The Kaof HCN is 4.9 x 10-10
You combine the following solutions:
i. 250 mL of 0.500 M NaClO4
ii. 250 mL of 0.450 M KCN
iii. 125 mL of 0.625 M KI
iv. 125 mL of 0.580 M NaBr
--> What is the pH of the final solution?
The Kaof HCN is 4.9 x 10-10 You combine the following solutions: i. 250 mL of...
Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.170 in KCN. For HCN, Ka= 4.9 x 10^-10 (pKa = 9.31). Use both the equilibrium approach and the Henderson-Hasselbalch approach.
!!!!!!!!!!!!!!! Ka HCN: 4.9 x 10^-10 !!!!!!!!!!!!!!!!!! 8. (10 points) Determine the pH of a 1.50 M Sodium Cyanide (KCN) solution. Be sure to show the 5% check.
A chemistry graduate student is given 125. mL of a 0.90 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with Ka = 4.9 10 -10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.44? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to...
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)
Calculate the volumes of 0.200 M hydrocyanic acid, HCN (Ka = 4.9 x 10–10) solution, and 0.200 M of sodium cyanide, NaCN, solution needed to prepare 100.0 mL buffer solution with pH = 9.5
Calculate the pH of a 1.2 M HCN solution. Ka = 4.9 x 10 ^-10 for HCN (would appreciate if you wrote it down on a piece of paper so I don't get confused by the math)
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?
Answer the following for a titration of 25.0 mL of 0.87 M HCN Ka = 4.9 x 10-10) with 0.39 M KOH. a.) The pH when 10.0 mL of KOH has been added. (6pts) b.) The pH at the equivalence point. (9pts)
Would the following solutions provide an effective buffer. a) 250. mL of 0.15 M HC2H3O2 + 25 mL of 0.10 M NaOH yes no b) 125 mL of 0.50 M HNO2 + 75 mL of 0.40 M KNO2 yes no c) 250. mL of 0.25 M HCO2H + 125 mL of 0.50 M KOH yes no d) 250. mL of 0.50 M HClO4 + 150. mL of 0.50 M NaClO4 yes no e) 250. mL of 0.50 NaOH + 500....
5. [10 pts] Rank the following 10 solutions from lowest pH to highest Rhe i. 2.0 M hydrochloric acid ii. 5.0 M hydrochloric acid iii. 3.0 M sodium hydroxide iv. 2.0 M calcium hydroxide v. 2.0 M hydrofluoric acid vi. 2.0 M very weak base vii. 50.0 mL of deionized water viii. After 50.0 mL of Solution I is titrated with 50.0 mL of Solution 11 ix. After 50.0 mL of Solution I is titrated with 50.0 mL of Solution...