. Predict the direction in which the equilibrium will lie for the reaction
NO2- (aq) + HClO3(aq) <----> HNO2(aq) + ClO3- (aq) Ka(HNO2) = 4 X 10-4
A) reactants will be favored
B) products will be favored
C) cannot be determined
D) reactants and products will be equally favored
E) depends on Kb values which are not given.
Ka = 4.0 x 10-4
means Ka is small.
if Ka is small equilibrium lie towards reactants. means more reactants presents compared to products.
answer = option A = reactants will be favoured.
. Predict the direction in which the equilibrium will lie for the reaction NO2- (aq) +...
For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq) Drag the appropriate stresses to their respective bins. Adding NH4+(aq) Adding NH3(g) Adding OH-(aq) Removing NH4+(aq) Removing OH-(aq) Shifts in the direction of the reactants: Shift in the direction of the products:
(a) Predict which direction the reaction will proceed when an aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. (b) Give reason H3PO4(aq) + NO2-(aq) = H2PO4-(aq) + HNO2(aq) (H3PO4K21 = 7.2x10-3, K22 = 6.3x10-8, K23 = 4.2x10-13, HNO2 Ka1 = 7.1X104)
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2 k1? NH4+ + H2O -> H3O+ + NH3. ka = 5.6 x 10^-10 NO2- + H2O -> HNO2 + OH- kb =2.2 x 10^-11 2H2O -> H3O+ + OH- kw = 1.0 x10^-14 Write symbolic expression for equilibrium constants for each reaction. Derive expression for k1 in terms of ka, kb, and kw; find numerical value of k1.
Predict the direction in which the equilibrium will lie for the following reaction: C_6H_5COO^- + HF C_6H_5COOH + F^- K_a (C_6H_5 COOH) = 6.5 Times 10^ - 5; K_a (HF) = 7.1 Times 10^ - 4 Which of the following yields a basic solution when dissolved in water? NH_3, Na_2O LiOH CO_2 1 and II 1 and III 1, III, and IV 1, II, and III 1, II, III, and IV Calculate the pH of a 6.7 Times 10^-2 M...
The equilibrium constant for the reaction HNO2 (aq) + H2 O ( ℓ) ↔ NO2¯ (g) + H3O+ (aq) is 4.3 x 10 − 4 at 25º C. Will nitrous acid spontaneously dissociate when: a) [HNO2] = [NO2¯] = [H3O + ] = 1.0 M ? b) [HNO2] = 1.0 M and [NO2¯ ] = [H3O + ] = 1.0 x 10− 5 M ? Please help solve this question and include the process as well. Thanks.
Question 11 3 pts Predict the direction in which the equilibrium will lie for the following reaction: H2SO3 + HCO3 ---> HSO + H2CO3 K, H2SO3 -1.0 x 102 K, H2CO3.4.2x107 to the right to the left In the middle
Question 9 (1 point) Predict the direction in which the equilibrium will lie for the following reaction. HCI + - HI+ CI O) to the right O) to the left O) in the middle
H2CO3 + NO2- <--> HCO3- + HNO2 Identify the base and conjugate acid, and predict which side of equilibrium is favored.
NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC (a) Calculate G if the P(NO2) = 0.29 atm, and P(N2O4) = 1.6 atm. (b) Predict the direction in which the reaction will shift to reach equilibrium. Explain how you determined this. (c) Once equilibrium is reached are there more reactants or products present. Explain how you determined this.
Question 9 From the equilibrium concentrations given, calculate Ka and Kb HNO2:[H30*) = 0.011 M; (NO2"] = 0.0438 M; [HNO2] = 1.07 M. Show work. Only putting an answer will be worth 1 point. B IV AA- IE *3 2 1 x X, - EV GOTT 12pt Paragraph E -