**Question:**Which of the following is NOT a property of an acid?**Options:**1. ☐ reacts with acids2. ☐ donates a proton3. ☐ has pH less than 74. ☐ feel slippery5. ☐ taste sour**Explanation:**- **Reacts with acids:** Generally, acids react with bases, not with other acids.- **Donates a proton:** Acids are known to donate protons (H⁺ ions) in reactions.- **Has pH less than 7:** Acids have a pH value that is less than 7.- **Feel slippery:** This is a property of bases, not acids.- **Taste sour:** Acids typically taste sour.The correct answer is **"feel slippery"** as it is not a property of an acid.

Given properties: reacts with acids donates a proton has a pH less than 7 feel slippery taste sour We have to find the property that is not a property of an acid.

Answered: Which of the following is NOT a…

Science

Chemistry

Which of the following is NOT a property of an acid? O reacts with acids O donates a proton O has pH less than 7 O feel slippery O taste sour

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: The hydrogen concentration of a solution is 1 x 10-14 M. What is the pH? pH = Is this an acid,…

A: Answer: The pH of the solution is 14 and the solution is Basic.

Q: Write a net ionic equation to show that hydrocyanic acid , HCN , behaves as an acid in water. + H20…

A: The answer to the following question is-

Q: What is the hydronium ion concentration of a 0.0037 M solution of HNO3?

A: HNO3 is a strong acid so it completely ionized in water to produce hydronium ion and nitrate ion…

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 9.0 × 10-6 M? pH =

Q: In the neutralization reaction below17.3 mL of H2SO4 solution are required to neutralize 32.2 mL of…

Q: Determine the concentration of NO−3 for 0.16 MM KNO3

A: A strong electrolyte dissociates completely into its ionic constituents in an aqueous solution. The…

Q: The hydrogen concentration of a solution is 1 x 10-6 M. What is the pH? pH = Is this an acid,…

A: [H+] = 1 x 10-6 M PH = ?

Q: Which of the following is perchloric acid? HClO2 HClO3 HClO4

A: The given acids are the oxoacids of the chlorine atoms. They contain H-Cl-On bond. The n is the…

Q: is the Arrhenius definition of an acid and a base? O a An acid contains hydrogen; a base contains a…

A: The concept of Arrhenius acid base is applicable for only aqueous solution.

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: In HClO2 the ions present are H+ and ClO2 -. Similarly in Ba(OH)2 the ions present are Ba2+ and OH-.…

Q: Calculate the concentration of all ions present in 6.06 g Na,S in 1.00 L of solution.

A: Molarity = moles/volume of solution(in L) Number of moles = mass/molar mass

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.0 × 10-7 M? pH =

A: The concentration of hydrogen ion in the solution is too low thus, the pH of the solution is the…

Q: Describe the pH of the above solution. (pH of a solution containing 1 x 10-7 M of hydronium ions…

A: Since the pH of any solution is given by pH = -log[H3O+]. where [H3O+] = concentration of H3O+ ions…

Q: A 0.261 g sample of NaHC2O4 (one acidic proton) required 17.5 mL of sodium hydroxide solution for…

A: The complete balanced Chemical Reaction is - NaHC2O4 + NaOH ----> Na3C2O4 + H2O Thus, one mole of…

Q: Does neutral mean there are no acids or bases present? Can a neutral solution have hydronium or…

A: Acid : Acid is the substance which can donate proton (H+) to other substances in aqueous medium.…

Q: Which are the strong acids? HCI, HI, HNO3, and H2CO3

A: Strong acid is that which dissociate in to ions when dissolved in water and weak acid do not…

Q: What is the hydronium M ion concentration for an unknown solution with a pH of 9.65? Please write…

A: Given PH = 9.65 [ H3O+ ] = ?

