**Arrange the following 0.10 M solutions in order of increasing pH.**There is an arrow pointing right with the label "From lowest to highest pH."Below the arrow are five blank spaces with less-than symbols ("<") between them, indicating the order to be filled.**Instructions:**Drag and drop your selection from the following list to complete the answer:- NH₄Cl- NaCH₃CO₂- NaCl- KOH- HCl**Note:** Arrange these chemicals in order based on their pH when in a 0.10 M solution.

Answered: Image /qna-images/answer/a5786931-00e6-4f94-a8f7-692eb97044c3.jpg

Arrange the following 0.10 M solutions in order of increasing pH. From lowest to highest pH Drag and drop your selection from the following list to complete the answer: NH4CI NACH3 CO2 NaCl кон HCI V

Arrange the following 0.10 M solutions in order of increasing pH. From lowest to highest pH Drag and drop your selection from the following list to complete the answer: NH4CI NACH3 CO2 NaCl кон HCI V

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...

See similar textbooks

Related questions

Q: Determine the [H+][H+] , pH, and pOH of a solution with an [OH−][OH−] of 6.3×10−5 M6.3×10−5 M at 25…

A: Given, a solution with an OH-=6.3×10-5 M at 25°C OH-, PH and POH is:

Q: :NH + Ph—C=C: FN + CH3CH₂COOH H e :N: + Ph-C=CH NH + CHỊCH,COO ・・・・ O-H 00-H H

Q: Determine the [H+][H+] , pH, and pOH of a solution with an [OH−][OH−] of 5.1×10−9 M5.1×10−9 M at 25…

A: OH- concentration of a solution is 5.1 × 10-9 M at 25 °C .We have to determine the - H+…

Q: Consider an unknown solution. Tests were conducted and the following results were obtained. Red…

Q: 01.50 x 10-4 02.22 × 10-10 04.50 × 10⁹ 01.12 x 10-5 04.50 × 10-5 entrati (in M) of a NaOH solution…

A: • The values provided in the question are:- i) pOH of a NaOH solution= 4.35 >> We need…

Q: Each row of the table below describes an aqueous solution at about 25°C . Complete the table. That…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Identify which of the compounds below will behave as a Brønsted-Lowry acid or base when dissolved in…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Since, H3PO4 is a triprotic acid it dissociates with water a follows-

Q: Each row of the table below describes an aqueous solution at about 25°C . Complete the table.…

A: An incomplete table based on pH calculation, which is to be accomplished.

Q: Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That…

A: The formula to relate hydronium ion concentration and pH is as follows: pH = -log[H3O+]

Q: How do I know whether something is a weak acid or weak base? I know there's a list of tables of…

Q: e [ОН] in

Q: Calculate either [H3O+] or [OH-] for each of the solutions. Solution A: [OH-] = 2.77 x 10-7 M;…

A: The objective of the question is to calculate the missing concentration of either hydronium ions…

Q: What is the percent ionization of a 0.36M aqueous solution of formic acid, HCHO2 that is also 0.08 M…

A: 0.36 M aqueous solution of formic acid is present in 0.08 M HCl. The Ka of formic acid is 1.7 * 10-4…

Q: [H+] = 1.0 x 10-7 pOH = 7.00 pOH = 12.12 Answer Bank [OH-] = 1.4 x 10-3 pH = 13.41 pH = 3.64 pOH =…

A: At 25oC, the solution are classified as acidic, basic or neutral on the basis of the value of pH. If…

Q: The base ionization constant of ammonia is 1.8 x 105. In a 0.090 M NH3 solution, what percentage of…

A: According to Ostwald dilution law degree of dissociation of a weak electrolyte is inversely…

Q: Calculate the percent ionization of acetic acid solutions having the following concentrations.…

A: Given :

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the [H3O+].

A: Given: The concentration of hydroxide ions is provided,i.e. [OH-] = 1.0 x 10-5 M. The hydronium ion…

Q: Calculate the pOH of a 0.05% HNO3 solution. (Densities: HNO3 = 1.51 g/cm; H20 = 1 %3D %3D g/cm3)…

A: The question is based on the concept of molarity. it is defined as number of moles of solute…

Q: Which of the following solutions has a p

A: Salt hydrolysis : the process in which cation (or) anion (or) both of a salt reacts with water to…

Q: Identify the strong base(s) in the list below (You may assume that all of the substances listed are…

A: rubidium hydroxide (RbOH) is strong base because of ionic bond .

