Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 64

Water is added to \(25.0 \mathrm{~mL}\) of a \(0.866 \mathrm{M} \mathrm{KNO}_{3}\) solution until the volume of the solution is exactly \(500 \mathrm{~mL}\). What is the concentration of the final solution?

Short Answer

Expert verified
The concentration of the final solution is \(0.0433 \mathrm{M}\).

Step by step solution

01

Determine Given Values

Identify the known values given in the exercise. The initial volume (V1) is \(25.0 \mathrm{~mL}\), the initial molarity (M1) is \(0.866 \mathrm{M}\), and the final volume (V2) is \(500 \mathrm{~mL}\). The final molarity (M2) is what we are trying to find.
02

Convert volumes to same units

Here the volumes are already in the same units (\(mL\)), so no conversion is necessary.
03

Apply the Dilution Formula

Use the dilution formula \(M1V1 = M2V2\) to solve for the final molarity (M2). Substituting the numbers from step 1 gives us \(0.866 \mathrm{M} * 25.0 \mathrm{~mL} = M2 * 500 \mathrm{~mL}\).
04

Calculate the Final Molarity

Solving the equation from Step 3 for M2 gives us \(M2 = (0.866 \mathrm{M} * 25.0 \mathrm{~mL}) / 500 \mathrm{~mL}\). This simplifies to \(M2 = 0.0433 \mathrm{M}\). Therefore, the final concentration of the solution is \(0.0433 \mathrm{M}\).

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

Distilled water must be used in the gravimetric analysis of chlorides. Why?

The concentration of \(\mathrm{Cu}^{2+}\) ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide \(\left(\mathrm{Na}_{2} \mathrm{~S}\right)\) solution to \(0.800 \mathrm{~L}\) of the water. The molecular equation is $$ \mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{CuSO}_{4}(a q) \longrightarrow_{\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\operatorname{CuS}(s)} $$ Write the net ionic equation and calculate the molar concentration of \(\mathrm{Cu}^{2+}\) in the water sample if \(0.0177 \mathrm{~g}\) of solid \(\mathrm{CuS}\) is formed.

A 5.012 -g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was \(3.195 \mathrm{~g}\). The compound was dissolved in water and reacted with an excess of \(\mathrm{AgNO}_{3}\). The precipitae of \(\mathrm{AgCl}\) formed weighed \(7.225 \mathrm{~g}\). What is the formula of the original compound?

For the complete redox reactions given here, (i) break down each reaction into its half-reactions; (ii) identify the oxidizing agent; (iii) identify the reducing agent. (a) \(2 \mathrm{Sr}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{SrO}\) (b) \(2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}\) (c) \(2 \mathrm{Cs}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{CsBr}\) (d) \(3 \mathrm{Mg}+\mathrm{N}_{2} \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}\)

Give Arrhenius's and Bronsted's definitions of an acid and a base. Why are Bronsted's definitions more useful in describing acid-base properties?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic 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