Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 78

A 30.0 -mL. sample of an unknown strong base is neutralized after the addition of \(12.0 \mathrm{mL}\) of a \(0.150 \mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is 0.0300 \(M,\) give some possible identities for the unknown base.

Short Answer

Expert verified
Possible identities of the unknown base with a concentration of 0.0300 M are Calcium hydroxide (Ca(OH)2), Barium hydroxide (Ba(OH)2), and Strontium hydroxide (Sr(OH)2), as two moles of these bases are needed to neutralize one mole of HNO3 due to their two reactive hydroxide ions (OH-).

Step by step solution

01

Calculate the moles of HNO3 used in the reaction

First, we need to find the number of moles of the strong acid (HNO3) used to neutralize the unknown base. The concentration (M) is given, as well as the volume of the HNO3 solution. Using the formula moles = Molarity × Volume (in Liters), we can find the moles of HNO3: moles of HNO3 = (0.150 M) × (12.0 mL × 0.001 L/mL) = 0.00180 moles
02

Calculate the moles of the unknown base

Next, we need to find the number of moles of the unknown strong base, knowing its concentration and volume. We use the same formula as in Step 1: moles of the base = (0.0300 M) × (30.0 mL × 0.001 L/mL) = 0.000900 moles
03

Determine the mole ratio between HNO3 and the unknown base

Now, we can find the mole ratio between the strong acid and the base by dividing the moles of the base by the moles of HNO3: mole ratio = (moles of the base) / (moles of HNO3) mole ratio = 0.000900 / 0.00180 = 0.500 The mole ratio tells us how many moles of the base required to neutralize one mole of HNO3.
04

Determine possible identities of the unknown base

Since the mole ratio between the acid and base is 0.500, this means that two moles of the base are needed to neutralize one mole of HNO3, and as a result, the unknown base has two reactive hydroxide ions (OH-) in its formula. Some examples of strong bases with this property are: 1. Calcium hydroxide (Ca(OH)2) 2. Barium hydroxide (Ba(OH)2) 3. Strontium hydroxide (Sr(OH)2) These are the possible identities of the unknown strong base since they all have two hydroxide ions that would neutralize one mole of the HNO3.

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

Give an example how each of the following insoluble ionic compounds could be produced using a precipitation reaction. Write the balanced formula equation for each reaction. a. \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) c. \(\mathrm{PbSO}_{4}(s)\) b. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\) d. \(\mathrm{BaCrO}_{4}(s)\)

In a \(1-\) L beaker, \(203 \mathrm{mL}\) of \(0.307 M\) ammonium chromate was mixed with \(137 \mathrm{mL}\) of \(0.269 M\) chromium(III) nitrite to produce ammonium nitrite and chromium(III) chromate. Write the balanced chemical equation for the reaction occurring here. If the percent yield of the reaction was \(88.0 \%,\) what mass of chromium(III) chromate was isolated?

Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. \(\mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\) b. \(\mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) c. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\mathrm{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(i)\)

A \(25.00-\mathrm{mL}\) sample of hydrochloric acid solution requires \(24.16 \mathrm{mL}\) of \(0.106 \mathrm{M}\) sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

The unknown acid \(\mathrm{H}_{2} \mathrm{X}\) can be neutralized completely by \(\mathrm{OH}^{-}\) according to the following (unbalanced) equation: $$ \mathrm{H}_{2} \mathrm{X}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{X}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ The ion formed as a product, \(\mathrm{X}^{2-},\) was shown to have 36 total electrons. What is element X? Propose a name for \(\mathrm{H}_{2} \mathrm{X}\). To completely neutralize a sample of \(\mathrm{H}_{2} \mathrm{X}, 35.6 \mathrm{~mL}\) of \(0.175 \mathrm{M}\) \(\mathrm{OH}^{-}\) solution was required. What was the mass of the \(\mathrm{H}_{2} \mathrm{X}\) sample used?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

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