4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that were susceptible to degradation if their pH was not maintained at a certain level. [a.] Engr. Baylon prepared the buffer for the product that requires a pH of around 4.0 by mixing 0.225 M of phosphoric acid and 0.414 M of sodium dihydrogen phosphate [b.] 0.640 M of ethanolamine, HOC,H,NH, were mixed with 0.750 M of its chloride salt, HOC,H¼NH3CI, by Engr. Samonte for the alkali goods that requires a pH of 9.5 max. Are the prepared buffers solutions applicable for their intended use? Take the acid ionization constant of phosphoric acid of ethanolamine is 2.68x10-5 be 7.1x10-3 while the base ionization constant

4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that were susceptible to degradation if their pH was not maintained at a certain level. [a.] Engr. Baylon prepared the buffer for the product that requires a pH of around 4.0 by mixing 0.225 M of phosphoric acid and 0.414 M of sodium dihydrogen phosphate [b.] 0.640 M of ethanolamine, HOC,H,NH, were mixed with 0.750 M of its chloride salt, HOC,H¼NH3CI, by Engr. Samonte for the alkali goods that requires a pH of 9.5 max. Are the prepared buffers solutions applicable for their intended use? Take the acid ionization constant of phosphoric acid of ethanolamine is 2.68x10-5 be 7.1x10-3 while the base ionization constant

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 0.471 M KHC0; and 0.349 M Na,CO3. Determine the pH change when 0.106 mol KOH is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =|
A buffer solution that is 0.320 M in HCIO and 0.320 M in KC10 has a pH of 7.46. The addition of 0.01 mol of OH to 1.0 L of this buffer would cause the pH to The capacity of this buffer for added OH could be increased by the addition of 0.121 mol| Submit Answer Retry Entire Group 4 more group attempts remaining
I need both solutions......
Calcium Benzoate: a) A sample of saturated CaBz2 solution is at equilibrium. The initially-prepared concentrations are [Ca?+]; = A and [Bz]; =B. This sample is allowed to saturate, and then the remaining solid is filtered out. As determined by titration, the final benzoate ion concentration in solution is [Bz]:= C. What is the solubility product of CaBz2, in terms of A, B, and C?| b) In our lab experiment, the CaBz2 solution is saturated at equilibrium before titration. Why must the CaBz2 solutions be saturated?
e and le akeCovakiAcivity dolorntor asinnment-take [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution contains 0.305 M NH,CI and 0.338 M NH3 (ammonia). Determine the pH change when 0.089 mol KOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change = Submit Answer Retry Entire Group 1 more group attempt remaining erevs Next ENG 令 D US Home End Areert & 7 8
Example sample of BaCl2 25ml, 40 ml of a standard solution Silver Nitrate 0.1M was added to it, the excess Silver was titrated with a standard solution of ammonium thiocyanate 0.098M, and it was found that 15 ml sufficient to precipitate the silver. What is the weight of barium chloride in the solution?
The pH of a Buffer containing 1.OM CH3COOH and 0.1M CH3COONA (pka of * :CH3COOH =4.74) is 3.0 4.74 3.74 5.74
At what pH will FelO0, precipitate from a 0.06000 M Fe" solution? K 2800x10 At what pH will HgIOH); precipitate from a 0.06000 M Hg" solution? K 3.100x1o Which hydroxide precipitates at a lower OH concentration? Choose one O HelOH) 2 O Cannot be determined U Cannot be determinea In a solution buffered to a pH of 3.00, what is (Fe"VIHg" Is the separation of Hg" from Fe" "complete" in a solution buffered to a pH of 3.00? Choose one: O Yes O No O Cannot be determined
2. A precipitate of Pbl, is formed when 5 mL of 0.012 M Pb(NO,), is added to 5 mL of 0.030 M KI. It was found experimentally that the final concentration of I in the 10 mL solution after equilibrium was 8 x 10³M a) How many moles of Pb?* are originally in the solution? b) How many moles of I' are originally present? c) How many moles of I´ remained in solution after equilibrium?
Consider the buffer pair, HCHO,/NaCHO,. What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted to 3.90 and the pK, for HCHO2 equals 3.74? This buffer solution contains equal concentrations of HCHO, and NaCHO O This buffer solution contains relatively more NACHO, than HCHO, More information is needed to determine the relative proportion of each member. This buffer solution contains relatively more HCHO, than NaCHO,.
The buffers had a strong base added so that they both reach equivalence point. Buffer F has 100mL of 0.01M to it while Buffer G has 2.1mL of 0.5M NaOH. Determine the buffer capacity in moles for both buffers AND indicate which is stronger.
A buffer solution contains 0.487 M CH,NH,Cl and 0.252 M CH,NH, (methylamine). D the pH change when 0.058 mol KOH is udded to 1.00 Lof the buffer. etemine pH ater addition - pli before addition- pH change-( Submit Answer Retry Entire Group more group attempts remaining Determine the pHi change when 0.080 mol HCIO, is added to 1.00 Lof a buffer solution that is 0.340 M in CH,COOH and 0.283 M in CH,COO". pH after addition - pH before addition pl change -[ Submit Answer Retry Entire Group 9 more group attempts remaining