# Solving Molarity Problems

Determine the mass of miconazole used to form the aforementioned solution in milligrams.” C Step 1: Determine which formula(s) to use. Using the relationship between mass, moles and molecular weight, we can convert the number of moles to mass later (see previous article). The concentration is already expressed in M so we do not need to do any conversion here. Now that we are using the correct units, we may now use Formula 1 to determine the number of moles.On the other hand, the volume of the solvent is expressed in ml so we will need to convert the volume from ml to l. Step 4: Convert moles to mass Recall from the previous article that the relationship between moles and mass is as follows: Using a periodic table and the provided chemical formula of miconazole, the molecular weight of miconazole is determined as 416.13 g/mol. 0.0208 g = 20.8 mg Answer to Problem 2: 20.8 mg of miconazole was dissolved in 50 ml of solvent to form a solution with a concentration of 0.001 M.

Determine the mass of miconazole used to form the aforementioned solution in milligrams.” C Step 1: Determine which formula(s) to use. Using the relationship between mass, moles and molecular weight, we can convert the number of moles to mass later (see previous article). The concentration is already expressed in M so we do not need to do any conversion here. Now that we are using the correct units, we may now use Formula 1 to determine the number of moles.On the other hand, the volume of the solvent is expressed in ml so we will need to convert the volume from ml to l. Step 4: Convert moles to mass Recall from the previous article that the relationship between moles and mass is as follows: Using a periodic table and the provided chemical formula of miconazole, the molecular weight of miconazole is determined as 416.13 g/mol. 0.0208 g = 20.8 mg Answer to Problem 2: 20.8 mg of miconazole was dissolved in 50 ml of solvent to form a solution with a concentration of 0.001 M.

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Typically in a laboratory setting such as ones in an academic setting, it isn’t uncommon to work with volumes of solvent less than a litre for health and safety reasons and to curtail costs.

In such cases, known amounts of chemical substance are dissolved in volumes lower than one litre and the concentration is generally expressed in molarity (M or mol/L). We will now go through some examples to try and help you understand how to calculate the molarity and how to do calculations to do with molarity.

Express the concentration in mol/L.” The relationship between molarity, moles and volume are shown below.

where M = molarity (M or mol/L), n = number of moles (mol) and v = volume (L). We were given the number of moles of the substance and the volume of solvent used. In order to solve Problem 1, we will need to use Formula 1. The number of moles of D-Xylose is already expressed in mol so we do not need to do any conversion here. Now that we are using the correct units, we may now use Formula 1 to determine the concentration in molarity.

2200 mg of cis-(−)-carveol = 2.2 g of cis-(−)-carveol. “Suppose you were tasked to make up 50 ml of 25 m M aqueous solution of KBr. Using the relationship between moles, molecular weight and mass, we can determine the amount of KBr we need to form 50 ml of 25 m M aqueous solution of KBr. Conversion from millilitre to litre: 50 ml = 0.05 l Conversion from millimolar to molar: 25 m M = 0.025 M Step 3: Use the formulas Conversion from millilitre to litre: 50 ml = 0.05 l Conversion from millimolar to molar: 25 m M = 0.025 M Converting moles to mass: Answer to Problem 4: 0.14875 g of KBr needs to be dissolved in 50 ml of water to form a 50 ml 25 m M aqueous solution of KBr.

How much KBr (in grams) is needed to form 50 ml of 25 m M aqueous solution of KBr? We were given the volume of solvent and the concentration of the solution. We weren’t provided the molecular weight of KBr so we will need to consult a periodic table to determine its molecular weight by using the sum of the atomic weights of K and Br (works out as 119.0 g/mol). Attempt to do all four problems on your own and check your answers.

Now that we know both the number of moles of miconazole and its molecular weight, we can now use the formula above to determine the mass of miconazole used to form the 0.001 M solution. “A trainee prepared a solution of cis-(−)-carveol (152.24 g/mol), a component of spearmint oil, for polarimetry studies.

Given that 2200 mg of cis-(−)-carveol was dissolved in 20 ml of solvent to form the aforementioned solution, express the concentration of the solution prepared by the trainee in molarity (M).” Step 1: Determine which formula(s) to use.

The solute (perhaps a salt) is added to the flask first and then water is added until the solution reaches the mark.

The flasks have very good calibration so volumes are commonly known to at least four significant figures. Notice that you are given two concentrations, but only one volume.

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