Two aliquot of a water sample is titrated against a strong acid using phenolphthalein and bromocresol green indicator. The volume for the bromocresol green endpoint is 18.7 mL and for phenolphthalein endpoint is 18.7 mL, what is/are the probable source of alkalinity? Section а. OH- b. OH and CO,- с. СО, d. HCO; 2-

Two aliquot of a water sample is titrated against a strong acid using phenolphthalein and bromocresol green indicator. The volume for the bromocresol green endpoint is 18.7 mL and for phenolphthalein endpoint is 18.7 mL, what is/are the probable source of alkalinity? Section а. OH- b. OH and CO,- с. СО, d. HCO; 2-

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

What is the pH at 110.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with Kp = (7.58x10^-9)) with 0.200 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
A buffered solution containing dissolved aniline, C, H,NH₂, and aniline hydrochloride, C, H,NH, Cl, has a pH of 5.64. A. Determine the concentration of CH, NH3 in the solution if the concentration of C, H,NH, is 0.230 M. The pK, of aniline is 9.13. [CH_NH;] = ApH: = B. Calculate the change in pH of the solution, ApH, if 0.351 g NaOH is added to the buffer for a final volume of 1.65 L. Assume that any contribution of NaOH to the volume is negligible. 7.5 7.45 x10-5 Incorrect Incorrect M
Calculate the volume in mL of 0.311 M KOH necessary to titrate 23.38mL of 0.342 M diprotic sulfuric acid, H2SO4 to a phenolphthalein end-point. Report your answer to a precision of 2 decimal places.
1. Calculate what pH should be for Mg2+ at 1.31 x 10-2 concentration. (Mg(OH)2(s)<-> Mg2+ (aq) + 2OH-(aq)) 2. Then calculate the percent error of the pH level of pH=10.60 to the theoretical pH of the first question.
10. What chemical species, besides water, is present in the highest concentration in an aqueous solution of the weak base (CH3)2NH? 11. In each of the following pairs, identify the stronger acid and state a reason for your answer: H2PO, HPO, HNO2 HNO3 PH3 NH3 H2SO4 H2SEO4 PH3 H2S 12. In each of the following pairs, circle the solution that would have the lower pH 0.100 М НСI 0.100 м НС2НЗО2 0.100 М НСI 0.200 М НСI 0.100 M HC2H;O2 (Ka = 1.8 x 10) 0.100 M HCIO3 (Ka = 5.0 x 10) 0.100 M HC2H3O2 (Ka = 1.8 x 10) 0.100 M HC2H3O2 mixed with 0.100 M NaCzH3O2 %3D 13. It took 32.15 mL of 0.200 M NaOH to titrate 1.50 g of an unknown acid, HA. Calculate the molar mass of HA.
0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein end point. What is the molar mass of the acid? ½ H2A (aq) + KOH (aq) --> ½ K2A (aq) + H2O (l) Molar mass of KOH: 56 gr/mol a. 100 gr/mol b. 150 gr/mol c. 200 gr/mol d. 50 gr/mol
7.5mL of 333mM Tris was added to 192.5ml of water. The resulting solution was added to 240mL of water and the pH was adjusted to 8.0 using 10mL of HCl. A further 33.3mL of water was added. What is the concentration of the final solution (in millimolar)? The MW of Tris is 121.14
50.00 mL of 0.100 M CH;COOH is being titrated with 0.100 M of NaOH. What is the pH at the equivalence point? K, of CH3COOH is 1.8 x 105. Upload your work in order to receive credit.
Kindly explain why, thank you!
The pK, values for the dibasic base B are pKi = 2.10 and pk2 = 7.49. %3! Calculate the pH at each of the points in the titration of 50.0 ml. of a 0.55 M B(aq) solution with 0.55 M HCI(aq). What is the pH before addition of any HCI? pH What is the pH after addition of 25.0 ml. HCI? pH = What is the pH after addition of 50.0 mL HC? pH What is the pH after addition of 75.0 mlL HCI? pH = What is the pH after addition of 100.0 ml. HCI? pH =
I don’t understand this problem. Please help.
A solution witha volume of 1.00 Lis 0.350 M in CH3COOH(aq) and 0.450 M in CH3COONA(aq). What will the pH be after 0.0400 mol of HCl is added to the solution? Ka for CH3COOH(aq) = 1.80 x 10 OA. 4,94 OB. 9.23 C.4.77 D.9.06 E. 4.85