1)
HNO2 dissociates as:
HNO2 -----> H+ + NO2-
2.5 0 0
2.5-x x x
Ka = [H+][NO2-]/[HNO2]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((4.6*10^-4)*2.5) = 3.39*10^-2
So,
[H+] = x = 3.39*10^-2 M
Answer: 3.39*10^-2
2)
% ionisation = x * 100 / initial concentration
= (3.39*10^-2)*100 / 2.5
= 1.36 %
Answer: 1.36 %
12. Find the [H30') and percent ionization of a 2.5 M HNO, solution according to the equation below. (Hint: Assume...
II. Problem Solving. Show all work, thoroughly and completely Do not omit any steps. No credit will be given for illegible, ambiguous, or unclear work. CIRCLE OR UNDERLINE YOUR FINAL ANSWERS 11. Calculate the pOH and pH of a 0.025 M HF. K, (HF)= 3.0 x 10 (Hint: Assume the change is small) (15 points) 12. Find the [Hj0') and percent ionization of a 2.5 M HNO2 solution according to the equation below. (Hint: Assume the change is small) (15...
Calculate the percent ionization of hydrofluoric acid, HF, in a 0.600 M solution. (K for HF - 6.6 x 10-4) HF(aq) + H2O(l) = H30*(aq) + F(aq) O 3,3% O 42% O 6.0% O 2.1% 9.1%
Question 6 What is the percent ionization for a 0.15 M solution of nitrous acid, HNO2 (K, - 4.6 x 10-)? 0.83% 1.7% 5.5% 100% 0.31%
1. Find the pH and percent ionization of a 1.00M solution of HINO.. For HNO2 pk.-3.34. (10 points) HNO 2 EHT Nož pka=(3,34)-log=-0.524
Find the percent ionization of: a) a 1.05 M HC2H3O2 solution. Ka = 1.79 x 10-5 b.) a 2.50 M HNO2 solution. Ka = 4.60 x 10-4
Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures. View Available Hint(s) nothing % Part B Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures. View Available Hint(s) pH and Percent Ionization of a Weak Base 20 of 22 > A Review Constants Periodic Table The degree to which a weak base dissociates is given by...
Find the percent ionization of a 0.663 M HF solution. The K a for HF is 3.5 × 10 -4
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...
13. Consider the reactions below; H2S(g) + H2O(1) H2S(g) + 2H2O(l) H30'(aq) + HS (ag); K1 - 2.5 x 10 + 2H30 (aq) + (aq); K3 = 6.8 x 10-16 Use the information above to calculate the K for the reaction given below (6 points); HS (aq) + H2O(0) H:0 (aq) + (aq); K = ? 14. Consider the reaction below; 2NO2(g) + 2Cl2 2NOCl2(g) + O2(g) If the equilibrium constant Kat 100°C is 1.5 x 10, calculate its k....
Answer ASAP please!!! 8. Calculate the percent ionization in a 0.56 M aqueous solution of phenol (C6H5OH), if the pH is 5.07 at 25°C (Ka = 1.3 x 10-10). A. 1.5 x 10-3 % B. 1.1 x 10-1 % C. 1.5 x 10-5% D. 2.5 % E. 3.5 x 10-3% [Ni(en)]2+ (aq) + 6 NH3 (aq) 9. What is Keq for the following reaction? [Ni(NH3)]2+ (aq) + 3 en (aq) = Ký [Ni(NH3)4]2+ = 1.2 x 109 K [Ni(en)]2+ =...