Homework Answers
ANSWER 11.A :-
ANSWER 11.B :-
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answer 11a and 11b
11. The initial pH of a 0.2M arginine solution is 14. a....
13. Calculate the pH when 35mL of 0.5M ammoni 0.2M hydrochloric acid. HICI= 208,2 nmole NH32...
13. Calculate the pH when 35mL of 0.5M ammoni 0.2M hydrochloric acid. HICI= 208,2 nmole NH32 35X0.5= 17.5 moles pOH = pk bt log bolt=4,76+ log bolt = 4.23 salt base in 13 ,5 NH3t HCl - NHACI Initial 17.5 u final 13,5 - wean bast salt Basic Buffer pH = 14-4.23 = 9.76 14. Sketch the titration curve when 35mL of 0.5M ammonia (K5=1.8x10^-5) is titrated with 0.2M hydrochloric acid.
1) NaOH(aq) + HCl(aq) - NaCl(aq) + H2O(1) To determine the concentration of a NaOH(aq) solution,...
1) NaOH(aq) + HCl(aq) - NaCl(aq) + H2O(1) To determine the concentration of a NaOH(aq) solution, a student titrated a 50. mL sample with 0.10 M HCl(aq). The reaction is represented by the equation above. The titration is monitored using a pH meter, and the experimental results are plotted in the graph below. 13. 0S 7.04 Answer Key on School Loop @ P 1.07. 0 25.0 50.0 Volume HCI added (mL) One student titrated the NaOH(aq) with 1.0 M HCl(aq)...
36. Use the following titration curve to answer the following 14 pH 30.0 10.0 20.0 Volume...
36. Use the following titration curve to answer the following 14 pH 30.0 10.0 20.0 Volume of titrant added (mL) a) What type of sample is being titrated (Be specific)? b) What is the pH at the equivalence point(s) c) What is the Kai and Ka2 for this sample d) What pH region(s) would this make a suitable buffer? e) What was the initial concentration of the sample that would provide this curve? (USE Kal)
You are asked to make one litre of 0.2M Tris-CI buffer pH 8.8, using Tris base and IM hydrochlori...
You are asked to make one litre of 0.2M Tris-CI buffer pH 8.8, using Tris base and IM hydrochloric acid. a) given the MW of Tris is 121.1, how much Tris would you weigh out to make one litre of b) what is the ratio of [Tris base] to [Tris acid] in the final buffer solution? (pKa of Tris is c) what is the total concentration of Tris (i.e. Tris base form+Tris acid form) in the final 0.2M Tris-Cl buffer?...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
25 mL of 0.080 M solution of ammonia was titrated with 0.10 M HCl solution until...
25 mL of 0.080 M solution of ammonia was titrated with 0.10 M HCl solution until the pH attained "saturation value". Draw the titration curve illustrating dependence between pH and volume of the HCI solution. Give the required answers in the boxes provided. Ko of NH3 = 1.8 x 10-5 Give initial pH value (must be correct within 0.5 pH unit) .... pH Circle whether the pH value at the equivalence point is lower than 7, equal to 7 or...
6-8 Uruudlit added 5. On your titration curve in 4, clearly label the equivalen buffering is...
6-8
Uruudlit added 5. On your titration curve in 4, clearly label the equivalen buffering is occurring. Use Option to answer questions 6-8 *. clearly label the equivalence point and any region in which o. Draw the Lewis structure of the acid and mark the acidic hydrogen with an ). acid and mark the acidic hydrogen with an asterisk H- 7. Draw a Lewis structure of the conjugate base of the acid. 8. Suppose the acid is neutralized with a...
-e-laboratory Assignment Name: ead the experiment and answer the following questions as directed by your instructor...
-e-laboratory Assignment Name: ead the experiment and answer the following questions as directed by your instructor A student is performing a titration. Diagrams of the buret at the beginning and the end of the titration are shown at right. To the correct number of significant figures, what is the initial volume, the final volume, and the volume of solution added during the titration? 16 2) Formic acid (HCOOH) is a weak acid with K. - 1.8 x 10-4. a) Write...
