Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 14, Problem 75E
The pH of a 0.15-M solution of HSO4- is 1.43. Determine Ka for HSO4- from these data.
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Chapter 14 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 14 - Write equations that show NH3 as both a conjugate...Ch. 14 - Write equations that show H2PO4- acting both as an...Ch. 14 - Show by suitable net ionic equations that each of...Ch. 14 - Show by suitable net ionic equations that each of...Ch. 14 - Show by suitable net ionic equations that each of...Ch. 14 - Show by suitable net ionic equations that each of...Ch. 14 - What is the conjugate acid of each of the...Ch. 14 - What is the conjugate acid of each of the...Ch. 14 - Identify and label the Bronsted-Lowry acid, its...Ch. 14 - Identify and label the Bronsted-Lowry acid, its...
Ch. 14 - What are amphiprotic species? Illustrate with...Ch. 14 - State which of the following species are...Ch. 14 - State which of the following species are...Ch. 14 - Is the self-ionization of water endothermic or...Ch. 14 - Explain why a sample of pure water at 40 C is...Ch. 14 - The ionization constant for water (Kw) is 2.91014...Ch. 14 - The ionization constant for water (Kw) is...Ch. 14 - Calculate the pH and the pOH of each of the...Ch. 14 - Calculate the pH and the pOH of each of the...Ch. 14 - What are the pH and pOH of a solution of 2.0 M...Ch. 14 - What are the hydronium and hydroxide ion...Ch. 14 - Calculate the hydrogen ion concentration and the...Ch. 14 - Calculate the hydronium ion concentration and the...Ch. 14 - The hydronium ion concentration in a sample of...Ch. 14 - The hydroxide ion concentration in household...Ch. 14 - Explain why the neutralization reaction of a...Ch. 14 - Explain why the neutralization reaction of a weak...Ch. 14 - Use this list of important industrial compounds...Ch. 14 - The odor of vinegar is due to the presence of...Ch. 14 - Household ammonia is a solution of the weak base...Ch. 14 - Explain why the ionization constant, Ka, for H2SO4...Ch. 14 - Explain why the ionization constant, Ka, for HI is...Ch. 14 - Gastric juice, the digestive ?uid produced in the...Ch. 14 - Nitric acid reacts with insoluble copper (II)...Ch. 14 - What is the ionization constant at 25 C for the...Ch. 14 - What is the ionization constant at 25 C for the...Ch. 14 - Which base, CH3NH2 or (CH3)2NH, is the stronger...Ch. 14 - Which is the stronger acid, NH4+ or HBrO?Ch. 14 - Which is the stronger base, (CH3)3N or H2BO3-?Ch. 14 - Predict which acid in each of the following pairs...Ch. 14 - Predict which compound in each of the following...Ch. 14 - Rank the compounds in each of the following groups...Ch. 14 - Rank the compounds in each of the following groups...Ch. 14 - Both HF and HCN ionize in water to a limited...Ch. 14 - The active ingredient formed by aspirin in the...Ch. 14 - What do we represent when we write:...Ch. 14 - Explain why equilibrium calculations are not...Ch. 14 - Are the concentrations of hydronium ion and...Ch. 14 - What two common assumptions can simplify...Ch. 14 - What two common assumptions can simplify...Ch. 14 - Which of the following will increase the percent...Ch. 14 - Which of the following will increase the percent...Ch. 14 - What is the effect on the concentrations of NO2-,...Ch. 14 - What is the effect on the concentration of...Ch. 14 - Why is the hydronium ion concentration in a...Ch. 14 - From the equilibrium concentrations given,...Ch. 14 - From the equilibrium concentrations given,...Ch. 14 - Determine Kb for the nitrite ion, NO2-. In a...Ch. 14 - Determine Ka for hydrogen sulfate ion, HSO4-. In a...Ch. 14 - Calculate the ionization constant for each of the...Ch. 14 - Calculate the ionization constant for each of the...Ch. 14 - For which of the following solutions must we...Ch. 14 - Even though both NH3 and C6H5NH2 are weak bases,...Ch. 14 - Calculate the equilibrium concentration of the...Ch. 14 - Calculate the equilibrium concentration of the...Ch. 14 - Calculate the equilibrium