Write the expression for the K₂ for each of the following reactions H₂CO3 + H₂O <-> H3O+¹ + HCO3-¹ [ ][ Ka [ H₂CO3 + 2 H₂O <-> 2 H3O+1 + CO3² 1²[ Ka [ a. acetic b. hydrochloric c. phosphoric d. perchloric g. sulfurous h. hydrosulfuric i. OH-1 -2 n. HPO3-² 0. H₂PO3-1 p. CO3² q. HCO3-1 u. H2O v. H₂CO3 = j. H30+1 r. H₂S k. SO4² e. hydrofluoric 1. Mg+2 S. HS-1 t. S-2 f. sulfuric m. C-1

Write the expression for the K₂ for each of the following reactions H₂CO3 + H₂O <-> H3O+¹ + HCO3-¹ [ ][ Ka [ H₂CO3 + 2 H₂O <-> 2 H3O+1 + CO3² 1²[ Ka [ a. acetic b. hydrochloric c. phosphoric d. perchloric g. sulfurous h. hydrosulfuric i. OH-1 -2 n. HPO3-² 0. H₂PO3-1 p. CO3² q. HCO3-1 u. H2O v. H₂CO3 = j. H30+1 r. H₂S k. SO4² e. hydrofluoric 1. Mg+2 S. HS-1 t. S-2 f. sulfuric m. C-1

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 81E: In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C)...

See similar textbooks

Similar questions

. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calcul the concentration of H+ if the initial concentration of acid is 0.100 M. d Q4- How many grams of sodium hydroxide (M.wi=58.5) can be added 0 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changi POH by more than lunit? Ky=1.8x 10°? w
At 25oC, a 100mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of the solution is 1.05g/cm3. If this solution is diluted further to form 700mL, what will be the A) [OH-], B) pH and C) % dissociation of the resulting acetic acid solution? CH3COOH -> H+ + CH3COO- (Kb = 5.56x10-10)
Selenic acid, H2SeO4, is a diprotic acid that actually is a strong acid for the donation of its first proton and has a pKa2 = 1.7. What will be the Ka and the chemical equation for showing the donation of the second proton? (hint: products will be H3O+ and SeO42-) I take 2.00 g the pure compound and dilute it to 100.0 mL of solution. Find the initial concentration and use two ICE tables to show the equilibrium concentrations of [H3O+], [OH-], [HSeO42-] and [SeO42-]. What will be the concentration of H2SeO4? (hint: no math is necessary here as this is a strong acid).
What will happen to the pH of a 2.0 HF solution (pH=1.42, Ka=7.23x10^-4) if you added some NaF to it? Explain how you came to this conclusion and why this happens.
5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach?9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)
NH3 is a weak base. It ionizes in water to produce NH4+ and OH-. Its Kb = 1.8  10-5 and Kw = 1  10-14 at 25oC. Please complete following tasks for a solution of 0.0500 M NH3 (aq) at 25oC. (a) ionization % of NH3, (b) pH of this solution, (c) concentration of OH- ; and (d) concentration of NH4+
Write the equations that represent the first and third ionization steps for phosphoric acid (H3PO4) in water. (Use H3O+ instead of H+.) first ionization step: + H2O(l) + third ionization step: + H2O(l) + --- The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-? --- The value of Ka for nitrous acid is 4.50×10-4.What is the value of Kb, for its conjugate base, NO2-?
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____
At 25oC, a 50mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of the solution is 1.05g/cm3 . If this solution is diluted further to form 500mL, what will be the: A) [OH- ] B) pH C) % dissociation of the resulting acetic acid solution?
What mass of NaA (MW=100 g/mole) must be added to a 100.0 ml of a 0.1 M solution of HA (Ka=1x10-5) to achieve a pH of 6.0?