Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 102

The number of moles of hydroxide ion in 0.300 L of \(0.0050 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) is (a) \(0.0015 ;(\mathrm{b}) 0.0030 ;(\mathrm{c}) 0.0050\) (d) 0.010.

Short Answer

Expert verified
So, the number of moles of hydroxide ion in 0.300 L of 0.0050 M Ba(OH)2 solution is 0.0030 moles (option b).

Step by step solution

01

Identifying the given variables

In our problem, the concentration [C] of barium hydroxide is 0.0050 M and the volume [V] given is 0.300L.
02

Formulate the relationship

Ba(OH)2 \[ \rightarrow \] Ba2+ + 2OH-, from one formula unit of Ba(OH)2 we get 2 hydroxide ions. Thus, the concentration of hydroxide ions is twice the concentration of the barium hydroxide.
03

Calculate the moles of Ba(OH)2

To calculate the moles (n) of Ba(OH)2, use the formula n = C x V. Substituting the given values, number of moles of Ba(OH)2 = 0.0050 M x 0.300L = 0.0015 moles.
04

Resolve for the concentration of OH⁻

Since each mole of Ba(OH)2 produces 2 moles of OH⁻, the number of moles of OH⁻ will be 2 times the moles of Ba(OH)2. The moles of OH⁻ is therefore = 2 x 0.0015 moles = 0.0030 moles.

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

Complete and balance these half-equations. (a) \(\mathrm{SO}_{3}^{2-} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) (acidic solution) (b) \(\mathrm{HNO}_{3} \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})\) (acidic solution) (c) \(\mathrm{Al}(\mathrm{s}) \longrightarrow \mathrm{Al}(\mathrm{OH})_{4}^{-}\) (basic solution) Indicate whether oxidation or reduction is involved.

A method of producing phosphine, \(\mathrm{PH}_{3}\), from elemental phosphorus, \(P_{4}\), involves heating the \(P_{4}\) with \(\mathrm{H}_{2} \mathrm{O} .\) An additional product is phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\) Write a balanced equation for this reaction.

A \(25.00 \mathrm{mL}\) sample of \(0.132 \mathrm{M}\) \(\mathrm{HNO}_{3}\) is mixed with \(10.00 \mathrm{mL}\) of \(0.318 \mathrm{M} \mathrm{KOH} .\) Is the resulting solution acidic, basic, or exactly neutralized?

Complete and balance these half-equations. (a) \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-} \longrightarrow \mathrm{CO}_{2}\) (acidic solution) (b) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \longrightarrow \mathrm{Cr}^{3+}\) (acidic solution) (c) \(\mathrm{MnO}_{4}^{-} \longrightarrow \mathrm{MnO}_{2}\) (basic solution) Indicate whether oxidation or reduction is involved.

A sample of battery acid is to be analyzed for its sulfuric acid content. A \(1.00 \mathrm{mL}\) sample weighs \(1.239 \mathrm{g}\). This \(1.00 \mathrm{mL}\) sample is diluted to \(250.0 \mathrm{mL}\), and \(10.00 \mathrm{mL}\) of this diluted acid requires \(32.44 \mathrm{mL}\) of \(0.00498 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) for its titration. What is the mass percent of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in the battery acid? (Assume that complete ionization and neutralization of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) occurs.)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Organic 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