A solution is prepared with 5.0 g of HCl and 195.0 g of H2 O. The HCl solution has a density o

A solution is prepared with 5.0 g of HCl and 195.0 g of H2...

A solution is prepared with $5.0 \mathrm{~g}$ of $\mathrm{HCl}$ and $195.0 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$. The HCl solution has a density of $1.49 \mathrm{~g} / \mathrm{mL}$. (9.4) a. What is the mass percent $(\mathrm{m} / \mathrm{m})$ of the $\mathrm{HCl}$ solution? b. What is the total volume, in milliliters, of the solution? c. What is the mass/volume percent (m/v) of the solution? d. What is the molarity of the solution?

A solution is prepared with $5.0 \mathrm{~g}$ of $\mathrm{HCl}$ and $195.0 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$. The HCl solution has a density of $1.49 \mathrm{~g} / \mathrm{mL}$. (9.4)
a. What is the mass percent $(\mathrm{m} / \mathrm{m})$ of the $\mathrm{HCl}$ solution?
b. What is the total volume, in milliliters, of the solution?
c. What is the mass/volume percent (m/v) of the solution?
d. What is the molarity of the solution?

Key Concepts

Molarity

Molarity is a concentration unit defined as the number of moles of solute per liter of solution. It is one of the most common ways to express how much of a substance is present in a given volume of solution, and it is essential for stoichiometric calculations in chemical reactions.

Mole Calculation

Mole calculation involves converting the mass of a substance to the number of moles using its molar mass. This process is fundamental in chemistry for relating mass-based measurements to the actual number of particles, which is necessary for determining molarity and balancing chemical equations.

Density

Density is the ratio of mass to volume for a substance, usually expressed in units such as grams per milliliter (g/mL). It is a critical concept in solutions chemistry, as it allows one to convert between mass and volume in order to calculate concentrations and prepare solutions accurately.

Mass Percent Concentration

Mass percent concentration is a way to express the concentration of a solution by comparing the mass of the solute to the total mass of the solution, then multiplying by 100. It provides a direct measure of the ratio between the solute and the entire solution, making it useful in various analytical and preparative techniques.

Mass/Volume Percent Concentration

Mass/volume percent concentration describes the mass of the solute present in 100 mL of solution. This measurement is especially useful in experimental settings where volumetric measurements are easier to perform, allowing for quick assessments of solution strength.

Transcript

00:01 This question contains multiple calculations in reference to a single solution.

00:07 The solution that is prepared contains 5 grams of hcl and 195 grams of h2o.

00:17 The density of this solution is 1 .49 grams per milliliter.

00:25 The first question is what is the mass percent, mass solute per mass solution, of the mass percent? hcl.

00:40 To calculate the mass percent, we'll take the mass of the solute, hcl, and divide it by the total mass of the solution, not just the mass of the water, the total mass of the solution.

00:54 So it'll be the 5 grams hcl plus the 195 grams of water giving us 200 grams of solution.

01:03 We multiply that because we want a percentage by 100 and we get 2 .5 percent mass, hcl.

01:15 The next part of this question asks you to determine the total volume in milliliters of the solution.

01:23 Well, we weren't given any information associated with milliliters, just mass and a density, but we should be able to use the density to convert the mass into a volume as these are the units of density.

01:38 So let's start with the total mass.

01:40 The total mass of the solution is five, plus 195 or 200 grams.

01:47 Density showing us the relationship between mass and volume of the solution can be used as a conversion factor.

01:56 For every 1 .49 grams of the solution, there is 1 milliliter of the solution.

02:01 So we divide 1 .49 into 200, and we get 134 milliliters of solution...

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