3. In the reaction below, H:O is a(n):H;SO; + H:0 –→ H;O*+HSO;a. Baseb. acid4. What is the pH of a 1.53 x 104M solution of HC1?b. 8.18S. conjugate acidd. conjugate basea. 5.825. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is1.8x10 Calculate its pH value.a. 0.698c. 6.99d. 4.15b. 2.72c. 11.28d. none of theanswer are correct6. Na: CO: forms alkaline solution when dissolved in water. Why?a. Because water hydrolysis produces hydroxideb. CO, ions reacts with H from water to produce HCO;c. Na: CO, dissociates completely to prođuce CO;- ionsd. CO,- ions reacts with water to produce carbonic acid7. The buffer solution maintains pH by some events excepta. The addition of a little acidb. The addition ofa little basec. Addition of waterd. The addition of excess acid

The question is based upon acid base concept and we know that acid are those molecule which donate…

3. In the reaction below, H;O is a(n): H;SO, + H:O → H;O*+HSO; a. Base 4. What is the pH of a 1.53 x 104M solution of HCI? 2. 5.82 b. acid S. conjugate acid d. conjugate base b. 8.18 C. 6.99 d. 4.15

3. In the reaction below, H;O is a(n): H;SO, + H:O → H;O*+HSO; a. Base 4. What is the pH of a 1.53 x 104M solution of HCI? 2. 5.82 b. acid S. conjugate acid d. conjugate base b. 8.18 C. 6.99 d. 4.15

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...

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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.

Question

3. In the reaction below, H:O is a(n):
H;SO; + H:0 –→ H;O*+HSO;
a. Base
b. acid
4. What is the pH of a 1.53 x 104M solution of HC1?
b. 8.18
S. conjugate acid
d. conjugate base
a. 5.82
5. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is
1.8x10 Calculate its pH value.
a. 0.698
c. 6.99
d. 4.15
b. 2.72
c. 11.28
d. none of the
answer are correct
6. Na: CO: forms alkaline solution when dissolved in water. Why?
a. Because water hydrolysis produces hydroxide
b. CO, ions reacts with H from water to produce HCO;
c. Na: CO, dissociates completely to prođuce CO;- ions
d. CO,- ions reacts with water to produce carbonic acid
7. The buffer solution maintains pH by some events except
a. The addition of a little acid
b. The addition ofa little base
c. Addition of water
d. The addition of excess acid

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