Consider a solution containing 0.40 M HA and 0.40 MA. If HA has a ka of...
Consider a solution containing 1.30 M HA and 0.30 M A . If HA has a K, of 3.90E-3, what would the pH of this solution be? Submit Answer Tries 0/98
Consider a solution containing 1.90 M HA and 0.70 M A. IF HA has a k, of 5.40E-6, what would the pH of this solution be? Submit Answer Tries 0/98 This discussion is closed. Type here to search 09 Sus esc QwO@Ovo
Consider a solution containing 0.40 MHA and 1.30 MA'. If HA has a k, of 6.20E-3, what would the pH of this solution be?
A 0.685 M solution of a weak acid HA has a pH of 4.50. What is the percent ionization of HA in the solution? Submit Answer Tries 0/98 For the solution described above, what is the K,? Submit Answer Tries 0/98 This discussion is closed. Ote E o Type here to search 6
Consider the Ka values for the following acids: Acid ka HA 4.40E-6 HB 7.01E-6 HC 1.24E-5 HD 3.38E-5 HE 1.25E-5 Write the formula for the acid which has the STRONGEST conjugate base. Submit Answer Tries 0/98 What is the corresponding Kb value for the strongest acid from the table above? Submit Answer Tries 0/98
What would the pH of a solution containing 1.11g of an acid HX (Molar Mass of HX = 52.00 g/mol) after the addition of 2.93g of NaX? Assume no volume change to the solution after the addition of the Nax. (HX Ka = 5.48E-4) Submit Answer Tries 0/98
Consider a diporitc acid, HA, where Ka1 = 6.37E-4 and Kay = 8.14E-9. Answer the following questions regarding this solution: If the initial concentration of the acid is 0.57M, what is the pH of the solution? Submit Answer Tries 0/98 What will the concentration of A2-be at equilibrium? Submit Answer Tries 0/98
Consider a titration at 25°C where 0.186 M NaOH is added to 0.107 M HCl. The initial volume of HCl solution is 63 ml. What would the pH be after the addition of 24 mL of NaOH? Submit Answer Tries 0/98 What would the pH be at the equivalence point? Submit Answer Tries 0/98 What would the pH be after the addition of 343 mL of NaOH? Submit Answer Tries 0/98
Consider 55.0 mL of a solution of weak acid HA (Ka = 1.20 × 10-6), which has a pH of 4.250. What volume of water must be added to make the pH = 5.250 ? Volume Submit Answer Try Another Version 1 item attempt remaining
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.