(a)
Interpretation: From the given concentration of
Concept Introduction:
Autoionization of water is the reaction in which the water undergoes ionization to give a proton and a hydroxide ion. Water is a very weak electrolyte and hence it does not completely dissociate into the ions. The ionization happens to a very less extent only. The ionization of water is an equilibrium reaction and hence this has equilibrium rate constant.
To calculate the concentration of
(a)
Answer to Problem 16.21QP
Answer
The concentration of
Explanation of Solution
Given
Concentration of
Formula
Where,
Substitute the given concentration of
Thus the concentration of
(b)
Interpretation: From the given concentration of
Concept Introduction:
Autoionization of water is the reaction in which the water undergoes ionization to give a proton and a hydroxide ion. Water is a very weak electrolyte and hence it does not completely dissociate into the ions. The ionization happens to a very less extent only. The ionization of water is an equilibrium reaction and hence this has equilibrium rate constant.
To calculate the concentration of
(b)
Answer to Problem 16.21QP
Answer
The concentration of
Explanation of Solution
Given
Concentration of
Formula
Where,
Substitute the given concentration of
Thus the concentration of
c)
Interpretation: From the given concentration of
Concept Introduction:
Autoionization of water is the reaction in which the water undergoes ionization to give a proton and a hydroxide ion. Water is a very weak electrolyte and hence it does not completely dissociate into the ions. The ionization happens to a very less extent only. The ionization of water is an equilibrium reaction and hence this has equilibrium rate constant.
To calculate the concentration of
c)
Answer to Problem 16.21QP
Answer
The concentration of
Explanation of Solution
Given
Concentration of
Formula
Where,
Substitute the given concentration of
Thus the concentration of
(d)
Interpretation: From the given concentration of
Concept Introduction:
Autoionization of water is the reaction in which the water undergoes ionization to give a proton and a hydroxide ion. Water is a very weak electrolyte and hence it does not completely dissociate into the ions. The ionization happens to a very less extent only. The ionization of water is an equilibrium reaction and hence this has equilibrium rate constant.
To calculate the concentration of
(d)
Answer to Problem 16.21QP
Answer
The concentration of
Explanation of Solution
Given
Concentration of
Formula
Where,
Substitute the given concentration of
Thus the concentration of
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Chapter 16 Solutions
EBK CHEMISTRY: ATOMS FIRST
- Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M inNH3(aq) and 0.100 M in NH4Cl(aq). ΔpH= Calculate the change in pH when 7.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. ΔpH=arrow_forwardEach row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B с H₂O H₂O, NaOH H₂O, NaOH H₂O initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add KI add NaBr add H Br add HI effect of change on pH (check one) pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the samearrow_forwardYou are given two glasses of water that have different temperatures. The temperature of the first glass is at 298 K, while the second glass has a temperature of 303 K. It has been determined that the Kw value for the second glass of water is 1.47 x 10-¹4. Which of the following statements is true? (a) The pH of the room temperature glass is higher, but both glasses have the same acidity. (b) The room temperature glass of water has a higher pH, and is more basic than the other glass of water. (c) Both glasses of water are neutral, so both will have a pH of 7.00. (d) The room temperature water has a lower pH, so is more acidic. (e) The warmer glass of water has a lower pH, and is more acidic than the other glass of water.arrow_forward
- Calculate the equilibrium constant for the following reaction: CH3COOH(aq) + F¯ (aq)=CH₂COO (aq) + HF (aq) Be sure your answer has the correct number of significant digits. Note: Reference the K of acids at 25 °C table for additional information. a x10 x Sarrow_forwardEach row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A C H₂O H₂O, HNO3 H₂O H₂O, HNO3 initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add NaOH add KNO3 add NaCl add KOH effect of change on pH (check one) pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the samearrow_forwardWhat is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is equal to 5.2 × 10–13 at 100.0 °C.arrow_forward
- Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C D H₂O H₂O, NaOH H₂O H₂O, NaOH initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic оо 00 neutral change add HCl add Na Br add K Cl add H Br effect of change on pH (check one) pH higher pH lower ο ο1ο ο ο ο ο ο pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the samearrow_forwardGiven 0.01 M solutions of each of the following acids, which solution would have the lowest pH? -117 Hypoiodous acid (HOI), K = 2.3 x 10 Hypobromous acid (HOBr), K = 2.5 x 10 Lactic acid (HC₂H₂O₂), K = 1.3 x 10 Chlorous acid (HClO₂), K = 1.1 x 10²arrow_forwardMethanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENTarrow_forward
- Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.060 M in HBr(aq) at 25 °C. pH = pOH:arrow_forwardYou are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placearrow_forwardA solution NaOH(aq) contains 6.6 g NaOH(s) per 100.0 mL of solution. Calculate the pH and the pOH of the solution at 25 °Carrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning