Given the pressing need for you to understand titration calculations, I have forced another container of NaOH of unknown concentration. You decide to play it safe and use KHP (MW = 204.2 g/mol) as your standardization acid. So, you dissolve 0.114 g of KHP in 35 mL of water. Then, your titration requires 22.33 mL of the unknown NaOH. What is the concetration of the NaOH? Watch your sig figs.

During a titration a 0.30 L sample of H2SO4 requires 569 mL of 2.50 M NaOH to reach the equivalence point. What is the initial concentration of H2SO4? (Do not include units in your answer. If you round during your calculation make sure to keep at least 3 decimal places. Report your answer to 2 decimal places.)

1) If you weigh out 0.2349 g of tris, what volume of the 0.1 M HCI solution will you need to reach the end point of this titration? (Note: this is a nice way to get the approximate volume before starting a titration!) 2) If you weighed out 0.4670 g of KHP, what volume of the 0.1 M NaOH solution will you need to reach the end point of this titration?

25.00 mL of an unknown acidic solution is titrated with 0.198 M NaOH solution. Exactly 22.34 mL of the NaOH solution is needed to reach the equivalence point. What is the concentration of the unknown solution?

Please answer all parts.

A flask contains 0.015 mol of HCl in 10.0mL of solution.  a. What is the molarity of the HCl solution?  b. In a titration with NaOH, how many moles of NaOH will be required to reach the end point?  c. If 12.5 mL of NaOH are required to reach the end point, what is the molarity of the NaOH solution?

Part E: Ammonia. A 0.467 g sample known to contain ammonia is titrated with 0.2791 M HCI. If 38.87 mL is required for the titration, calculate the percent ammonia in this sample.

Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka 2.8 x 10 ) and KOBr and testing its behavior when strong acid or base is added to it. = Part 1 First, Lareina combines 81.42 g KOBr and 245 mL of 1.70 M HOBr, and adds enough distilled water to make 950 mL of solution. What is the pH of this solution? pH solution= Part 2 Next, Lareina adds 12.0 mL of 2.40 M HNO₂ to 385 mL of the solution made in Part 1. What is the pH of the solution after the HNO is added? pH after HNO, added = Part 3 Finally, Lareina 18.0 mL of 2.10 M NaOH ito 375 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added=