Answered: Correct Solve an equilibrium problem…

Correct Solve an equilibrium problem (using an ICE table) to calculate the pH of each of the following solutions. Part B 0.13 mol L- CH3NH3CI Express your answer using two decimal places.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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M Review I Constar
Correct
Solve an equilibrium problem (using an ICE table)
to calculate the pH of each of the following
solutions.
Part B
0.13 mol L- CH3 NH3C1
Express your answer using two decimal places.
V ΑΣφ
pH =
Submit
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[References] A chemist prepares dilute solutions of equal molar concentrations of CH3 NH,, CH3 NH, CI, NaNO,, and NaNO3 Rank these solutions from highest pH to low pH. (K, for CH3 NH2 is 4.4 x 10 K. for HNO, is 4.5 x 10 4.) Decreasing of pH Drag and drop your selection from the following list to complete the answer CH,NH2 NaNO; CH;NH3 CI NaNO,
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6 CHOOSE ALL THE FOLLOWING THATS TRUE
The Bronsted-Lowry (B-L) definition of acids and bases was developed mainly because there were problems with the Arrhenius definition that kept some acids and/or bases from being classified properly. Which of the following explains the problem of the Arrhenius definition and how the Bronsted-Lowry definition help fix the classification problems. The Arrhenius definition only classified acids/bases dissolved in water as well as bases were only those that released hydroxide ions into solution. Where in the B-L definition the acid & base does not have to be in a water solution and it says a base is any substance that accepts a hydrogen ion. The Arrhenius definition only classified acids/bases dissolved in water as well as bases were only those that released hydrogen ions into solution. Where in the B-L definition the acid & base does not have to be in a water solution and it says a base is any substance that accepts a hydrogen ion. The Arrhenius definition only classified acids/bases…
You make a 0.315 M solution of an acid. The solution pH is 2.26. Calculate the Ka value forthe acid.
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b) Determine the formula of the acid and the formula of the base to which each salt is related and put it them the appropriate columns in Table IV. using A= Acidic Salt, B = Basic Salt, and N = Neutral Salt. a) Copy your classification for each salt in Table III into Table IV. You can abbreviate in the "strength" (i.e. weak or strong) for each acid and base. NaOH + TABLE IV Parent Base Base Strength Salt Parent Acid Acid Strength Class. 0.1 M KC,H,CO, weak 0.1 M CH,NHNO, 0.1 M Sr(NO,)2 2. 0.1 M NaC,H,02 SB KA 0.1 M CH,CH,NH,CI 2. 0.1 M RBCIO 4 0.1 M NHI strong SB 0.1 M NaHCOO 0.1 M KBr strong SB 0.1 M K,S
Use the References to access important values if needed for this question. The pH of an aqueous solution of 0.530 M aniline (a weak base with the formula CHNH2) is Submit Answer 5 question attempts remaining
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