heavy water (deuterium oxide, D2O). To calculate its molarity you need two costants. Its density at 25C and its molar mass. These are 1.107 g/cm3 and 20.0276 g/mol Molarity = (density / molar mass ) x 1000 moles per litre = 50.78 Molar

Molarity is the no of moles of solute dissolved per litre of a solution. now if u want to find it from the percentage purity , here is the formula for that Molarity = % purity x density x 10 ___________________ molar weight of the solute note : density is usually given %purity problems, if its not u can evualvate it from from formula { d= mass/volume} i hope it solves the problem

1.12 m

Molarity is defined by amount of solute per unit volume; the density is irrelevant; therefore, the molar is simply 0.142 as stated in the question.

0.736 i think good luck

The molar mass of water is 18 g/mole. In one liter, at 4ºC there will be 1000 g (density = 1g/ml). Thus, 1000g x 1 mol/18 g = 55.56 M. At 25ºC, the density of water is ~1.18, thus, 1000 ml x 1.18g/ml = 1180g. The molarity will be 1180 g x 1 mol/18 g = 65.56 M

molarity of moles of solute/liters of solution(not solvent) the volume of the solvent(even if it started at 1 L) would change after adding the solute depending on the molar mass, density, etc of the solute, the molarity would be different

First, you need to get the mass flow rates of all the fluids, then calculate the mass fraction for each of the components. cfluid1 = Mfluid1 / ( Mfluid1 + Mfluid2 + ... ) Next, you can calculate the mixture density as follows; rmix = 1 / ( cfluid1 / rfluid1 + cfluid2 / rfluid2 + ... ) Explanation of the descripstions used. Mfluidx = mass flow rate of fluid x cfluidx = mass fraction of fluid x rfluidx = density of fluid x rmix = density of the mixture (all fluids)

molarity equals moles of solute /volume of solution in litres . moles of NaOH equals 5g/40g = 0.125 and volume of solution will be volume of water + volume of NaOH = 0.5 litre+0.002 l which is nearly 0.5 litre . (volume of NaOH is calculated by its density) so molarity = 0.125mol/0.5litre = 0.25 M

Molarity:1.0 mol (NaOH) /L(solution) = 1.0 M NaOHThe conversions of molality, b, to and from the molarity , c,for one-solute solutions are:c = ρ.b / [1 + b.M]andb = c / [ρ -c.M]where ρ is the mass density of the solution, b is the molality, and M is the molar mass of the solute.

6 kg = 6000 grams and density of water = 1.00 grams/milliliters. 1.00 g/ml = 6000 grams/X ml = 6000 ml which = 6 liters ======================== Molarity = moles of solute/Liters of solution Molarity = 2 moles NaOH/6 Liters = 0.3 M NaOH solution -----------------------------

In dilute solutions... ie closer a solution is to pure water the closer molality and molarity come to equalling each other. This is because the molality uses mass and molarity uses volume, the ratio of these two (mass and volume) is density, and water has the density of 1 therefore the mass and volume are equal to each other. THEREFORE calculating the molarity of water is the same as calculating the molality of water.

The concentration is 1 mol/L or 5,611 g KOH/100 mL solution.

2.79

"MolaRity" is the correct spelling for mass per amount solution."MolaLity" is the correct spelling for mass per amount solvent.The conversions of molality, b, to and from the molarity , c,for one-solute solutions are:c = ρ.b / [1 + b.M]andb = c / [ρ -c.M]where ρ is the mass density of the solution, b is the molality, and M is the molar mass of the solute.

If the density is 1.0 g/ml, one liter of the solution will weigh 1000 grams. 3.0 % of this mass or 30 grams of it is constituted of H2O2. The molar mass of H2O2 is 2 (1.008 + 15.999) = 34.014. The molarity of this solution is therefore 30/34.014 = 0.88, to the justified number of significant digits.