For the reaction NO(g) + 1/2 O_2 NO_2(g) at 750 degree C, the equilibrium consta
ID: 1064234 • Letter: F
Question
For the reaction NO(g) + 1/2 O_2 NO_2(g) at 750 degree C, the equilibrium constant K_c, equals 1.0 K (RT)^1/2 K (RT)^-3/2 K_p(RT)^3/2 K_P(RT)^1/2 H_2SO_3(aq) + H_2O(l) H_3O^+(aq) + HSO_3^-(aq) HSO_3^-(aq) + H_2O(l) H_3O^+(aq) + SO_3^2-(aq) In the above reversible reactions, which are the Bronsted acids? H_2SO_3, H_2O, HSO_3^- H_3O^+, H_2O, SO_3^-2 HSO_3^-, H_2O, SO_3^2- H_2O, H_3O^-, HSO_3^- H_2SO_3, H_3O^+, HSO_3^- What is the net ionic equation for the acid-base reaction between nitrous acid and sodium hydroxide? HNO_2(aq) + NaOH(aq) rightarrow NaNO_2(aq) + H_2O(l) H^+(aq) + OH^-(aq) rightarrow H_2O(l) HNO_2(aq) + OH^-(aq) rightarrow NO_2^-(aq) + H_2O(l) H^+(aq) + NO_2^-(aq) + Na^+(aq) + OH^-(aq) rightarrow NaNO_2(aq) + H_2O(l) H^+(aq) + NO_2^-(aq) + Na^+(aq) + OH^-(aq) rightarrow Na^+(aq) + NO_2^-(aq) + H_2O(l) The pH of a 0.013 M ammonia solution is 10.72. What is its hydroxide-ion concentration? 1.5 times 10^-2 M 5.2 times 10^-3 M 5.2 times 10^-4 M 0.72 times 10^-4 M 1.91 times 10^-11 M The hydronium-ion concentration of a 0.050 M lactic acid solution is 2.62 times 10^-3. The acid dissociation constant is 1.37 times 10^-4. The pH of this lactic acid solution is 0.42. 1.30 2.58. 3.86. 5.94. Calculate the pH of a 0.017 M Ba(OH)_2 solution. 0.034 1.47 1.77 12.13 12.53 A 0.10 M solution of a weak monoprotic acid has a pH of 3.30. What is the equilibrium constant, K_a, for this acid? 5.0 times 10^-3 5.0 times 10^-4 2.5 times 10^-5 2.5 times 10^-6 2.5 times 10^-7 A solution that is formed by combining 400. mL of 0.20 M HNO_3 with 600. mL of 0.10 M NaOH has an H_3O^+ concentration of 0.20 M. 0.l0 M. 0.060 M. 0.020 M. 5.0 times 10^-13. What is the pH of a 0.03 M solution of benzoic acid (K_a = 6.6 times 10^-5)? 0.5 2.9 4.2 9.3 9.8Explanation / Answer
For the reaction NO(g)+1/2 O2(g)--> NO2 (g) at 750K, the equilibrium constant Kc equals
[A] 1.0.
[B] Kp(RT)3/2.
[C] Kp(RT)–3/2.
[D] Kp(RT)2/3
. [E] Kp(RT)1/2.-------------ANSWER
==================================================
H2so4 (aq) +H2O -----H3o +Hso3
In the above reversible reactions , which are bronsted acids
H2SO3 ,------ acids
H3O,--------- acids
=================================================
NET IONIC REACTION NITROUS ACID ANDSODIUM HYDROXIDE
HNO2 +OH -------NO2 +H20
molecular equation
HNO2(aq) + NaOH(aq) --> NO2-(aq) + H2O(l) + Na+(aq)
this is the ionic equation
HNO2(aq) + Na+(aq) + OH-(aq) --> NO2-(aq) + H2O(l) + Na+(aq)
this is the net ionic equation
HNO2(aq) + OH-(aq) --> NO2-(aq) + H2O(l) --------------answer
===================================================
The pH of a 0.015 M ammonia solution is 10.72. What is its hydroxide-ion concentration?
a. 1.5 x 10^-2 M
b. 5.2 x 10^-3 M
c. 5.2 x 10^-4 M ------------answer
d. 0.72 x 10^-4 M
e. 1.91 x 10^-11 M
pH + pOH = 14.00.
Since the pH is 10.72, that makes the pOH 3.28.
Since pOH is the -log[OH-], we find 10^-3.28 to get the concentration of OH-.
This comes out to be 5.2 x 10-4, or C
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.