A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+(aq) + A'(aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, Ka? Answer in scientific notation. Answer: A...
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+ (aq) + A (aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, K ? Answer in scientific...
Consider a weak acid "HA". What is the pH of a 1.055 mol L-1 solution of HA? The KA of HA is 1.73 x 10-7 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
A 0.250 M solution of a weak acid HA has a pH of 3.10. What is the percent ionization of HA in the solution? For the solution described above, what is the Ka?
A 0.020 M solution of a weak acid HA has a pH of 3.50. What is the percent ionization of HA in the solution? For the solution described above, what is the Ka?
What is the pH of a 0.0013 M Ca(OH)2 solution? Answer to 2 decimal places. A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) ↔ H+(aq) + A-(aq) A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is...
A weak monoprotic acid, HA dissociates by 1.300 % and has a pH of 2.15. Calculate the Ka value for the acid HA. Record your answer in scientific notation to 3 sig figs. Preview
What is the pH of a 0.44 M solution of a weak acid HA, with a Ka of 3.19×10−12? The equilibrium expression is: HA(aq)+H2O(l)⇌H3O+(aq)+A−(aq)
A .175 M weak acid solution has a pH of 3.25. Calculate the Ka for the acid. (hint your answer should contain three significant figures and be written in scientific notation ex. 4.67E-2 )
What is the pH of a 6.85 × 10−3 M weak acid solution, HA, if Ka = 4.5 × 10−6? Group of answer choices 1.2 4.8 9.1 3.8 6.5 What is the pOH of 4.50 × 10−4M HBr? Group of answer choices 10.7 6.7 1.7 12.3 3.3 What is the pH of a 9.67 × 10−3M solution of NaOH? Group of answer choices 13.0 4.6 12.0 9.4 2.0 A 6.5 × 10-2 M solution of a weak acid, HA, has...