answer number 40, a and c with all work shown,
the ka value for HF us 3.5 x 10^-4
answer number 40, a and c with all work shown, the ka value for HF us...
Use the Henderson-Hasselbalch equation to calculate the pH of each solution (Express all answers in two decimal places) A) a solution that is 0.155 M in propanoic acid and 0.110 M in potassium propanoate B) a solution that contains 0.620% C5H5N by mass and 0.900% C5H5NHCl by mass C) a solution that is 16.5 g of HF and 27.0 g of NaF in 125 mL of solution. PART A) Ka for propanoic acid is 1.3x10^-5
I need a, b and c please. Thanks! Use the Henderson-Hasselbalch equation to calculate the pH of each solution: Part A a solution that is 0.155 M in propanoic acid and 0.125 Min potassium propanoate Express your answer using two decimal places. VO ALTRO? pH = Submit Request Answer Part B a solution that contains 0.715% C, H N by mass and 0.865% CsHNHCl by mass Express your answer using two decimal places. V AED RO? pH- Submit Request Answer...
Use the Henderson-Hasselbalch equation to calculate the pH of each of the following solutions. A. a solution that contains 0.800% C5H5N by mass and 0.950% C5H5NHCl by mass (where pKa=5.23 for C5H5NHCl B. a solution that has 17.0 g g of HF and 27.0 g g of NaF in 125 mL m L of solution (where pKa=3.17 for HF acid)
i already know they answer please explain your solutions Ka for CH3COOH = 1.8x10^-5 pka i calculated 4.74 ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...
Use the Henderson–Hasselbalch equation to calculate the pH of each solution: Part B a solution that contains 0.775% C5H5N by mass and 0.950% C5H5NHCl by mass. ( Express your answer using two decimal places.) Part C a solution that is 12.0 g of HF and 22.5 g of NaF in 125 mL of solution (Express your answer using two decimal places.) - Calculate the pH of the solution that results from each of the following mixtures. Part A4 150.0 mL...
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small amount of nitric acid is added the pH only slightly drops. Write the chemical equation that shows the added nitric acid being neutralized by this buffer. 2. What is the pH of a buffer that is 0.120 M formic acid (HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic acid is 1.8 x 10^ -4 . 3. The curve shows the...
Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that contains 0.695% C5H5N by mass and 0.845% C5H5NHCI by mass Express your answer using two decimal places. Hν ΑΣφ ? рH- 15.2 Previous Answers Request Answer Submit Incorrect; Try Again; One attempt remaining Part C a solution that is 13.5 g of HF and 24.0 g of NaF in 125 mL of solution Express your answer using two decimal places. ΑΣφ ? pH Request Answer Submit
Use the Henderson-Hasslebalch equation to calculate the pH of each solution: (Express your answer using two decimal places) Part A) A solution that contains 0.620% C5H5N by mass and 0.900% C5H5NHCl by mass (Kb for C5H5N is 1.7 x 10^-9) Part B) A solution that is 16.5 g of HF and 27.0 g of NaF in 125 mL of solution (Ka for HF is 3.5x10^-4)
Please answer #2 php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your work. Don't forget the significant figures and units!! Would the following mixtures result in buffer solutions? (Justify your answers) 1. a 100.0 ml, of 0.10 M NH, 100.0 mL of0.15 M NHaCl b. 50.0 mL of 0.10 M HCIO4, 35.0 mL if 0.15 M NaCIO c. 125.0 ml, of 0.15 CH?NH2. 120.0 mL of 0.25 M CHNE ICI d. 165.0 mL of 0.10 M...
Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL. measured pH 0.0 20 Did the pH change a little or a lot when NaOH was added to the butter? Was the change you observed consistent with the action of a butter? For the ammonium chloride-ammonia buffer give the measured pH for the 50.0 mL of 0.10 Mammonia. Is this solution acidic, neutral, or basic? Did the pH of the ammonia increase or decrease...