(a) What is the pKbof NO2−?
(
Ka of nitrous acid is 7.1
×
10−4
)
pKb=
(b) What is the pKaof
the hydrazinium ion,
H2N-NH3+?
(
Kb of hydrazine = 8.5
×
10−7
)
pKa=
a) HNO2 ka = 7.1 x 10-4
pKa = - log Ka = - log [7.1 x 10-4] = 3.15
pKa + pKb = 14
pKb = 14 - 3.15
pKb = 10.85
b) NH2-NH2 = Kb = 8.5 x10-7
pKb = - log Kb = - log [8.5 x 10-7] = 6.07
pKb + pKa = 14
pKa = 14 - 6.07
pKa = 7.93
What is the pKa of the hydrazinium ion, H2N-NH3+? Kb of hydrazine = 8.5*10^-7
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−] in 0.54 M HNO2?
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
Ka for nitrous acid, HNO2, is 4.50×10-4. Ka for hydrofluoric acid, HF, is 7.20×10-4. Ka for hydrocyanic acid, HCN, is 4.00×10-10. What is the formula for the strongest conjugate base? ______?____
A certain acid has pKa = (7.997x10^0). What is the acid's Ka? (Ka, Kb, pKa, and pKb are unitless quantities.)
Be sure to answer all parts. Nitrous acid, HNO2, has a K of 7.1 x 10-4. What are [4,0*], [No, ], and (OH) in 0.53 M HNO, [H30+] - [NO2 ] - [OH] = x 10 M (Enter your answer in scientific notation.)
. The Ka of nitrous acid is 4.0 × 10−4. What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M nitrous acid and 45.0 mL of 1.25 M sodium nitrite? The answer is 3.45 Please show the solution. Thank you.
A solution of nitrous acid, HNO2 is 6.3x10^-3 M, which is a weak acid with Ka=7.2x10^-4. Calculate: [HNO2] [NO2] pH What is the concentration of a nitrous acid solution with a pH of 2.21
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
The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to reference(Pages 833 - 836) Section19.7 while completing this problem. Part A Write the chemical equation for the equilibrium that corresponds to Ka. Write the chemical equation for the equilibrium that corresponds to . H+(aq)+NO2−(aq)⇌HNO2(aq) HNO2(aq)⇌H+(aq)+NO2−(aq) HNO2(aq)⇌H−(aq)+NO2+(aq) HNO2(aq)+H+(aq)⇌H2NO2+(aq) HNO2(aq)+H−(aq)⇌H2NO2+(aq) Part B Using the value of Ka, calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. Express your answer using three significant figures. ΔG∘...