I have a 50.0 mL sample of a solution of hydrocyanic acid, HCN, of unknown concentration. I titrate the HCN solution with a stock solution of 10.0 M LİOH. I reach endpoint when 6.50 mL of LIOH solution have been added. What is the original concentration of my HCN solution? (Canvas is stupid and won't let you enter all the sig figs - it's ok)

I have a 50.0 mL sample of a solution of hydrocyanic acid, HCN, of unknown concentration. I titrate the HCN solution with a stock solution of 10.0 M LİOH. I reach endpoint when 6.50 mL of LIOH solution have been added. What is the original concentration of my HCN solution? (Canvas is stupid and won't let you enter all the sig figs - it's ok)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A buffer solution contains 1.2 M sodium benzoate and 1.5 M benzoic adic. K, for benzoic acid is 6.3 x 10-5. Correct! Calculate the pH of this buffered solution. pH = 4.10 eTextbook and Media Hint Attempts: 1 of 3 used 0.10 mol NaOH(s) is mixed with 1L of the above buffered solution. What reaction happens? (Benzoic acid is C6H5COOH(aq).) The reaction equation should be written with states and charges of all reactants/products. Save for Later Attempts: 0 of 3 used Submit Answer
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)?The Ka for HOCl is 3.0 x 10-8 M. (the answer is 3.96) Please I really need these questions below answered they have to do with the above question. What is the pH after 6.40 mL of NaOH are added? What is the pH at the equivalence point? What is the pH after 11.00 mL of NaOH are added? What is the pH after 14.10 mL of NaOH are added? What is the pH when half the acid has been neutralized?
How would the volume of base needed to perform the KHP titration have changed if a solution of 0.100 M barium hydroxide was used instead of the sodium hydroxide solution?
Make sure answer has correct significant di
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCl is 3.0 x 10-8 M.(THE ANSWER IS 4.96) I DONT NEED THIS ABOVE QUESTIONS DONE!!!! THE QUESTIONS BELOW RELATE TO IT THOUGH!!!! What is the pH after 4.80 mL of NaOH are added? What is the pH at the equivalence point? What is the pH after 9.80 mL of NaOH are added?
:(((((((/////
I need help please.
please help w/ 7 a,b,c,d
Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH;COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH,COOH is 1.8 x 10. NEXT > Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq) + H2O(1) H,O (aq) CH;COO (aq) Initial (M) Change (M) Equilibrium (M)
Incorrect Your answer is incorrect. • KC: Your answer is incorrect. • Cacl, Vour answer is incorrect. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll ind K, data in the ALEKS Data tab. Does enlubility change with pH? hiyhest solubility compound pll 5 pll 6 pll 8 yes O no yes Ba(OH), O no O yes Caci, e no
Solve the same way as shown