What is the pH of 4.3 x 10-4 M NaOH(aq)?O 17.410.6O 3.4O -3.4O 24.6

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Answered: What is the pH of 4.3 x 10-4 M NaOH…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.25QAP

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What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?
The sodium salt of propionic acid, NaCH3CH2CO2 is used as an antifungal agent by veterinarians. Calculate the equilibrium concentration of H3O+ and OH the pH for a solution of 0.10M NaCH3CH2CO2.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest electronegativity?. (b) Which of the atoms is smallest?. (c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine. (d) Will the oxide of each element be acidic, basic, or amphoteric?
The chemistry of gallium: (a) Gallium hydroxide, like aluminum hydroxide, is amphoteric. Write a balanced equation to show how this hydroxide can dissolve in both HCl(aq) and NaOH(aq). (b) Gallium ion in water, Ga3+(aq), has a Ka value of 1.2 103. Is this ion a stronger or a weaker acid than Al3+(aq)?
What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
a. The principal equilibrium in a solution of NaHCO3 is HCO3(aq)+HCO3(aq)H2CO3(aq)+CO32(aq) Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between [H2CO3] and [CO32]? c. Using the equilibrium H2CO3(aq)2H+(aq)+CO32(aq) derive an expression for the pH of the solution in terms of Ka1 and Ka2 using the result from part b. d. What is the pH of a solution of NaHCO3?
Boric acid, H3303, is not a Bronsted-Lowry acid but a Lewis acid.. (a) Write an equation for its reaction with water. (b) Predict the shape of the anion thus formed. (c) What is the hybridization 0n the boron consistent with the shape you have predicted?
Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.
Chloroacetic acid, ClCH2CO2H, is a moderately weak acid (Ka=1.40103). If you dissolve 94.5 mg of the acid in water to give 125 ml of solution, what is the pH of the solution?
What is the pH of 2.7 x 10-2 M NaOH(aq)? О 3.6 O 1.6 O 12.4 O 13.1 O 10.4
What is the pH of 7.8 x 10-5 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 О 3.7 O 4.1

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What is the pH of 4.3 x 10-4 M NaOH (aq)? O 17.4 10.6 О 3.4 O -3.4 O 24.6