Q: When dissolved in water, which of the following will not affect the pH? O NH4BR O CaCO3 O NANO3 O…

A: NH4Br is salt of strong acid, HBr and weak base, NH4OH and the solution is acidic in nature, pH of…

Q: 10.0 M NH3 pH: [H30+]: [OH-]: pOH:

Q: what is the concentration of cl- ions in a 0.1 M solution of calcium chloride?

Q: solution of a weak acid has a concentration of 0.133 M. If the solution is also 0.024 M in…

A: concentration = 0.133 M = C Percentage ionisation= 8.69 Hydrobromic acid concentration= 0.024 M We…

Q: How can we complete the table from hypochlorous acid to sodium cynanide?

A: Since you have asked multiple subpart question, we will solve the first three-question for you. If…

Q: 700 mi boas 92sd new roATS We have to a Predict: Acid, base or salt? Data Table 1: Name and…

A: As per the guidelines, I can only answer first three sub-parts of the question. If you want any…

Q: Determine the concentration of oxygen ions in 0.5000 M SnO3

A: Given Concentration of SnO3 = 0.5000 M Concentration of oxygen ion = ?

Q: Write the formula of the acid and base that need to be reacted to produce the salt: AlCl3

A: Al(OH)3 is the base and HCl is the acid to form AlCl3 as salt.

Q: What is the [H3O+] of an acidic solution that hs a ph of 11.25

A: To calculate pH you need to know the concentration of the hydroniumion [H3O+]. The pH is then…

Q: What volume of0.317 M KOH solution will be required to titrations 25.00 mL of 0.285 M HN O3

A: The molarity of a solution is defined as the ratio of the number of moles of solute that are present…

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H] = 8.5 x 10-7 M? pH =

Q: Write the dominant form of the compound in water for each compounds: HNO3, H2O, PbSO4, NH4OH,…

A: The reactions when the given compounds are dissolved in water are as follows:

Q: The hydronium ion concentration is 1x10(-5). What is the [H+] concentration?

A: H3O+ = 1x 10^(-5) H+ + H2O-----> H3O+ THIS REPRESENT THAT H+ AND H3O+ ARE SAME SO IN THIS CASE…

Q: What is the pH of a 0.130 M solution of HNO₃?b

Q: For K w, the product of [H 3O +] and [OH -] is

A: Kw is the water constant and is defined as product of hydronium ion and hydroxyl ion Kw = [H3O+]…

Q: {OH-} =0.002 M pH=

Q: 7) Name the following bases: Base formula Positive ion Negative ion Base name ex> NAOH Na OH sodium…

A: Base are the substances which give OH- ions in their aqueous solutions. Positive ions are also…

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

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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

Part A - Solution 1 After being given a solution containing a set of unknown ions, you perform the following sequence of tests to determine the identity of the cations in solution: 1. A flame test produces no color 2. You take a small portion of the solution and add NaOH. A vapor is produced that turns red litmus blue. 3. You add HCI to solution, which results in the formation of a white precipitate. The supernatant is separated and used for the remainder of the tests. 4. The addition of buffered NH4*/NH3 to a portion of the supernatant from step 3 does not produce a precipitate. 5. The addition of ammonium oxalate to a portion of the superntant from step 3 does not produce a precipitate 6. The addition of a strong base to a portion of the supernatant from step 3 generates a precipitate. 7. The supernatant from step 6 is separated from the precipitate. The addition of HCI and K4Fe(CN)6 to the solution produces no reaction. Based on these tests, identify which of the following ions must…
The [H3O+] of a solution with pH =7 is
Which salt is a strong electrolyte? O iron (III) phosphate ammonium sulfate O calcium carbonate silver chloride
If the concentration of [H30+] = 4.2 x 10-5, what is the pH of the solution?
Write the three dissociation equations of H3PO4 and the respective Ka equations.
Write the balanced chemical equations for the neutraliztion reactions between:
9. What is the pH of a solution with [H3O+] = 7.3 x 10-4 M?
When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown?Co + Ni2+ = Co2+ + Ni