0.1 molar NaCl solution
Identify the acid and base which reacted to form NaCl. Identify
each as strong or weak.
Acid: __________________ Strength:_________ Base:
__________________ Strength:_________
Calculate the theoretical pH of the solution. Show your work. If
appropriate, write out the hydrolysis reaction equation.
. Measure the pH of the aqueous solution and determine the
experimental Kh.
pH of solution: _________
Experimental Kh: ____________
a) How does the theoretical pH correspond to the experimental
pH?
b) List two factors which could cause this discrepancy.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
0.1 molar NaCl solution Identify the acid and base which reacted to form NaCl. Identify each...
0.1 molar NaC2H3O2 solution Identify the acid and base which reacted to form NaC2H3O2. Identify each as strong or weak. Acid: __________________ Strength:_________ Base: __________________ Strength:_________ Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. . Calculate the theoretical Kh value. Show your work. Measure the pH of the aqueous solution and determine the experimental Kh. Show your work. pH of solution: _________ Experimental Kh: ____________ . a) How does the...
61.8% Tools F 8. Sign 0.1 molar NH4Cl solution 20. Identify the acid and base which reacted to form NH CI Identify each as strong or weak. Acid: Strength: Base: Strength 21. Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. 22. Calculate the theoretical Kh value. 23. Measure the pH of the aqueous solution and determine the expenmental K. Show your work. pH of solution Experimental K. 24. How does...
multi photo exp # on last photo Acid-Base Properties of Salt Solutions Worksheet 1. What is a salt? How is it formed? 2. What is pK, and what does it represent? How does this value correspond to the strength of an acid? 3. What is pK, and what does it represent? How does this value correspond to the strength of a base? 4. How is pH affected by the concentration of a solution? 5. What does Kw represent? How is...
pullions? If not, Record your ILIUM suggest a reason for the discrepancy. Hydrolyzes? Parent Acid Strength Parent Acid Parent Base Parent Base Strength Salt (Yes or No? Which ion? Predicted Acidity Experimental Acidity: Bromothymol Blue Test NH4Cl HCI Strong NH3 weak yes: NH4 hydrolyzes acidic NaNO3 Na2CO3 NaCl (NH4)2SO4 NaHCO3 NaF NaC2H302 Al2(SO4)3 Table 5: Hydrolysis of Salts
7) 0.1 N NaOAc (salt of a strong base and a weak acid) Questions: Which salt solutions give acidic solutions? Titration of a weak base with a strong acid gives the salt of the weak base. Which indicator should be used? Which salt solutions give virtually neutral solutions according to your estimates? *Titration of a strong acid with a strong base yields a solution of their respective salts. Which indicator should be used?Which salt solutions give basic solutions? Titration of a weak acid with a strong...
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). Question options: a) pH= 7.00 b) pH= 5.28 c) pH = 4.56 d) pH= 4.74
10. The formation of complex ions causes the solubility of a slightly soluble solid to: A increase B. decrease C. stay the same D. none of the above 11. The equivalence point of a titration occurs: A. when all of the analyte has been titrated (reacted B. usually just before the endpoint. C. Both A and B D. Neither A or B 12. How does a buffer resist change in pH upon addition of a strong acid? A) The strong...
Salt of a Weak Base and a Strong Acid. pH of Solution. Calculate the pH of a 1.19 M aqueous solution of triethylamine hydrochloride ((C2H5)3NHCI) (For triethylamine, (C2H5)3N, Kb = 4.00x 10-4.) Give two decimal places in your answer.
What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 30.0 mL of 0.1 M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points? In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence...
A solution of a weak base is titrated with a solution of a standard strong acid. The progress of the titration is followed with a pH meter. Which of the following observations would occur?