3. In the reaction below, H2O is a(n):H2SO; +H20 → H;0*+HSO;b. acida. BaseSue conjugate acidd. conjugate base4. What is the pH of a 1.53 x 10-6 M solution of HCl?c. 6.99a. 5.82b. 8.18d. 4.155. Acetic acid is a weak monoprotic acid. Its concentration is 0.20 M and its Ka value is1.8x10- Calculate its pH value.a. 0.698b. 2.72с. 11.28d. none of theanswer are correct6. Naz CO; forms alkaline solution when dissolved in water. Why?a. Because water hydrolysis produces hydroxideb. CO32- ions reacts with H from water to produce HCO;c. Na, CO; dissociates completely to produce CO;2- ionsd. CO;?- ions reacts with water to produce carbonic acidThe buffar celutien

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Answered: 3. In the reaction below, H2O is a(n):…

3. In the reaction below, H2O is a(n): H2SO; +H2O → H;O*+ HSO; a. Base b. acid Su conjugate acid d. conjugate base 4. What is the pH of a 1.53 x 10-6 M solution of HC1?

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.

Question

3. In the reaction below, H2O is a(n):
H2SO; +H20 → H;0*+HSO;
b. acid
a. Base
Sue conjugate acid
d. conjugate base
4. What is the pH of a 1.53 x 10-6 M solution of HCl?
c. 6.99
a. 5.82
b. 8.18
d. 4.15
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
b. 2.72
с. 11.28
d. none of the
answer are correct
6. Naz CO; forms alkaline solution when dissolved in water. Why?
a. Because water hydrolysis produces hydroxide
b. CO32- ions reacts with H from water to produce HCO;
c. Na, CO; dissociates completely to produce CO;2- ions
d. CO;?- ions reacts with water to produce carbonic acid
The buffar celutien

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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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A sample of water from a stream has [H3O*]=3.1 × 10-9 M. Which statement below accurately describes this water sample? A. The water sample is acidic. B. The water sample is a basic solution. C. The pOH of the water sample is 8.50. D. pH of the water sample is much les than 7.0. E. The pH of the water sample is 7.5.
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A. Calculate the concentration of HBr if a solution has a pH of 2.05? B. Predict the pH of a 0.347 M NaOH solution?
A. Complete and balance the reaction: HCI (aq) + H20 (0) --> ? B. Consider a 3.22x10M HCI (aq) solution. Calculate the [H30"), [OH], and pH of the solution. C. Enter the pH of the solution below. Show your work. Round the pH to the hundredths place. Tyne vour answer
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