Please answer all the questions #1. HA is a weak acid. an aqueous solution of HA...
QUESTION 7 HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0 °C. The Ka of HZ is _ 1.2 x 10-5 6.9 x 10-9 1.4 x 10-10 9.9 x 10-2 2.8 x 10-12
A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA has a pH of 1.890 at 25°C. HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq) What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =
Just give me the answers 14) A0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pHi of 5.35. The value of Kg for HA is A) 14 10-10 B) 7.1 10-9 E) 33 104 918-10-5 D) 3.0 10-5 15) The Kg for HON is 49-10-10, What is the value of Kb for CN-? A) 49-10-24 B) 20 10-5 D) 4.9-104 9 4.0 10-6 E) 2.0 109 16) Caleulate the pOH of a 0.0827 M aqueous...
The weak acid HA has a Ka of 1.80×10−5. If a 1.9 M solution of the acid is prepared, what is the pH of the solution?
Question 1 : HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M. Question 2 : We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA. Question 3 : We place 0.661 mol of a weak acid, HA,...
Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has a pH of 4.39. What is the Ka of the acid?
Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has a pH of 4.39. What is the Ka of the acid?
A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions: a) What is the equilibrium constant (Ka) for the dissociation of this acid? b) What is the pH of the solution? c) How much ‘weaker’ in active acidity of the HA solution compared to 0.2 M HCl solution? d) How many mls of 0.1 M NaOH would be needed to neutralize completely 250 ml of the 0.2 M HA solution?
Consider a weak acid "HA". What is the pH of a 0.853 mol L-1 solution of HA? The KA of HA is 6.32 x 10-6
What is the pH of a 500 mL aqueous solution containing 0.25 mol of a weak acid, HA, and 0.23 mol of its conjugate base, A-? Ka (HA) = 4.8*10^-7