/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 99 Calculate the volume of a \(0.15... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 99

Calculate the volume of a \(0.156 \mathrm{M} \mathrm{CuSO}_{4}\) solution that would react with \(7.89 \mathrm{~g}\) of zinc.

Short Answer

Expert verified
773 mL of the 0.156 M CuSO4 solution is needed.

Step by step solution

01

Write the Balanced Chemical Equation

First, identify the chemical reaction between zinc (Zn) and copper(II) sulfate (\( ext{CuSO}_4 \). This is a single displacement reaction and can be written as:\[ ext{Zn} + ext{CuSO}_{4} \rightarrow ext{ZnSO}_{4} + ext{Cu}\]This equation is balanced as written; one atom of Zn reacts with one molecule of \(\text{CuSO}_4\).
02

Calculate Moles of Zinc

Next, convert the mass of zinc to moles using its molar mass. The molar mass of Zn is approximately 65.38 g/mol.\(\text{Moles of Zn} = \frac{7.89 \, \text{g}}{65.38 \, \text{g/mol}} \approx 0.1207 \, \text{moles}\)
03

Determine Moles of CuSO4 Required

From the balanced equation, 1 mole of Zn reacts with 1 mole of \(\text{CuSO}_4\). Therefore, 0.1207 moles of Zn will require 0.1207 moles of \(\text{CuSO}_4\).
04

Calculate Volume of CuSO4 Solution

Now, use the concentration of the \(\text{CuSO}_4\) solution to find the required volume. The concentration is given as 0.156 M, which means 0.156 moles per liter.Using the formula\[\text{Volume} = \frac{\text{Moles of } \text{CuSO}_4}{\text{Concentration}} = \frac{0.1207 \, \text{moles}}{0.156 \, \text{M}} \approx 0.773 \, \text{liters}\]
05

Final Step: Convert to Milliliters

Finally, convert the volume from liters to milliliters:\(0.773 \, \text{liters} \times 1000 \, \frac{\text{mL}}{\text{liter}} = 773 \, \text{mL}\)

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molar Concentration
Molar concentration describes the number of moles of a solute in one liter of solution. It is expressed in moles per liter (mol/L) or simply as M for molarity. Understanding molarity is essential for performing stoichiometric calculations in chemistry.
For example, in the reaction involving copper(II) sulfate (CuSO鈧�) and zinc (Zn), we know that the molar concentration of the CuSO鈧� solution is 0.156 M. This means there are 0.156 moles of CuSO鈧� in every liter of solution.
  • This allows us to calculate how many moles are present in a given volume of solution.
  • It is crucial when figuring out how much reactant is needed or produced in a chemical reaction.
Always ensure that your units match when performing calculations involving molarity.
Chemical Reactions
Chemical reactions occur when substances interact to form new products. In our exercise, zinc (Zn) reacts with copper(II) sulfate (CuSO鈧�) in a single displacement reaction.
The balanced chemical equation for this reaction is:
\[\text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu}\]Balanced equations are vital as they indicate the proportion of reactants and products. Here are some basics about this type of chemical reaction:
  • A balanced reaction respects the law of conservation of mass, meaning the number of atoms for each element is the same on both sides of the equation.
  • Single displacement reactions involve one element being replaced by another in a compound.
Understanding the balanced equation helps us determine how chemicals interact and the amounts needed for reactions to occur.
Molar Mass
Molar mass is the mass of one mole of a substance, usually expressed in grams per mole (g/mol). It serves as a bridge between the mass of a substance and the amount in moles.
Take zinc (Zn) as an example; its molar mass is approximately 65.38 g/mol. This means that one mole of zinc weighs 65.38 grams.
  • To convert a given mass to moles, divide the mass by the molar mass.
  • In our problem, the conversion of 7.89 g of zinc is accomplished by dividing by its molar mass, leading to approximately 0.1207 moles of zinc.
Molar mass is fundamental in stoichiometry as it allows for the conversion between grams and moles, enabling accurate calculations in chemical equations.
Solution Volume
Solution volume is the amount of space that a solution occupies, typically measured in liters or milliliters. Calculating the volume required for a reaction is a common task in chemistry.
In the CuSO鈧� and Zn reaction, we needed to find the volume of CuSO鈧� solution that contains 0.1207 moles of solute given a molarity of 0.156 M.
You can determine the volume with the formula:
\[\text{Volume} = \frac{\text{Moles of solute}}{\text{Molarity}}\]
  • In this case, dividing the 0.1207 moles of CuSO鈧� by the 0.156 M molarity gives a volume of approximately 0.773 liters.
  • Converting to milliliters by multiplying by 1000 results in 773 mL.
Proper calculation of solution volume ensures the right amount of reactant is used, impacting the outcome of chemical experiments.

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

For each of the following pairs of combinations, indicate which one will produce the greater mass of solid product: a) \(105.5 \mathrm{~mL} 1.508 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) and \(250.0 \mathrm{~mL}\) \(1.2075 \mathrm{M} \mathrm{KCl}\) or \(138.5 \mathrm{~mL} 1.469 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) and \(100.0 \mathrm{~mL} 2.115 \mathrm{M} \mathrm{KCl}\) b) \(32.25 \mathrm{~mL} 0.9475 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) and \(92.75 \mathrm{~mL} 0.7750 \mathrm{M}\) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) or \(52.50 \mathrm{~mL} 0.6810 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) and \(39.50 \mathrm{~mL} 1.555 \mathrm{M}\) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) c) \(29.75 \mathrm{~mL} 1.575 \mathrm{M} \mathrm{AgNO}_{3}\) and \(25.00 \mathrm{~mL} 2.010 \mathrm{M}\) \(\mathrm{BaCl}_{2}\) or \(52.80 \mathrm{~mL} 2.010 \mathrm{M} \mathrm{AgNO}_{3}\) and \(73.50 \mathrm{~mL} 0.7500 \mathrm{M}\) \(\mathrm{BaCl}_{2}\)

Acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right)\) is a monoprotic acid commonly known as "aspirin." A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took \(12.25 \mathrm{~mL}\) of \(0.1466 \mathrm{M} \mathrm{NaOH}\) to neutralize the solution. Calculate the number of grains of aspirin in the tablet (one grain \(=0.0648 \mathrm{~g}\) ).

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

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is an important industrial chemical used in fertilizers, detergents, and the food industry. It is produced by two different methods. In the electric furnace method elemental phosphorus \(\left(\mathrm{P}_{4}\right)\) is burned in air to form \(\mathrm{P}_{4} \mathrm{O}_{10}\), which is then combined with water to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\). In the wet process the mineral phosphate rock \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]\) is combined with sulfuric acid to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (and \(\mathrm{HF}\) and \(\mathrm{CaSO}_{4}\) ). Write equations for these processes, and classify each step as precipitation, acid-base, or redox reaction.

Determine which of the following metals can react with acid: (a) \(\mathrm{Au},(\mathrm{b}) \mathrm{Ni},(\mathrm{c}) \mathrm{Zn},(\mathrm{d}) \mathrm{Ag},(\mathrm{e}) \mathrm{Pt}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Inorganic 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.