HNO2 has an acid dissociation constant of Ka = 4.0 x 10-4

Question

Question

HNO₂ has an acid dissociation constant of K_a = 4.0 x 10^-4. What is the pH of a 0.25 M NO₂^- solution?

a. 2.00 b. 4.30 c. 8.40 d. 10.25 e. 14.00

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Given the following acid dissociation constants, Ka (HNO2) = 4.0 x 10-4 Ka (HCN) = 4.0...

Given the following acid dissociation constants, Ka (HNO2) = 4.0 x 10-4 Ka (HCN) = 4.0 x10-10 determine the equilibrium constant for the reaction below. HCN(aq) + NO2 - (aq) CN- (aq) + HNO2(aq)
If nitrous acid (HNO2) has a Ka 4.0 x10-4 at 25 degrees C, what is the...

If nitrous acid (HNO2) has a Ka 4.0 x10-4 at 25 degrees C, what is the percent dissociation of nitrous acid in a 0.40 M solution?
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate...

You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate the concentration of HNO2 and its conjugate base in a 0.025 M HNO2 Solution. Please please show all work!

What is the pH of a 0.35 M solution of NO2-? (Ka of HNO2 = 4.0...

What is the pH of a 0.35 M solution of NO2-? (Ka of HNO2 = 4.0 x 10-4) 7.32 8.47 5.53 9.86 4.16
Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the...

Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the pH of a solution that contains 1.0 M KNO2(aq) and 0.50 M HNO2(aq).
For the following equation: The Ka value of HNO2 is 4.0 x 10-4. If the equilibrium...

For the following equation: The Ka value of HNO2 is 4.0 x 10-4. If the equilibrium concentration of HNO2 is 0.54 M. what is the equilibrium concentration of NO2/H30? 2 points HNO, + H, O NO + H20+ Your answer

#4 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11....

#4 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.061 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.14 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
a) An unknown indicator (called “HIn”) has a Ka of 4.0 x 10-6. The color of...

a) An unknown indicator (called “HIn”) has a Ka of 4.0 x 10-6. The color of the neutral form is green, and that of ionized form is red. The indicator is added to a HCl solution, which is then titrated against a NaOH solution. At what pH will the indicator change color? b) 350. mL of a NaOH solution was added to 500. mL of 2.50 M HNO2. The pH of the mixed solution was 1.75 units greater than that...
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4)...

Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M

IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10)...

IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10) solution is titrated with 0.200 M NaOH. Find the pH before titration and after 25 mL, 50 mL, and 60 mL of NaOH has been added.