What mass of the indicated solute does each of the following...

What mass of the indicated solute does each of the following solutions contain? a. $2.50 \mathrm{L}$ of $13.1$ $M$ $\mathrm{HCl}$l solution b. $15.6 \mathrm{mL}$ of $0.155$ $M$ $\mathrm{NaOH}$ solution c. $135 \mathrm{mL}$ of $2.01$ $M$ $\mathrm{HNO}_{3}$ solution d. $4.21 \mathrm{L}$ of $0.515$ $M$ $\mathrm{CaCl}_{2}$ solution

What mass of the indicated solute does each of the following solutions contain?
a. $2.50 \mathrm{L}$ of $13.1$ $M$ $\mathrm{HCl}$l solution
b. $15.6 \mathrm{mL}$ of $0.155$ $M$ $\mathrm{NaOH}$ solution
c. $135 \mathrm{mL}$ of $2.01$ $M$ $\mathrm{HNO}_{3}$ solution
d. $4.21 \mathrm{L}$ of $0.515$ $M$ $\mathrm{CaCl}_{2}$ solution

Key Concepts

Molarity

Molarity is a measure of the concentration of a solution expressed as the number of moles of solute per liter of solution. It is a central concept for relating the volume of a solution to the quantity of solute present, which is essential for calculating how much of a solute is contained in a given volume.

Volume Conversion

Volume conversion, particularly converting milliliters to liters, is an important step because molarity is defined in terms of liters. Accurate conversion ensures correct calculation of the moles of solute in the solution.

Calculation of Moles

Calculating the number of moles of a solute involves multiplying the molarity of the solution by its volume in liters. This step converts the concentration information into an absolute amount of substance, which can then be used to determine mass.

Molar Mass and Mass Calculation

Molar mass is the mass of one mole of a substance and is used to convert the number of moles into a mass value, typically in grams. By multiplying the number of moles by the molar mass, one obtains the mass of the solute present in the solution.

Transcript

00:01 So we are asked to find the mass of each solute in the given solution.

00:07 So i've written now what we are given for a, b, c, and d.

00:12 So let's start with a.

00:14 We have 2 .50 liters of 13 .1 molar hcl solution.

00:22 So we have volume, which is here, 2 .5, and we have concentration, which is 13 .1 molars.

00:30 So we can find the number of moles.

00:33 So moles is equal to concentration times volume.

00:38 So i can plug in what we have.

00:41 We have 13 .1 molars and 2 .5 liters.

00:54 And that gives us 32 .75 moles.

01:06 Now we're not looking for moles.

01:08 We're looking for mass, but we can use this moles to find the mass, since we can also find the molar mass of hcl using the periodic table.

01:18 So the mass is equal to the molar mass of hcl times the number of moles.

01:26 So the molar mass of hcl will be the molar mass of hydrogen, which is 1 .01 grams per mole, plus the mass of chlorine.

01:38 That calculation and that equals 36 .46 grams per mole.

01:58 Multiply by the moles we just found, which is 32 .75 moles.

02:14 And that answer, this calculation gives us the answer of 1 ,190 after we round to three significant digits.

02:25 Since there's three significant digits in the question, which is the lowest number.

02:32 So that gives us 1 ,190 grams of hcl.

02:43 For b, we can do the same thing, but our volume is given to us in milliliters.

02:51 So i'm going to convert that to liters, since this equation we use n equals c times v.

03:00 Uses liters.

03:02 So 15 .6 milliliters is equal to 0 .0156 liters since we divided this 15 .6 by a thousand, since there are 1 ,000 mill liters in one liter.

03:22 So now that we have our units straightened out, we can use n equals c times v to find the number of moles.

03:31 So n, equals concentration, which is 0 .015, sorry, 0 .15 molars is our concentration, and 0 .0156 liters.

04:00 And that gives us 0 .002 for.

04:14 1 -8 moles...

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