Question 3 (2 points) Saving. • Calculate the pH of 0.0040 M butanoic acid, which is...
Question 6 (2 points) Calculate the pH of 0.0080 M butanoic acid, which is a monoprotic acid; Ka=1.52 x 10-5. Assume that the 5% approximation rule applies. Provide your answer to two places after the decimal. Your Answer: Answer
Question 12 (2 points) ✓ Saved Calculate the pH of a solution labelled 0.73 M ammonia, NH3(aq), which is a weak monoprotic base. Kb(NH3) = 1.8 x 10-5. Use the 5% approximation rule. Provide your answer to two places after the decimal. Your Answer: Answers
Calculate the [H+) and pH of a 3.75 x 10-4 M butanoic acid solution. The K, of butanoic acid is 1.52 x 10-5. M pH =
Calculate the (H+) and pH of a 2.55 x 10-4 M butanoic acid solution. The Ką of butanoic acid is 1.52 x 10-5. 0.000063246 M pH = 4.1989
Calculate the [H+] and pH of a 0.000143 M butanoic acid solution. Keep in mind that the Ka of butanoic acid is 1.52 x10-5. this is a problem that will require you to use the quadratic. Start by setting up the quadratic equation before using the quadratic formula and find the coefficients. Then solve the quadratic. Quadratic formula:ax2+bx+c=0; enter the values of a, b, and c a= b= c= [H+]= M pH=
7) Calculate the K, of butanoic acid (monoprotic) if a 0.025 M aqueous solution has a pH of 3.21 at 25°C 8) trans-cinnamic acid (C,H,O, monoprotic) has a K = 3.60 x 10-5 a. Calculate the pH of a 0.020 M aqueous solution of this acid. b. Calculate the percentage of acid dissociated (i.e., in the "A" form) in this solution using your calculations in (a). CHEM 120B-Activity #3 Acids and Bases Page 5
Question 6: Postlecture 11 A 1.45 L buffer solution consists of 0.189 M butanoic acid and 0.302 M sodium butanoate. Calculate the pH of the solution following the addition of 0.066 moles of NaOH . Assume that any contribution of the NaOH to the volume of the solution is negligible. The ?a of butanoic acid is 1.52×10−5 . pH=
A 1.37 L buffer solution consists of 0.153 M butanoic acid and 0.326 M sodium butanoate. Calculate the pH of the solution following the addition of 0.071 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 x 10-5. pH =
A 1.41 L buffer solution consists of 0.154 M butanoic acid and 0.280 M sodium butanoate. Calculate the pH of the solution following the addition of 0.068 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-5. pH =
A 1.35 L buffer solution consists of 0.115 M butanoic acid and 0.331 M sodium butanoate. Calculate the pH of the solution following the addition of 0.079 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-5. pH =