Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 27

Calculate the molarity of each of these solutions. a. A 5.623-g sample of \(\mathrm{NaHCO}_{3}\) is dissolved in enough water to make \(250.0 \mathrm{~mL}\) of solution. b. A \(184.6-\mathrm{mg}\) sample of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) is dissolved in enough water to make \(500.0 \mathrm{~mL}\) of solution. c. A \(0.1025-\mathrm{g}\) sample of copper metal is dissolved in \(35 \mathrm{~mL}\) of concentrated \(\mathrm{HNO}_{3}\) to form \(\mathrm{Cu}^{2+}\) ions and then water is added to make a total volume of \(200.0 \mathrm{~mL}\). (Calculate the molarity of \(\mathrm{Cu}^{2+}\).)

Short Answer

Expert verified
The molarities of the solutions are as follows: a. \(0.26776\text{ M}\) for the NaHCO3 solution b. \(0.001255\text{ M}\) for the K2Cr2O7 solution c. \(0.00807\text{ M}\) for the Cu²⁺ ions in solution

Step by step solution

01

Find the moles of NaHCO3

First, we need to find the molar mass of NaHCO3. Molar mass of NaHCO3 = 22.99(g/mol for Na) + 1.01(g/mol for H) + 12.01(g/mol for C) + 3 * 16.00(g/mol for O) = 84.01 g/mol Now, we'll find the moles of NaHCO3 by dividing the mass by the molar mass: moles of NaHCO3 = 5.623 g / 84.01 g/mol = 0.06694 mol
02

Convert volume to liters

We need to convert the volume of the solution from mL to L: 250 mL = 250/1000 = 0.250 L
03

Calculate molarity

Now we can find the molarity using the formula: Molarity (M) = moles of solute / volume of solution in L Molarity (M) = 0.06694 mol / 0.250 L = 0.26776 M #b. Finding the molarity of K2Cr2O7 solution#
04

Find the moles of K2Cr2O7

First, find the molar mass of K2Cr2O7. Molar mass of K2Cr2O7 = 2 * 39.10(g/mol for K) + 2 * 51.996(g/mol for Cr) + 7 * 16.00(g/mol for O) = 294.18 g/mol Next, convert the mass from mg to g: 184.6 mg = 184.6 / 1000 = 0.1846 g Now, find the moles of K2Cr2O7 by dividing the mass by the molar mass: moles of K2Cr2O7 = 0.1846 g / 294.18 g/mol = 0.0006274 mol
05

Convert volume to liters

We need to convert the volume of the solution from mL to L: 500 mL = 500/1000 = 0.500 L
06

Calculate molarity

Now we can find the molarity using the formula: Molarity (M) = moles of solute / volume of solution in L Molarity (M) = 0.0006274 mol / 0.500 L = 0.001255 M #c. Finding the molarity of Cu²⁺ ions in solution#
07

Find the moles of Cu

First, find the molar mass of Cu. Molar mass of Cu = 63.546 g/mol Now, find the moles of Cu by dividing the mass by the molar mass: moles of Cu = 0.1025 g / 63.546 g/mol = 0.001614 mol
08

Convert volume to liters

We need to convert the total volume of the solution from mL to L: 200 mL = 200/1000 = 0.200 L
09

Calculate molarity

Now we can find the molarity using the formula: Molarity (M) = moles of solute / volume of solution in L Molarity (M) = 0.001614 mol / 0.200 L = 0.00807 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

If \(10 . \mathrm{g}\) of \(\mathrm{AgNO}_{3}\) is available, what volume of \(0.25 \mathrm{MAgNO}_{3}\) solution can be prepared?

What mass of solid aluminum hydroxide can be produced when \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) is added to \(200.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{KOH} ?\)

Saccharin \(\left(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S}\right)\) is sometimes dispensed in tablet form. Ten tablets with a total mass of \(0.5894 \mathrm{~g}\) were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of \(\mathrm{BaSO}_{4}\) obtained was \(0.5032 \mathrm{~g}\). What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?

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. \(0.0500 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\) c. \(0.250 \mathrm{M} \mathrm{KOH}\)

A stock solution containing \(\mathrm{Mn}^{2+}\) ions was prepared by dissolving \(1.584\) g pure manganese metal in nitric acid and diluting to a final volume of \(1.000 \mathrm{~L}\). The following solutions were then prepared by dilution: For solution \(A, 50.00 \mathrm{~mL}\) of stock solution was diluted to \(1000.0 \mathrm{~mL}\). For solution \(B, 10.00 \mathrm{~mL}\) of solution \(A\) was diluted to \(250.0 \mathrm{~mL}\). For solution \(C, 10.00 \mathrm{~mL}\) of solution \(B\) was diluted to \(500.0 \mathrm{~mL}\). Calculate the concentrations of the stock solution and solutions \(A, B\), and \(C .\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

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