You have collected following information. Volume of the acetic acid (CH3COOH)use for the titration = 2: Morlarity of the NaOH solution = 0.90 M Initial burette reading = 22.82 mL Final burette reading = 45.67 mL

A saturated solution of barium hydroxide is tritrated with 0.0350 M hydrochloric acid. The titration of 15.0 mL of the basic solution required 34.2 mL of the acid solution. Calculate the concentration of the barium hydroxide solution. (plz help i dont get it)

For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is  Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same)  and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.

Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10-⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the solution pH when 10.00 mL of titrant have been added? (Two decimal places) Type your answer...