Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 53

Exactly \(1.00 \mathrm{mL}\) of an aqueous solution of \(\mathrm{HNO}_{3}\) is diluted to \(100.0 \mathrm{mL}\). It takes \(29.78 \mathrm{mL}\) of \(0.0142 \mathrm{M}\) \(\mathrm{Ca}(\mathrm{OH})_{2}\) to convert all of the \(\mathrm{HNO}_{3}\) to \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) The other product of the reaction is water. Calculate the molarity of the undiluted HNO \(_{3}\) solution.

Short Answer

Expert verified
The molarity of the undiluted HNO_3 solution is 0.84552 M

Step by step solution

01

Identify the reaction equation

Determine the reaction equation between \(HNO_3\) (nitric acid), \(Ca(OH)_2\) (calcium hydroxide) and their resulting products. The balanced equation is: \(2HNO_3 + Ca(OH)_2 \rightarrow Ca(NO_3)_2 + 2H_2O\) This means that two moles of nitric acid react with one mole of calcium hydroxide to produce calcium nitrate and water.
02

Calculate the mol of \(Ca(OH)_2\)

Determine the number of mole of \(Ca(OH)_2\) used in the reaction via the formula: \[mol = Molarity \ x \ Volume\] Where the molarity is given as 0.0142 M and the volume is 29.78 mL or 0.02978L. Plugging these values into the formula gives: \[mol = \ 0.0142 M \times 0.02978 L = 0.00042276\ mol \] of \(Ca(OH)_2\)
03

Calculate the mol of \(HNO_3\)

In the balanced equation, it can be observed that 2 moles of \(HNO_3\) reacts with 1 mole of \(Ca(OH)_2\). This means that the amount of \(HNO_3\) moles is twice the amount of \(Ca(OH)_2\). So the \(HNO_3\) moles is: \[0.00042276 \ mol \times 2 = 0.00084552\ mol \] of \(HNO_3\)
04

Calculate the Molarity of undiluted \(HNO_3\)

Recall that molarity is defined as the number of moles per liter of solution. As it was stated that one ml of the acid was diluted to 100mL, the molarity of the undiluted solution \(HNO_3\), using the formula \( Molarity = \frac{mol}{Volume} \), would be: \[\frac{0.00084552}{0.001 L} = 0.84552 M\]

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

For a specific reaction, ammonium dichromate is the only reactant and chromium(III) oxide and water are two of the three products. What is the third product and how many grams of this product are produced per kilogram of ammonium dichromate decomposed?

Solid silver oxide, \(\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s}),\) decomposes at temperatures in excess of \(300^{\circ} \mathrm{C},\) yielding metallic silver and oxygen gas. A 3.13 g sample of impure silver oxide yields \(0.187 \mathrm{g} \mathrm{O}_{2}(\mathrm{g}) .\) What is the mass percent \(\mathrm{Ag}_{2} \mathrm{O}\) in the sample? Assume that \(\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s})\) is the only source of \(\mathrm{O}_{2}(\mathrm{g}) .\) [Hint: Write a balanced equation for the reaction.]

A laboratory method of preparing \(\mathrm{O}_{2}(\mathrm{g})\) involves the decomposition of \(\mathrm{KClO}_{3}(\mathrm{s})\) $$ 2 \mathrm{KClO}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) $$ (a) How many moles of \(\mathrm{O}_{2}(\mathrm{g})\) can be produced by the decomposition of \(32.8 \mathrm{g} \mathrm{KClO}_{3} ?\) (b) How many grams of \(\mathrm{KClO}_{3}\) must decompose to produce \(50.0 \mathrm{g} \mathrm{O}_{2} ?\) (c) How many grams of KCl are formed, together with \(28.3 \mathrm{g} \mathrm{O}_{2},\) in the decomposition of \(\mathrm{KClO}_{3} ?\)

It is often difficult to determine the concentration of a species in solution, particularly if it is a biological species that takes part in complex reaction pathways. One way to do this is through a dilution experiment with labeled molecules. Instead of molecules, however, we will use fish. An angler wants to know the number of fish in a particular pond, and so puts an indelible mark on 100 fish and adds them to the pond's existing population. After waiting for the fish to spread throughout the pond, the angler starts fishing, eventually catching 18 fish. Of these, five are marked. What is the total number of fish in the pond?

The minerals calcite, \(\mathrm{CaCO}_{3},\) magnesite, \(\mathrm{MgCO}_{3}\) and dolomite, \(\mathrm{CaCO}_{3} \cdot \mathrm{MgCO}_{3},\) decompose when strongly heated to form the corresponding metal oxide(s) and carbon dioxide gas. A 1.000 -g sample known to be one of the three minerals was strongly heated and \(0.477 \mathrm{g} \mathrm{CO}_{2}\) was obtained. Which of the three minerals was it?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Nuclear 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