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Answer the following for a titration of 25.0 mL of 0.87 M HCN Ka = 4.9...
A titration is performed on a 25 mL sample of 0.15 M HCN (Ka = 4.9 x 10–10) with 0.30 M NaOH. Which of the following is the pH of the solution after 15 mL of NaOH is added?
Consider the titration of a 25.0 mL sample of 0.125 M HCN (Ka= 6.17x10^-10) with a 0.160M KOH. What is the pH after 19.53mL of KOH? What is pH after 21.5mL of KOH?
3) (10 points total) A 25.0-mL sample of 0.35 M HCOOH (formic acid) is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka-1.77 x 10 a) (4 points) What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ks-1.77 x 10 C 2-l04Co1s5 b) (6 points) Calculate at least nine (9) more titration points, build a table...
1. 50.00 mL of 0.1000 M propanoic acid (CH3CH2COOH – Ka = 1.34 X 10-5) is titrated with 0.2000 M KOH. Calculate the pH at the following points in the titration: 1) Initial pH – no KOH has been added. 2) 5.00 mL of KOH has been added. 3) 12.50 mL of KOH has been added. 4) At the equivalence point. (Calculate the volume of KOH to reach the equivalence point & identify a good indicator.) 5) Provide a sketch...
2.) 100.0 mL of a 0.100 M solution of HCN (K,=4.9 10-19) is titrated with a 0.200 M solution of KOH. Calculate the pH of solution iii) Before any addition of KOH solution. (2pts) After the addition of 10.0 mL of KOH solution. (2pts) At the half-equivalence point. (1pt) At the equivalence point. (2pts) After the addition of 100 mL of KOH solution. (1pt)
Consider the titration of a 25.0 mL sample of 0.100 M HCl with 0.200 M KOH. The volume of equivalence is 12.50 mL. (Remember to report pH values with two places past the decimal point.) A)What is the pH of the sample before any KOH is added? B)What is the pH after 9.00 mL of KOH have been added? C)What is the pH at the equivalence volume? D)What is the pH after the addition of 14.0 mL of KOH?
Consider the titration of 25.0 mL of 0.100 M HF with 0.125 M KOH. The Ka is 6.8 x 10-4 for HF. What is the pH after 20.0 mL of base are added? Please show steps.
Consider the titration of a 25.0mL sample of 0.125M HCN (Ka = 6.17x10^-10) with 0.160 M KOH. 1. What is the initial pH? 2. What is the pH at 6.00 mL base added? 3. What is the pH when 19.53 mL of KOH is added? 4. What is the PH if 21.5 mL of KOH is titrated with the solution?
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
Please help me out! Especially part 4! Thank you! Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C. Ka for HCN = 6.2×10-10. Part 1 Calculate the pH after 0.0 mL of KOH has been added. pH = Part 2 Calculate the pH after 50.0 mL of KOH has been added. pH = Part 3 Calculate the pH after 75.0 mL of KOH has been added. pH = Part 4 Calculate the pH...