question 28 QUESTION 27What is the pH of a buffer solution that is made of 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONA)? (Ką = 6.5 × 10-3 for benzoic acid)C6HSCO2H(aq) + H20(aq) 2 C6H5CO0'(aq) + H3O*(aq)QUESTION 28A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NAOH. What is the pH of the solution after 30.00 mL of NAOH have been added to the acid?HBr(aq) + NaOH(aq) → NaBr(aq) + H2O(aq)QUESTION 29MgCl2 are added dropwise to a 1.2 M NaF solution. The minimun concentration of MgCl2 needed to to initiate a precipitate of magnesium fluoride isM. [Ksp(M|F2) = 6.9 x 10-91X10-9MGF2(s) S Mg-(aq) + 2F(aq)

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Chapter16: Acid-base Equilibria

Section: Chapter Questions

Problem 16.142QP: K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic...

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K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic acid with 46.1 mL of 0.182 M sodium acetate. Calculate the pH of this solution at 25C after the addition of 5.82 mL of 0.125 M NaOH.
4.Suppose polyprotic acid H3X with Ka1=10-2, Ka2=10-5, Ka3 =10-10 . Answer the following questions for the buffer of 150 ml 0.1 M NaH2X and 50 ml 0.02 M Na2HX A) What is pH?B) Is the reverse reaction H2X-+ + H2O → H3X + OH- significant in determination of pH and why?C)Is the forward reaction HX2- + H2O → X3- + H3O+ significant in determination of pH and why?(Please do not use Henderson Hasselbalch equation!) Need answer for all three subparts Will definitely appreciate your efforts. Thank you.
What is the pH of the buffer that results when 12.0 g of NaH2PO4, and 8.00 g of Na2HPO4 are diluted with water to a volume of 0.50 L? (Ka of H2PO4– = 6.2 ×× 10–8, the molar masses of NaH2PO4 and Na2HPO4 are 120.0 g/mol and 142.0 mol, respectively) Group of answer choices 4.10 6.96 7.21 7.46 9.90
A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation
a student is preparing a Lactic acid (HLac) buffer (Ka= 1.4 X 10-4 , PH=4.00) answer the following questions: A. how many moles of conjugate base should be added to 315 mL of 0.45 M HLac to give a PH of 4.00? B. what is the ratio of the concentration of HLac to its conjugate base?
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. 150 gr/mol b. 200 gr/mol c. 100 gr/mol d. 50 gr/mol
Be sure to answer all parts.What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.16 M C6H5COOH and 0.46 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures.[H3O+] = _____pH = ______
What mass of sodium acetate must be added to 1.25 L of 1.12 M acetic acid to make a buffer solution whose pH=5.80? Ka of acetic acid is 1.8×10-5, MCH3CO2Na =82.04g/mol Question options: 230 g 23.0 g 1.3x103 g 130 g
Given: The pH of the buffer is 4.88 made by combining 0.500 L of 0.380 M HC3H5O2 (Ka=1.30X10-5) and 0.500 L of 0.380 M NaC3H5O2. 0.040 moles of NaOH were added to the buffer. a. total moles of HC3H5O2 in the solution? b. total moles of NaC3H5O2 in the solution?
From their Kb values, which of the following bases would be best for preparing a buffer of pH 9.00: (i) NH3 (ammonia, Kb = 1.8 3 1025), (ii) C6H5NH2 (aniline, Kb = 4.0 3 10210), (iii) H2NNH2 (hydrazine, Kb = 9.5 3 1027), (iv) C5H5N (pyridine, Kb = 1.6 3 1029)?
Cacodylic acid (dimethylarsinic acid, (HAsO2(CH3)2) is a common buffer used in biology to prepare and fix biological samples. It has a pKa value of 6.30. Calculate the pH of a buffer solution prepared by mixing 10.0 ml of 0.200 M NaOH woth 20.0 ml of 0.150 M cacodylic acid. Express answer on two decimal places.
Given: The pH of the buffer is 4.88 made by combining 0.500 L of 0.380 M HC3H5O2 (Ka=1.30X10-5) and 0.500 L of 0.380 M NaC3H5O2. 0.040 moles of HNO3 was added to the buffer. a. total moles of NaC3H5O2 in the solution? b. total moles of HC3H5O2 in the solution?

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