Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 88

A solution is made by mixing \(1.5 \mathrm{~g}\) of \(\mathrm{LiOH}\) and $23.5 \mathrm{~mL}\( of \)1.000 \mathrm{M}$ HNO3. (a) Write a balanced equation for the reaction that occurs between the solutes. (b) Calculate the concentration of each ion remaining in solution. (c) Is the resulting solution acidic or basic?

Short Answer

Expert verified
The balanced chemical equation for the reaction between LiOH and HNO3 is: \( LiOH + HNO_3 \rightarrow LiNO_3 + H_2O \). After the reaction, there are 1.668 M OH- ions, and 1.000 M Li+ and NO3- ions remaining in the solution. As there are no H+ ions remaining and the presence of OH- ions, the solution is basic.

Step by step solution

01

Write the balanced chemical equation

The reaction between LiOH (a base) and HNO3 (an acid) is an acid-base neutralization reaction, which produces water and a salt. The balanced chemical equation for the reaction is: \( LiOH + HNO_3 \rightarrow LiNO_3 + H_2O \)
02

Convert given amount of reactants into moles

As we are given mass of LiOH and the volume and concentration of HNO3, we have to convert these amounts into moles. Given, mass of LiOH = 1.5 g Molar mass of LiOH = 6.94 (Li) + 15.999 (O) + 1.008 (H) = 23.942 g/mol Moles of LiOH = mass/molar mass Moles of LiOH = 1.5 g / 23.942 g/mol = 0.0627 mol Given, volume of HNO3 = 23.5 mL = 0.0235 L Concentration of HNO3 = 1.000 M Moles of HNO3 = concentration × volume Moles of HNO3 = 1.000 M × 0.0235 L = 0.0235 mol
03

Determine the limiting reactant

Let's compare the mole ratio of reactants based on the balanced equation and the mole ratio from the given amounts of reactants. From the balanced equation: 1 mol LiOH : 1 mol HNO3 Given amounts: 0.0627 mol LiOH : 0.0235 mol HNO3 Since the given amounts of LiOH : HNO3 are greater than the mole ratio in the balanced equation, HNO3 is the limiting reactant. The reaction will consume all of the HNO3 and only a portion of the LiOH.
04

Calculate the remaining amounts of reactants and products

As HNO3 is the limiting reactant, it will be completely consumed. This means that in the resulting solution, there will be no HNO3 left and no H+ ions (from the consumed HNO3). Moles of LiOH remaining = Initial moles of LiOH - moles of consumed LiOH Moles of LiOH remaining = 0.0627 mol - 0.0235 mol = 0.0392 mol Moles of LiNO3 produced = moles of HNO3 consumed = 0.0235 mol
05

Calculate the concentration of each remaining ion

The total volume of the solution (assuming it does not change significantly due to the reaction) = 23.5 mL = 0.0235 L Concentration of remaining OH- ions (from LiOH) = moles of LiOH remaining / total volume Concentration of OH- ions = 0.0392 mol / 0.0235 L = 1.668 M Concentration of remaining Li+ and NO3- ions (from LiNO3) = moles of LiNO3 produced / total volume Concentration of Li+ and NO3- ions = 0.0235 mol / 0.0235 L = 1.000 M
06

Determine whether the solution is acidic or basic

Since there are no H+ ions remaining in the solution but there are OH- ions present, the solution will be basic. This is because a higher concentration of OH- ions compared to H+ ions will result in a pH greater than 7.

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

The commercial production of nitric acid involves the following chemical reactions: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \end{aligned} $$ (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction. (c) How many grams of ammonia must you start with to make $1000.0 \mathrm{~L}\( of a \)0.150 \mathrm{M}$ aqueous solution of nitric acid? Assume all the reactions give \(100 \%\) yield.

You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next an $\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)$ solution is added and a white precipitate forms. What is the identity of the unknown white solid? [Section 4.2\(]\)

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous \(\mathrm{HCl}\) in the stomach and each of the following substances used in various antacids: (a) $\mathrm{Al}(\mathrm{OH})_{3}(s),(\mathbf{b}) \mathrm{Mg}(\mathrm{OH})_{2}(s),(\mathbf{c}) \mathrm{MgCO}_{3}(s),$ (d) \(\mathrm{NaAl}\left(\mathrm{CO}_{3}\right)(\mathrm{OH})_{2}(s)\) (e) \(\mathrm{CaCO}_{3}(s)\)

Citric acid, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\), is a triprotic acid. It occurs naturally in citrus fruits like lemons and has applications in food flavouring and preservatives. A solution containing an unknown concentration of the acid is titrated with KOH. It requires $23.20 \mathrm{~mL}\( of \)0.500 \mathrm{M} \mathrm{KOH}$ solution to titrate all three acidic protons in \(100.00 \mathrm{~mL}\) of the citric acid solution. Write a balanced net ionic equation for the neutralization reaction, and calculate the molarity of the citric acid solution.

An \(8.65-g\) sample of an unknown group 2 metal hydroxide is dissolved in $85.0 \mathrm{~mL}$ of water. An acid-base indicator is added and the resulting solution is titrated with \(2.50 \mathrm{M}\) \(\mathrm{HCl}(a q)\) solution. The indicator changes color, signaling that the equivalence point has been reached, after \(56.9 \mathrm{~mL}\) of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the metal cation: \(\mathrm{Ca}^{2+}, \mathrm{Sr}^{2+},\) or $\mathrm{Ba}^{2+} ?$
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

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