What is the ph of a solution of m potassium hydroxide koh a strong base

the next three problems. What is the pH of the solution when 73.87 mL of the 1.521 M KOH are added to the .935 M acetic acid solution? What is the pH of the solution at the equivalence point? What is the pH of the solution when 153.8 mL of the 1.521 M KOH has been added to the .935 M acetic acid solution?

me how you got to the answer please, thanks.

n of iron at the equivalence point? For Fe(III)-EDTA, log Kf = 14.32 and at pH 7, α Y4- =5.0x 10-4 .

titrated with a 0.200 M solution of the base, LiOH. Write the balanced chemical reaction for neutralization reaction: HClO4 (aq) + LiOH (aq) → LiClO4 (aq) + H2O (l) Write the NET ionic equation for the neutralization reaction. OH⁻ (aq) + H⁺ (aq) → H2O (l) Compute the pH of the titration solution. Show your work i) before any of the base is added ii) after 25. mL of base is added iii) after 50. mL of base is added A student performs the titration with the same chemicals but with smaller volumes of each chemical . Which of the following titration curves could represent the titration. Explain A because this entails a strong acid and a strong base. Question 2 A student performs a titration of an unknown acid with a strong base and gets the following titration curve: a) The student consults the list of pKa of acids shown below. If the acid is listed in the table below, which is the most likely identity of the unknown acid? Explain. Acid Ka HF 7.2 x 10-4 CH3COOH 1.8 x 10-5 H2CO3 4.3 x 10-7 HBrO 2.0 x 10-9 The unknown acid is HBrO because the calculated Ka is in between 50^-4 and 50^-6 and 2.0 x 10^-9 lies in between them. b) What is the initial molarity of the acid? 10^-3 = 0.001M Question 3 a) Describe the components and the composition of an effective buffer solution. Explain how the components of the buffer allow the buffer to maintain its pH. An effective buffer solution has a weak acid and its conjugate base or a weak base and its conjugate acid. A buffer solution is most effective when the ratio of its component concentrations is close to 1, also when the pH is equal to the pka of the acid.; The components of the buffer allow the buffer to maintain its pH because buffers can absorb excess H+ions or OH– ions. An employer is interviewing four applicants for a job as a laboratory technician and asks each how to prepare a buffer solution with a pH of 5.0. The following constants may be helpful: hydrazoic acid, pKa = 4.74 Boric acid, pKa = 9.23 Archita A. says she would mix equal molar solutions of hydrazoic (HN3) and sodium azide (NaN3) solutions. Bradley B. says she would mix equimolar Boric acid (H3BO3) and HCl solutions. Carlos C. says he would mix equimolar Boric Acid (H3BO3) and sodium dihydrogen borate (NaH2BO3) solutions. Delia D. says he would mix equimolar hydrazoic Acid (HN3) and NaOH solutions. b) Which of these applicants has given an appropriate procedure? Explain your answer Delia because she is using Sodium hydroxide which results in a pH of 5. NaOH is a strong base and in order to have an effective buffer a weak acid must be incorporated which is the HN3. c) Explain what is wrong with the erroneous procedures. The rest all incorporate a strong acid and a strong base or a weak acid and a weak base which don’ result in an effective buffer. d) The applicants have access to the 1 Liter volumes of each of the solutions listed above. They have access to graduated cylinders. In order to make 1.0 Liter of the correct 5.0 buffer solution, what volumes of the two chemicals must be mixed?

acids from the primary sequence. How might this affect each of the three higher levels of protein structure, thus causing this condition? 2) Imagine that you are building an artificial eukaryotic cell starting with an artificial bacterial cell. What organelles would you need to add? 3)How can an enzyme recognize and bind one specific substrate in a cell containing thousands of different molecules? How will extremes of temperature and pH affect this specificity?

at would have been the concentration of HNO3 AFTER the 0.1000g of Li was added and allowed to react with some of HNO3? (Hint - Lim XS Problem) What would have been the pH of your acid solution after the metal was added?

r litre? What would have been the concentration of HNO3 AFTER the 0.1000g of Li was added and allowed to react with some of HNO3? (Hint - Lim XS Problem) What would have been the pH of your acid solution after the metal was added? If you wanted to fill a rubber balloon to an internal volume of 5.000L and pressure of 140.0kPa in a 25.00C room with hydrogen gas from the reaction of your metal and acid (Li and HNO3), what is the minimum quantity in millilitres of an 8.000M solution of your acid you would need to generate enough hydrogen gas? (assume you have more than enough metal).

after the addition of 16.9 mL of NaOH? (pKa of HNO2 = 3.37)

after the addition of 16.9 mL of NaOH? (pKa of HNO2 = 3.37) Keep 2 decimal places in your answer.

25 M HNO2 (Ka = 5.10 x 10-4)?

at pH does the solution buffer?