Write the acid ionization constants ( also referred to as the equilibrium constant for a weak...

Question

Question

Write the acid ionization constants ( also referred to as the equilibrium constant for a weak acid) for the following reactions:

a. H₂CO₃(aq) + H₂O(l) H₃O⁺(aq) + HCO₃^-(aq)

b. H₂S(aq) + H₂O(l) H₃O⁺ (aq) + HS^-(aq)

c. HC₃H₅O₃ + H₂O(l) H₃O⁺(aq) + C₃H₅O₃(aq)

Answer 1

Answer #1

H₂CO3(aq) + H₂0 (1) - H3O+ (aq) + HCO3(aq) Acid ionization constant (Kal. ka - Iguay [409] & [H₂O(0) = 1 as. [H2CO₃ (19)] [H2

Answer 2

Similar Homework Help Questions

1. Consider the following equilibrium for the dissociation of lactic acid, HC3H5O3 (a weak acid): HC3H5O3...

1. Consider the following equilibrium for the dissociation of lactic acid, HC3H5O3 (a weak acid): HC3H5O3 (aq) + H2O (l) → H3O+ (aq) + C3H5O3- (aq) If the Ka of lactic acid is 1.40E-4, calculate the value of ΔGo (in kJ/mole) for this reaction at 25.0oC.
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3...

The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq)&nb...

The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?

2. For the following reactions, determine the equilibrium constants and whether the reactants or products are...

2. For the following reactions, determine the equilibrium constants and whether the reactants or products are favored: a) HCOOH(aq) + H2O(l) → HCOO− (aq) + H3O + (aq) (To determine K, use [HCOOH] = 0.10 M and [HCOO− ] = [H3O + ] = 0.0042 M) b) H2CO3(aq) + ClO− (aq) → HCO3 − (aq) + HClO(aq) (To determine K, use Ka(H2CO3) = 4.3 × 10-7 and Ka(HClO) = 3.5 × 10-8 ) 3. For each of the above reactions...
Hypobromous acid, HBrO, is a weak acid. The following is the equilibrium constant for its reaction...

Hypobromous acid, HBrO, is a weak acid. The following is the equilibrium constant for its reaction with water: HBrO(aq) + H2O(l) <----------> H3O+(aq) + BrO-(aq) Ka = 2.5 x 10-9 What is the hydronium ion concentration, [H3O+], in a 1.32 M HBrO solution? Note: Assume that the ionization of the acid is small enough in comparison to its starting concentration that the concentration of unionized acid is almost as large at equilibrium as it was originally. This will allow you...
The ionization constant of a very weak acid, HA, is 8.8x10-9. Calculate the equilibrium concentrations of...

The ionization constant of a very weak acid, HA, is 8.8x10-9. Calculate the equilibrium concentrations of H2O, A', and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H30]= mol/L [A] = moll mol/L [HA] = pH =

For 0.030 MM H2CO3H2CO3, a weak diprotic acid, calculate the following values. Use ionization constants of...

For 0.030 MM H2CO3H2CO3, a weak diprotic acid, calculate the following values. Use ionization constants of H2CO3H2CO3: K1=4.4×10−7,K2=4.7×10−11 K1=4.4×10−7, K2=4.7×10−11, as necessary. A) [H3O+][H3O+] Express your answer using two significant figures. B) [HCO−3][HCO3−] Express your answer using two significant figures. C) [CO2−3][CO32−] Express your answer using two significant figures. pH of diprotic weak acid is not given?
A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA...

A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA has a pH of 1.890 at 25°C. HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq) What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =
Hydrosulfuric acid, also known as hydrogen sulfide, is a diprotic acid. Its two-stage ionization is shown...

Hydrosulfuric acid, also known as hydrogen sulfide, is a diprotic acid. Its two-stage ionization is shown below: H2S(aq) ⇆ H + + HS- (aq) Ka1 = 5.70x10-8 HS- (aq) ⇆ H + + S2- (aq) Ka2 = 1.0x 10-9 a. Calculate the concentration of HS- ion in a 0.222 M H2S solution. b. Determine the pH of the solution. c. Determine the S2- concentration. Please write out all answers step-by-step :-)

< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants...

< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants Periodic Table Percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid HA: A certain weak acid, HA, has a Ka value of 4.7x10-7 Percent ionization=1 _HA ionized HA initial x 100% Part A Percent ionization increases with increasing K. Strong acids, for which K, is very large,...