A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA? [A]...

A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA? [A] HA (aq) + H2O (l) H3O+ (aq) + A- (aq) [B] A- (aq) + H3O+ (aq) HA (aq) + H2O (l) [C] A- (aq) + OH- (aq) HOA2- (aq) [D] A- (aq) + H2O (l) HA (aq) + OH- (aq) [E] HA (aq) + H2O (l) H2A+ (aq) + OH- (aq) Please explain your answer

Expert Solution

queen_honey_blossom answered 2 years ago

The weak acid HA with a dissociation constant Ka is distributed between and organic solvent and...

The weak acid HA with a dissociation constant Ka is distributed between and organic solvent and water. If the only extractable species is the undissociated species HA with a partition coefficient K, derive an expression showing the dependence of the distribution ratio, D, on [H+] of the aqueous phase and draw conclusions from this expression.

Calculate the equilibrium constant for the following reaction of a weak acid and base HClO(aq) +...

Calculate the equilibrium constant for the following reaction of a weak acid and base HClO(aq) + NH3(aq) NH4+(aq) + ClO-(aq) given Ka (HClO) = 2.8 × 10-8, Kb (NH3) = 1.8 × 10-5 and Kw = 1.0 × 10-14.

A certain weak acid, HA, has a Ka value of 7.3

1. The degree to which a weak base dissociates is given by the base-ionization constant, Kb....

1. The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent...

Dissociation Constant For the dissociation reaction of a weak acid in water, HA(aq)+H2O(l)?H3O+(aq)+A?(aq) the equilibrium constant...

Dissociation Constant For the dissociation reaction of a weak acid in water, HA(aq)+H2O(l)?H3O+(aq)+A?(aq) the equilibrium constant is the acid-dissociation constant, Ka, and takes the form Ka=[H3O+][A?][HA] Weak bases accept a proton from water to give the conjugate acid and OH? ions: B(aq)+H2O(l)?BH+(aq)+OH?(aq) The equilibrium constant Kb is called the base-dissociation constant and can be found by the formula Kb=[BH+][OH?][B] When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an...

A 0.30 solution of a weak acid(HA) has a pH of 3.77. What is the Ka?

A certain weak acid, HA , with a Ka value of 5.61×10−6 , is titrated with...

A certain weak acid, HA , with a Ka value of 5.61×10−6 , is titrated with NaOH . Part A: A solution is made by titrating 8.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Part B: More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 71.0 mL ? Express the pH numerically to...

Consider a monoprotic weak acid (HA) that is titrated with a strong base. What is the...

Consider a monoprotic weak acid (HA) that is titrated with a strong base. What is the relationship between the strength of the weak acid and the pH of the solution at the equivalence point? There is no relationship between the strength of the acid and the pH at the equivalence point. The pH at the equivalence point is always 7 in an acid base titration. The weaker the acid, the higher the pH at the equivalence point. The stronger the...

Buffer 1 is created such that the weak acid, HA, is 0.80 M and base, A–...

Buffer 1 is created such that the weak acid, HA, is 0.80 M and base, A– , is 0.80 M. Buffer 2 is created such that the weak acid, HA, is 0.080 M, and base, A– , is 0.080M. Which buffer has the greater buffer capacity? Briefly explain

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A...

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A solution is made by titrating 44.17 mmol (millimoles) of HA and 0.09 mmol of the strong base. Then, more strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 41.7 mL ?

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