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution...
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of a titration of 50.00 of 0. 20 x 10-2) with NaOH solution. If the quadratic equa e accurate, what would the percent error in the pH if the simple equation were used to calculate the phine of 50.00 of 0.005M HA quadratic equation is assumed to the simpler (square root) 4. According to Figure 19.1 at which point(s) ABCD on the titration curve does...
13. Calculate the pH when 35mL of 0.5M ammoni 0.2M hydrochloric acid. HICI= 208,2 nmole NH32 35X0.5= 17.5 moles pOH = pk bt log bolt=4,76+ log bolt = 4.23 salt base in 13 ,5 NH3t HCl - NHACI Initial 17.5 u final 13,5 - wean bast salt Basic Buffer pH = 14-4.23 = 9.76 14. Sketch the titration curve when 35mL of 0.5M ammonia (K5=1.8x10^-5) is titrated with 0.2M hydrochloric acid.
1) NaOH(aq) + HCl(aq) - NaCl(aq) + H2O(1) To determine the concentration of a NaOH(aq) solution, a student titrated a 50. mL sample with 0.10 M HCl(aq). The reaction is represented by the equation above. The titration is monitored using a pH meter, and the experimental results are plotted in the graph below. 13. 0S 7.04 Answer Key on School Loop @ P 1.07. 0 25.0 50.0 Volume HCI added (mL) One student titrated the NaOH(aq) with 1.0 M HCl(aq)...
36. Use the following titration curve to answer the following 14 pH 30.0 10.0 20.0 Volume of titrant added (mL) a) What type of sample is being titrated (Be specific)? b) What is the pH at the equivalence point(s) c) What is the Kai and Ka2 for this sample d) What pH region(s) would this make a suitable buffer? e) What was the initial concentration of the sample that would provide this curve? (USE Kal)
You are asked to make one litre of 0.2M Tris-CI buffer pH 8.8, using Tris base and IM hydrochloric acid. a) given the MW of Tris is 121.1, how much Tris would you weigh out to make one litre of b) what is the ratio of [Tris base] to [Tris acid] in the final buffer solution? (pKa of Tris is c) what is the total concentration of Tris (i.e. Tris base form+Tris acid form) in the final 0.2M Tris-Cl buffer?...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
25 mL of 0.080 M solution of ammonia was titrated with 0.10 M HCl solution until the pH attained "saturation value". Draw the titration curve illustrating dependence between pH and volume of the HCI solution. Give the required answers in the boxes provided. Ko of NH3 = 1.8 x 10-5 Give initial pH value (must be correct within 0.5 pH unit) .... pH Circle whether the pH value at the equivalence point is lower than 7, equal to 7 or...
6-8
Uruudlit added 5. On your titration curve in 4, clearly label the equivalen buffering is occurring. Use Option to answer questions 6-8 *. clearly label the equivalence point and any region in which o. Draw the Lewis structure of the acid and mark the acidic hydrogen with an ). acid and mark the acidic hydrogen with an asterisk H- 7. Draw a Lewis structure of the conjugate base of the acid. 8. Suppose the acid is neutralized with a...
-e-laboratory Assignment Name: ead the experiment and answer the following questions as directed by your instructor A student is performing a titration. Diagrams of the buret at the beginning and the end of the titration are shown at right. To the correct number of significant figures, what is the initial volume, the final volume, and the volume of solution added during the titration? 16 2) Formic acid (HCOOH) is a weak acid with K. - 1.8 x 10-4. a) Write...
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of a titration of 50.00 of 0. 20 x 10-2) with NaOH solution. If the quadratic equa e accurate, what would the percent error in the pH if the simple equation were used to calculate the phine of 50.00 of 0.005M HA quadratic equation is assumed to the simpler (square root) 4. According to Figure 19.1 at which point(s) ABCD on the titration curve does...
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