2 3 4 Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the initial solution pH (when 0.00 mL of titrant have been added) (Two decimal places) Type your answer... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH (when 15.00 mL of titrant have been added? (Two decimal places) Type your answer.... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH at the equivalence point? (Two decimal places) Type your answer.... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH when 30.00 mL of titrant have been added? (Two decimal places) Type your answer... D D 100

In the video, what is the color of universal indicator in the most basic solution? What is (chemical name and formula) of the chunk of solid stuff added to the solution? What acid is produced when dry ice is added to water? Is this acid produced a weak or strong acid? According to the video, what is the approximate pH of a yellow solution with the universal indicator? Video is https://www.youtube.com/watch?v=iK_CCa5ZMKg&t=1s

Question 6 of 36 Retry A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H;NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10-10. 1 2 NEXT > Let x represent the original concentration of C6H5NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H;NH2(aq) + H20(1) ОН (ад) + CgH;NH;*(aq) Initial (M) 0.50 Change (M) Equilibrium (M) -1.6 x 10 10 Incorrect, 2 attempts remaining Your Initial concentration for C,H5NH3* is incorrect. Revisit the problem statement to determine the initial concentration of acid or base. Also, make sure that your values are in the correct concentration units, not mass or moles! Your Change in concentration for C6H5NH2 is incorrect. In this problem, you should use the given pH to determine the concentration of H3O* or OH at Equilibrium as appropriate. From there, you should be able…

I know it's a lot, but I would really appreciate some help!