Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 90

Concentrated hydrochloric acid is usually available at 37.7 percent by mass. What is its concentration in molarity? (The density of the solution is \(1.19 \mathrm{~g} / \mathrm{mL}\).)

Short Answer

Expert verified
The concentration of the hydrochloric acid solution is approximately 12.29 M.

Step by step solution

01

Calculate the mass of the solute (hydrochloric acid) in 1000 g of the solution

Since the hydrochloric acid is 37.7% by mass, this means that in 1000 g of the solution, there is \(37.7\% \times 1000 = 377\) g of hydrochloric acid.
02

Convert the mass of the hydrochloric acid to moles

The molar mass of hydrochloric acid (HCl) is approximately 36.5 g/mol. So, \( \frac{377}{36.5} = 10.33\) moles.
03

Calculate the volume of the solution in liters

The density is given as 1.19 g/mL. Therefore, the volume of 1000 g of the solution is \( \frac{1000}{1.19} = 840.34\) mL or 0.84034 L.
04

Calculate the concentration in molarity

Molarity is defined as the number of moles of solute per liter of solution. In this case, it's \( \frac{10.33}{0.84034} = 12.29 \) M.

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!

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

Define Raoult's law. Define each term in the equation representing Raoult's law, and give its units. What is an ideal solution?

Solutions \(A\) and \(B\) containing the same solute have osmotic pressures of 2.4 atm and 4.6 atm, respectively, at a certain temperature. What is the osmotic pressure of a solution prepared by mixing equal volumes of \(\mathrm{A}\) and \(\mathrm{B}\) at the same temperature?

A protein has been isolated as a salt with the formula \(\mathrm{Na}_{20} \mathrm{P}\) (this notation means that there are \(20 \mathrm{Na}^{+}\) ions associated with a negatively charged protein \(\mathrm{P}^{20-}\) ). The osmotic pressure of a 10.0 -mL solution containing \(0.225 \mathrm{~g}\) of the protein is \(0.257 \mathrm{~atm}\) at \(25.0^{\circ} \mathrm{C}\). (a) Calculate the molar mass of the protein from these data. (b) What is the actual molar mass of the protein?

What is the osmotic pressure (in atmospheres) of a \(12.36 M\) aqueous urea solution at \(22.0^{\circ} \mathrm{C} ?\)

Calculate the percent by mass of the solute in each of these aqueous solutions: (a) \(5.50 \mathrm{~g}\) of \(\mathrm{NaBr}\) in \(78.2 \mathrm{~g}\) of solution, (b) \(31.0 \mathrm{~g}\) of \(\mathrm{KCl}\) in \(152 \mathrm{~g}\) of water, \((\mathrm{c})\) \(4.5 \mathrm{~g}\) of toluene in \(29 \mathrm{~g}\) of benzene.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

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