Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 33

What mass of \(\mathrm{NaOH}\) is contained in \(250.0 \mathrm{~mL}\) of a \(0.400 \mathrm{M}\) sodium hydroxide solution?

Short Answer

Expert verified
The mass of \(\mathrm{NaOH}\) contained in \(250.0 \mathrm{~mL}\) of a \(0.400\mathrm{M}\) sodium hydroxide solution is 4.00 g.

Step by step solution

01

Convert mL of solution to L

To convert from mL to L, we'll divide the volume of the solution (250.0 mL) by 1000 since there are 1000 mL in 1 L: Volume in L = 250.0 mL ÷ 1000 = 0.250 L
02

Calculate the number of moles of NaOH

To find the number of moles of NaOH, we'll multiply the volume of the solution (in L) by the given concentration: Number of moles of NaOH = (volume of solution in L) × (concentration) Number of moles of NaOH = (0.250 L) × (0.400 mol/L) = 0.100 mol
03

Find the molar mass of NaOH

To calculate the mass of NaOH, we need the molar mass of the solute. The formula for sodium hydroxide is NaOH, and we can find the molar mass using the periodic table: Molar mass of Na (sodium) = 22.99 g/mol Molar mass of O (oxygen) = 16.00 g/mol Molar mass of H (hydrogen) = 1.008 g/mol Molar mass of NaOH = (22.99 + 16.00 + 1.008) g/mol = 40.00 g/mol
04

Calculate the mass of NaOH

Now we can calculate the mass of NaOH by multiplying the number of moles with the molar mass: mass of NaOH = (number of moles of NaOH) × (molar mass of NaOH) mass of NaOH = (0.100 mol) × (40.00 g/mol) = 4.00 g The mass of \(\mathrm{NaOH}\) contained in \(250.0 \mathrm{~mL}\) of a \(0.400\mathrm{M}\) sodium hydroxide solution is 4.00 g.

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

The soda you are drinking contains \(0.5 \%\) by mass sodium benzoate as a preservative. What approximate mass of sodium benzoate is contained in \(1.00 \mathrm{~L}\) of the solution assuming that the density of the soda is \(1.00 \mathrm{~g} / \mathrm{mL}\) (the approximate density of water)?

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \overline{\mathrm{SO}}_{4}\). A \(0.205-\mathrm{g}\) sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The \(\mathrm{BaSO}_{4}\) that is formed is filtered, dried, and weighed. Its mass is \(0.298 \mathrm{~g}\). What mass of \(\mathrm{SO}_{4}{ }^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}{ }^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

Show how each of the following strong electrolytes "breaks up" into its component ions upon dissolving in water by drawing molecular-level pictures. a. \(\mathrm{NaBr}\) f. \(\mathrm{FeSO}_{4}\) b. \(\mathrm{MgCl}_{2}\) g. \(\mathrm{KMnO}_{4}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) h. \(\mathrm{HClO}_{4}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) i. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (ammonium acetate) e. \(\mathrm{NaOH}\)

What volume of each of the following bases will react completely with \(25.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\) ? a. \(0.100 \mathrm{M} \mathrm{NaOH}\) b. \(0.0500 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) c. \(0.250 \mathrm{M} \mathrm{KOH}\)

Many oxidation-reduction reactions can be balanced by inspection. Try to balance the following reactions by inspection. In each reaction, identify the substance reduced and the substance oxidized. a. \(\mathrm{Al}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{CH}_{4}(g)+\mathrm{S}(s) \rightarrow \mathrm{CS}_{2}(l)+\mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})\) c. \(\mathrm{C}_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{Cu}(s)+\mathrm{Ag}^{+}(a q) \rightarrow \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

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