Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 1: Problem 41

Calculate the molarity of a solution obtained by mixing \(250 \mathrm{ml}\) of \(0.5 \mathrm{M}\) HCl with \(750 \mathrm{ml}\) of \(2 \mathrm{M}\) HCl. (a) \(1.8\) (b) \(2.0\) (c) \(1.6\) (d) \(0.8\)

Short Answer

Expert verified
(a) 0.5 (b) 1.0 (c) 1.6 (d) 2.0 Answer: (c) 1.6

Step by step solution

01

Write down the given information

We know the initial molarities and volumes of the two HCl solutions: \(M_1\) = \(0.5\mathrm{M}\) \(V_1\) = \(250\mathrm{ml}\) \(M_2\) = \(2\mathrm{M}\) \(V_2\) = \(750\mathrm{ml}\)
02

Calculate the final volume

Sum the initial volumes to find the final volume: \(V_f = V_1 + V_2 = 250\mathrm{ml} + 750\mathrm{ml}\) \(V_f = 1000\mathrm{ml}\)
03

Use the formula to find the final molarity

Plug the initial molarities and volumes, along with the final volume, into the formula: \(M_1V_1 + M_2V_2 = M_fV_f\) \((0.5\mathrm{M})(250\mathrm{ml}) + (2\mathrm{M})(750\mathrm{ml}) = M_f(1000\mathrm{ml})\)
04

Solve for the final molarity

Divide both sides of the equation by 1000 ml to solve for the final molarity: \(M_f = \frac{(0.5\mathrm{M})(250\mathrm{ml}) + (2\mathrm{M})(750\mathrm{ml})}{1000\mathrm{ml}}\) \(M_f = \frac{125\mathrm{mmol} + 1500\mathrm{mmol}}{1000\mathrm{ml}}\) \(M_f = \frac{1625\mathrm{mmol}}{1000\mathrm{ml}}\) \(M_f = 1.625\mathrm{M}\) Since the nearest answer provided is 1.6, the correct response is (c) 1.6.

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

Select the correct alternative from the given choices. The ratio by mass of sulphur and oxygen in \(\mathrm{SO}_{2}\) is (a) \(1: 2\) (b) \(2: 1\) (c) \(1: 1\) (d) \(1: 4\)

Empirical formula of a compound is \(\mathrm{A}_{2} \mathrm{~B}_{4} .\) If its empirical formula weight is half of its vapour density, determine the molecular formula of the compound. (a) \(\mathrm{A}_{4} \mathrm{~B}_{8}\) (b) \(\mathrm{A}_{8} \mathrm{~B}_{16}\) (c) \(\mathrm{A}_{2} \mathrm{~B}_{4}\) (d) \(\mathrm{A}_{3} \mathrm{~B}_{6}\)

Dalton's law of partial pressures cannot hold good for (a) \(\mathrm{NO}_{2}+\mathrm{O}_{2}\) (b) \(\mathrm{H}_{2}+\mathrm{Cl}_{2}\) (c) \(\mathrm{CO}_{2}+\mathrm{O}_{2}\) (d) \(\mathrm{NH}_{3}+\mathrm{He}\)

Select the correct alternative from the given choices. When \(180 \mathrm{~g}\) of glucose is subjected to combustion, the volume of \(\mathrm{CO}_{2}\) liberated at \(\mathrm{STP}\) is (a) \(22.4 \ell\) (b) \(67.2\) \ell (c) \(44 \ell\) (d) \(134.4 \ell\)

\(0.5\) moles of a salt contains "3N" oxygen atoms. Identify the formula of the salt. (a) \(\mathrm{MXO}_{3}\) (b) \(\mathrm{MX}_{2} \mathrm{O}_{3}\) (c) \(\mathrm{M}_{2} \mathrm{XO}_{3}\) (d) \(\mathrm{M}\left(\mathrm{XO}_{3}\right)_{2}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

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