Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 12

What mass of sodium oxalate \(\left(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) is needed to prepare \(0.250 \mathrm{L}\) of a \(0.100-M\) solution?

Short Answer

Expert verified
To find the mass of sodium oxalate needed, first calculate the moles of solute: Moles of solute = \(0.100 \mathrm{M} × 0.250 \mathrm{L}\) = \(0.025 \mathrm{mol}\).

Step by step solution

01

Find the number of moles required

Use the formula for molarity: Moles of solute = Molarity × Volume of solution Here, the molarity of the solution is \(0.100\) M and the volume of the solution is \(0.250\) L. Calculate the moles of sodium oxalate: Moles of solute = \(0.100 \mathrm{M} × 0.250 \mathrm{L}\)

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

In the winter of \(1994,\) record low temperatures were registered throughout the United States. For example, in Champaign, Illinois, a record low of \(-29^{\circ} \mathrm{F}\) was registered. At this temperature can salting icy roads with \(\mathrm{CaCl}_{2}\) be effective in melting the ice? a. Assume \(i=3.00\) for \(\mathrm{CaCl}_{2}\) b. Assume the average value of \(i\) from Exercise 87 (The solubility of \(\mathrm{CaCl}_{2}\) in cold water is \(74.5 \mathrm{g}\) per \(100.0 \mathrm{g}\) water.

Calculate the sodium ion concentration when \(70.0 \mathrm{mL}\) of 3.0 \(M\) sodium carbonate is added to \(30.0 \mathrm{mL}\) of \(1.0 \mathrm{M}\) sodium bicarbonate.

A solid mixture contains \(\mathrm{MgCl}_{2}\) and \(\mathrm{NaCl}\). When \(0.5000 \mathrm{g}\) of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at \(25.0^{\circ} \mathrm{C}\) is observed to be 0.3950 atm. What is the mass percent of \(\mathrm{MgCl}_{2}\) in the solid? (Assume ideal behavior for the solution.)

What mass of glycerin \(\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3}\right),\) a nonelectrolyte, must be dissolved in \(200.0 \mathrm{g}\) water to give a solution with a freezing point of \(-1.50^{\circ} \mathrm{C} ?\)

Rubbing alcohol contains 585 g isopropanol \(\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\right)\) per liter (aqueous solution). Calculate the molarity.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

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