Q: Each row of the table below describes an aqueous solution at about 25°C . Complete the table.…

A: Three numerical problems based on pH calculation, which are to be accomplished.

Q: Construct the expression for Kb for the weak base, CN-. CN- (aq) + H₂O(1) OH-(aq) + HCN(aq) Based on…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Since you have posted a question with multiple sub-parts, we will provide the solution only for the…

Q: Arrange the following 0.10 M solutions in order of increasing pH. From lowest to highest pH Drag and…

A: Hcl is strongly acidic. KOH is strong base. NH4Cl,NaCl,NaCH3CO2,are salt

Q: Calculate the percent ionization of a 0.441 M solution of hydrocyanic acid. (Assume that K₁ (HCN) =…

Q: A typical vitamin C tablet (containing pure ascorbic acid, H₂C6H606) weighs 500 mg. One vitamin C…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: A solution has [H+] = 4.0 x 10-3 M. The [OH"] in this solution is %3D 4.0 x 1011 1.0 x 10 14M 4.0 x…

A: Given data,[H+]=4.0×10-3M

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as an acid,…

A: pH is defined as the negative logarithm of hydrogen ion, H+ concentration of base ten .So, the…

Q: Calculate the [H+1]for this solution.

Q: Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the [H3O+].

Q: What is the pHpH of a 0.0075 MM solution of HClHCl? Express your answer using two decimal places.

A: 1- We know that, HCl is strong acid and it's released 100% H+ ion in water. So, the concentration…

Q: Determine the pHpH for the following solutions: A) [H3O+]=7.7×10−2M[H3O+]=7.7×10−2M, Express your…

A: pH is a negative logarithm of Hydrogen ion concentration. It is given by Sorenson. It can be written…

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.

Question

**Arrange the following 0.10 M solutions in order of increasing pH.**

There is an arrow pointing right with the label "From lowest to highest pH."

Below the arrow are five blank spaces with less-than symbols ("<") between them, indicating the order to be filled.

**Instructions:**
Drag and drop your selection from the following list to complete the answer:

- NH₄Cl
- NaCH₃CO₂
- NaCl
- KOH
- HCl

**Note:** Arrange these chemicals in order based on their pH when in a 0.10 M solution.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Answer

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Which of the following aqueous solutions will have the greatest concentration of H+? 0.0170 M H2SO4 0.8000 M H2NNH2 0.0170 M HCl 0.0180 M HCHO2
None
Classify each of the following substances as either a strong or weak acid, strong or weak base, or a soluble or insolu NH3 HCN BaBr2 HF CH3COOH Clear All strong acid weak acid strong base weak base soluble salt insoluble salt
Calculate the concentration of all species in a 0.240 MC6H5NH3Cl solution. Enter your answers numerically separated by commas. Express your answer using two significant figures. [C6H5NH+3], [Cl−], [C6H5NH2],[H3O+], [OH−] =
Consider a solution which is [OH-] = 1.0 x 10-5 M.Calculate the [H3O+].
A solution has [H]=4.0 x10-3 M. The [OH ] in this solution is () 4x 1011 M 4x 10-17 M ) 2.5 x 10-12 M 1 x 10-14 M none of these
Place the solutions below in order of increasing acid strength. 1. Citric Acid (C6H8O7) 2. Sodium Hydroxide (NaOH) 3. Aqueous Ammonia (NH3) 4. Sodium hydrogen carbonate (NaHCO3) 5. Boric Acid (H3BO3)
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic pH = 4.24 pOH = 12.17 [H+] = [OH] = 9.7 x 10-⁹ [OH-] = 9.3 x 10-6 = 8.3 × 10-m x Basic pH = 10.91 pOH = 3.22 [H+] = 7.6 × 10-¹0 Answer Bank Neutral [H+] = 1.0 x 10-7 pOH = 7.00