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- Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____QUESTION 4 Of the following solutions, which has the lowest buffering capacity? OA.0.212M HF and 0.667M NaF OB. 0.821M HF and 0.217M NaF OC. 0.821M HF and 0.909M NaF OD. They are all buffer solutions and would all have the same capacity. OE. 0.100M HF and 0.217M NaF
- For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)Give answer all questions with explanation please30. Indicate the FALSE statement about pH indicators and their use in titrations: A) A pH indicator suitable for titrations of strong bases with strong acids cannot be used for titrations of strong acids with strong bases. B) pH indicators should be used sparingly (in small amounts) as they are weak acids/ bases, and thus could affect the volume of titrant used. C) An indicator should be selected such that its pKits value matches the equivalence point pH. D) pH indicators all contain at least one acidic group that can be deprotonated to form a differently colored conjugate base. E) The colours of the acid and base forms of a given pH indicator depend on their chemical structures.
- 1[References] Use the References to access important values if needed for th Which of the following aqueous solutions are good buffer systems? 0.36 M barium iodide + 0.29 M calcium id lide 0.19 M hydrocyanic acid + 0.19 M potassium cyanide 0.20 M sodium hydroxide + 0.27 M sodium bromide 0.29 M ammonia + 0.36 M barium hydroxide 0.27 M perchloric acid + 0.23 M potassium perchlorate Submit Answer Try Another Version 1 item attempt remainingculate the pH during the titration gent. The Ka of acetic acid is 1.75x105. 801031 1801031/ A) 10.00 C) 191801031 of 50.00 191801031 191801031 19 E) 8.73 191801031 1 m of 0.100 M acetic acid with 0.1000 M sodium hydroxide at 25°C after the addition of 25.00 mL of 191801031 91801031 191801031 191801031 191801031 191801031 191801031 031 191801001 031 191801031 191801031 101801031 031 191801031 191801031 191801031 191801031 191801031 101801031 (91801031 101801031 191801031 191801031 191801031 191801031 191801031 191801031 191801031 19180103 191801031 101001031 191801031 191801031 181801031 191801031 181801004 391 191301051 19
- The pH value of titration of formic acid ( weak acid ) and ammonium hydroxide ( weak base ) at end point must be 7 False O TrueThe pH curve produced by titrating boric acid with sodium hydroxide will have __________ equivalence points. 0 1 2 3 4 Which of the following would not be in the expression for K for the neutralization of aqueous acetic acid with aqueous sodium hydroxide? acetic acid sodium hydroxide sodium acetate water all of these would be in the expression for K What mass in grams of nitric acid is present in 700 mL of a solution with a pH of 1.866? 0.600 9.52 0.0185 1.22 0.00954 In which of the following solutions will hydrochloric acid ionize less than in pure water? potassium chloride sodium nitrate ammonium bromide lithium phosphate sodium carbonatitration of acetic acid: what is the pH after 10.00mL sodium hydroxide solution are added? the mL base needed to reach equivalence point: 25.5 mL