4. When the weak acid HN; (K4 = 1.9 x 10-) is dissolved in water, which...
How do you do these problems? I got all of them wrong and
don't understand why.
- 10. Which of the changes will increase the value of K, for the reaction? 2 SO2(g) + O2(g) - 2 SO3(g) AH = -200 kJ/mol A. Lowering the temperature B. Increasing the pressure (CCAdding 02 D. Removing SO, 3. Which reaction describes why the pH is not 7 for the dissolution of NaNO2 in water? ADNa+ + 2 H2O = NaOH + H2O*...
3.
Determine the concentration of [H3O+] and the pH of a solution
0.025M of hydrozoic acid, HN3-. (PICTURE WITH ADDITIONAL INFO
BELOW)
4. Determine the pH of a solution 0.125M of hydroxilamine,
HONH2. (PICTURE WITH ADDITIONAL INFO BELOW)
3. Determine la concentración de [H3O+] y el pH de una solución 0.025M de ácido hidrazoico, HN3. HN, (g) + H20 (1) = H30+ + N3 K = 1.9 x 10-5 4. Determine el pH de una solución 0.125 M de hidroxilamina,...
33. A monoprotic weak acid when dissolved in water is 0.36% dissociated and produces a solution with a pH of 3.10. Calculate the Ka of the acid. SHOW WORK!!! A) 3.6 × 10–3 B) 2.2 × 10–1 C) 2.9 × 10–6 D) Need to know the initial concentration of the acid. E) None of these.
D Question 23 4 pts When a 0.100 mol of a pure compound is dissolved in 1.0 L of water, the solution pH changes from 7.00 to 4.24. Which of the following is most likely the identity of the substance? A weak base A neutral salt A weak acid A strong base A strong acid Question 24 4 pts If the hydronium ion concentration, [H30*), in a solution is 5.6x10-10 M, what is the hydroxide ion concentration, [OH"), and the...
9. When a weak base such as ammonia, NH3, is dissolved in water, what are ALL the species that exist in solution. Rearrange your list from the highest concentration to the lowest concentration. (Hint: H2O has the highest concentration) 10. In question 9, how many unknowns (don't count water) are there and how many equations are needed to determine the concentrations of those unknowns?
please answer both questions
QUESTION 8 The compound ammonia, NH3, is a weak base when dissolved in water. Which of the following is the correct equation for the reaction of ammonia in water? a NH3(aq) + H20(0) NH4(aq) + OH(aq) NH3(aq) + OH(aq) NH2 (aq) + H20(0) NH3(aq) + H20(1) -NH2 (aq) + H30*(aq) NH3(aq) + H200) NH2 (aq) + H30(aq) NH3(aq) + H30aq) NH4+ (aq) + H20(0) QUESTION 9 What is the pH of a solution that is 0.17...
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...
Question 3 (2 points) Which of the following is considered a weak acid when dissolved in water? c) H2SO3 b) HF a) HNO2 A) a only B) c only C) All of them D) b only E) None of them
If a buffer solution is 0.240 M in a weak acid (K4 = 4.6 x 10-5) and 0.510 M in its conjugate base, what is the pH? pH =
a)
b)
c)
d)
If the Kb of a weak acid is 2.9 10*, the K, of its conjugate acid must be which of the following? 2.9.10 6.46 7.54 3.4 10- The hydronium ion concentration of a 0.50 mol/L solution of hydrocyanic acid, HCN(aq), is 1.4 x 10-5 mol/L. Use Weak Acid Info 16.1 to answer the following question. The Ka for hydrocyanic acid is: 3.9 x 10-10 1.4 x 10-5 5.0 x 10-2 6.2 x 10-10 An acetic acid-sodium...