concentration of the...Ch. 14 - Calculate the equilibrium concentration of the...Ch. 14 - Using the Ka value of , place Al(H2O)63+ in the...Ch. 14 - Calculate the concentration of all solute species...Ch. 14 - Propionic acid, C2H5CO2H (Ka=1.34105), is used in...Ch. 14 - White vinegar is a 5.0% by mass solution of acetic...Ch. 14 - The ionization constant of lactic acid,...Ch. 14 - Nicotine, C10H14N2, is a base that will accept two...Ch. 14 - The pH of a 0.20-M solution of HP is 1.92....Ch. 14 - The pH of a 0.15-M solution of HSO4- is 1.43....Ch. 14 - The pH of a 0.10-M solution of caffeine is 11.16....Ch. 14 - Tile pH of a solution of household ammonia, a...Ch. 14 - Determine whether aqueous solutions of the...Ch. 14 - Determine whether aqueous solutions of the...Ch. 14 - Novocaine, C13H21O2N2Cl, is the salt of the base...Ch. 14 - Which of the following concentrations would be...Ch. 14 - Calculate the concentration of each species...Ch. 14 - Calculate the concentration of each species...Ch. 14 - Salicylic acid, HOC6H4CO2H, and its derivatives...Ch. 14 - The ion HTe- is an amphiprotic species; it can act...Ch. 14 - Explain why a buffer can be prepared from a...Ch. 14 - Explain why the pH does not change significantly...Ch. 14 - Explain why the pH does not change significantly...Ch. 14 - What is [H3O+] in a solution of 0.25 M CH3CO2H and...Ch. 14 - What is [H3O+] in a solution of 0.075 M HNO2 and...Ch. 14 - What is [OH-] in a solution of 0.125 M CH3NH2 and...Ch. 14 - What is [OH-] in a solution of 1.25 M NH3 and 0.78...Ch. 14 - What concentration of NH4NO3 is required to make...Ch. 14 - What concentration of NaF is required to make...Ch. 14 - What is the effect on the concentration of acetic...Ch. 14 - What is the effect on the concentration of...Ch. 14 - What will be the pH of a buffer solution prepared...Ch. 14 - Calculate the pH of a buffer solution prepared...Ch. 14 - How much solid NaCH3CO23H2O must be added to 0300...Ch. 14 - What mass of NH4Cl must be added to 0.750 L of a...Ch. 14 - A buffer solution is prepared from equal volumes...Ch. 14 - A 5.36-g sample of NH4Cl was added to 25.0 mL of...Ch. 14 - Which acid in Table 14.2 is most appropriate for...Ch. 14 - Which acid in Table 14.2 is most appropriate for...Ch. 14 - Which base in Table 14.3 is must appropriate for...Ch. 14 - Which base in Table 14.3 is most appropriate for...Ch. 14 - Saccharin, C7H4NSO3H, is a weak acid (Ka=2.1102)....Ch. 14 - What is the pH of 1.000 L of a solution of 100.0 g...Ch. 14 - Explain how to choose the appropriate acid-base...Ch. 14 - Explain why an acid-base indicator changes color...Ch. 14 - Why can we ignore the contribution of water to the...Ch. 14 - Why can we ignore the contribution of water to the...Ch. 14 - Draw a curve for a series of solutions of HF. Plot...Ch. 14 - Draw a curve similar to that shown in Figure 14.23...Ch. 14 - Calculate the pH at the following points in a...Ch. 14 - The indicator dinitrophenol is an acid with a Ka...
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- Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NO2 (g) = N2O4(g) AGº = -5.4 kJ Now suppose a reaction vessel is filled with 4.53 atm of dinitrogen tetroxide (N2O4) at 279. °C. Answer the following questions about this system: Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to '2' rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO 2 needed to reverse it. Round your answer to 2 significant digits. 00 rise ☐ x10 fall yes no ☐ atm G Ar 1arrow_forwardWhy do we analyse salt?arrow_forwardCurved arrows are used to illustrate the flow of electrons. Using the provided starting and product structures, draw the curved electron-pushing arrows for the following reaction or mechanistic step(s). Be sure to account for all bond-breaking and bond-making steps. H H CH3OH, H+ H Select to Add Arrows H° 0:0 'H + Q HH ■ Select to Add Arrows CH3OH, H* H. H CH3OH, H+ HH ■ Select to Add Arrows i Please select a drawing or reagent from the question areaarrow_forward
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