Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 4: Problem 11

You have two solutions of chemical \(\mathrm{A}\). To determine which has the highest concentration of A (molarity), which of the following must you know (there may be more than one answer)? a. the mass in grams of A in each solution b. the molar mass of \(\mathrm{A}\) c. the volume of water added to each solution d. the total volume of the solution Explain.

Short Answer

Expert verified
To determine which solution has the highest concentration of chemical A, we need to know the mass in grams of A in each solution (a), the molar mass of A (b), and the total volume of the solution (d). Option c, the volume of water added to each solution, is not required for determining the concentration.

Step by step solution

01

Understand the components of molarity

Molarity is calculated by dividing the moles of solute (chemical A) by the volume of the solution in liters. In this case, we need to identify which information from options a, b, c, and d helps us find the moles of solute, and the volume of the solution.
02

Option a: Mass of A in each solution

The mass of chemical A in each solution can be used to determine the moles present in each solution by dividing the mass (grams) by the molar mass (grams/mole). This information is essential to finding the molarity and concentration of each solution.
03

Option b: Molar mass of A

The molar mass of A is necessary to convert mass (grams) of solute to moles. Without the molar mass, we won't be able to find the number of moles of chemical A in each solution. So, knowing the molar mass of A is important for determining the concentration of the solutions.
04

Option c: Volume of water added

The volume of water added to each solution is not enough information to determine the total volume of the solution. It would be helpful if we knew the initial volume of the solution before water was added, but this information alone does not provide the total volume of the solution.
05

Option d: Total volume of the solution

The total volume of each solution is necessary for calculating the concentration of chemical A therein because the molarity (concentration) is expressed in terms of moles of solute per liter of solution. Knowing the total volume of the solution helps us to find the molarity.
06

Conclusion

To determine which solution has the highest concentration of chemical A, we need the following information: a. the mass in grams of A in each solution b. the molar mass of A d. the total volume of the solution. Option c is not required.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Concentration of Solutions
Understanding the concentration of solutions is key to mastering chemistry. In simple terms, the concentration of a solution tells us how much solute is present in a given quantity of solvent. The most common way to express concentration is molarity, symbolized by M, which is the number of moles of solute per liter of solution.

Molarity can be calculated using the formula: \[ M = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \].

To find the molarity, you need two critical pieces of information: the quantity of solute, which is typically measured in moles, and the volume of the solution in liters. In the context of our exercise, we're looking at two solutions of chemical A and trying to determine which has the higher concentration. Knowing the mass of A in each solution (option a) and the total volume of the solution (option d) allows you to use the molarity formula to find the concentration and compare the two solutions accurately.

Remember, just knowing how much water was added to a solution (option c) is not enough, as it doesn't account for the initial volume or any other components in the solution.
Molar Mass
Molar mass is a fundamental concept that bridges the gap between the mass of a substance and the number of moles present. It is defined as the mass of one mole of a substance, typically expressed in grams per mole (g/mol). The molar mass of a substance is calculated by adding up the atomic masses of all the atoms in one molecule of the substance.

When dealing with solutions, molar mass becomes essential, as it allows us to convert a given mass of solute into moles—crucial for calculating molarity. For chemical A in our exercise, knowing the molar mass (option b) is compulsory because you need it to convert the mass of A from grams to moles using the formula: \[ \text{moles of solute} = \frac{\text{mass in grams}}{\text{molar mass}} \].

Without the molar mass, the mass of the solute itself doesn't give us a meaningful value for calculating concentration, as we cannot translate it into the moles needed for the molarity equation.
Moles of Solute
Moles of solute are a measurement of the quantity of the substance that has been dissolved in a solution. One mole corresponds to Avogadro's number, approximately \(6.022 \times 10^{23}\) particles of the substance, be it atoms, molecules, ions, or electrons.

In the context of our exercise and the concept of molarity, the moles of solute interact directly with the volume of the solution to determine concentration. By knowing the mass of the chemical A in grams (option a) and using its molar mass (option b), you can calculate the moles of solute present.

With the moles of solute and the total volume of the solution (option d), you now have the two vital components needed to calculate molarity, letting you compare the concentration of chemical A in both solutions effectively.

Always remember to ensure your volume is in liters and your mass is in grams before performing your calculations to get accurate molarity readings.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

An average human being has about \(5.0 \mathrm{~L}\) of blood in his or her body. If an average person were to eat \(32.0 \mathrm{~g}\) of sugar (sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}, 342.30 \mathrm{~g} / \mathrm{mol}\) ), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?

A solution is prepared by dissolving \(0.6706 \mathrm{~g}\) oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make \(100.0 \mathrm{~mL}\) of solution. \(\mathrm{A}\) \(10.00-\mathrm{mL}\) aliquot (portion) of this solution is then diluted to a final volume of \(250.0 \mathrm{~mL}\). What is the final molarity of the oxalic acid solution?

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{aligned} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) & \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) & \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{aligned} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{~mL}\) of \(3.00 \mathrm{M}\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{~mL}\) of \(\mathrm{HCl}\) was added, what was the concentration of the \(\mathrm{HCl} ?\)

The vanadium in a sample of ore is converted to \(\mathrm{VO}^{2+}\). The \(\mathrm{VO}^{2+}\) ion is subsequently titrated with \(\mathrm{MnO}_{4}^{-}\) in acidic solution to form \(\mathrm{V}(\mathrm{OH})_{4}{ }^{+}\) and manganese(II) ion. The unbalanced titration reaction is \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{VO}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(t) \longrightarrow\) \(\mathrm{V}(\mathrm{OH})_{4}^{+}(a q)+\mathrm{Mn}^{2+}(a q)+\mathrm{H}^{+}(a q)\) To titrate the solution, \(26.45 \mathrm{~mL}\) of \(0.02250 \mathrm{M} \mathrm{MnO}_{4}^{-}\) was required. If the mass percent of vanadium in the ore was \(58.1 \%\), what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.

The blood alcohol \(\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}\right)\) level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of \(\mathrm{Cr}^{3+}(a q)\) and carbon dioxide. The reaction can be monitored because the dichromate ion \(\left(\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}\right)\) is orange in solution, and the \(\mathrm{Cr}^{3+}\) ion is green. The balanced equation is \(16 \mathrm{H}^{+}(a q)+2 \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}(a q) \longrightarrow\) \(4 \mathrm{Cr}^{3+}(a q)+2 \mathrm{CO}_{2}(g)+11 \mathrm{H}_{2} \mathrm{O}(t)\) This reaction is an oxidation-reduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free