The same HCl solution from #1 was used to titrate 20.00 mL of an NH3(aq) solution solution that has an unknown concentration. The equivalence point is reached after adding 22.50 mL of HCl(aq). a. Write out the complete balanced equation for the reaction that occurs in this titration. Wom b. How many moles of HCl were added to the NH3 solution? (IA)olor c. How many moles of NH3 were in the original 20.00 mL solution? ups in hobbLOao nto bobbe HOMS d. What was the concentration of NH3 in the original 20.0 mL solution? for

1 Explain the three steps that occur when KF dissolves in water. Draw diagrams for the hydration of the cation and for the anion.

Please don't provide handwritten solution .....

How many equivalents were used (20 mL, 0.75 M) of NaOBr. Please show and explain.

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...

Please calculate the amount of solid sodium hydroxide needed to make 200mL of a 0.2 M soulution. **Please give answer to nearest .001 g** Also, if 10 mL of the solution made in the last question is used to make another 125mL solution of NaOH, what is the new concentration? If you dont mind, please show the each step to solve the problem, that would be great!  Have a absolutely amazing day whoever you are that does these questions for students like me. :)

A 25.0-mL volume of a sodium hydroxide solution requires 19.6 mL of a 0.189 M hydrochloric acid for neutralization. A 10.0-mL volume of a phosphoric acid solution requires 34.9 mL of the sodium hydroxide solution for complete neutralization. Calculate the concentration of the phosphoric acid solution.

I titrate a sample of aqueous sulfuric acid with 14.27mL and 0.117M Potassium hydroxide. Calculate the number of moles of sulfuric acid that were in the sample.

From the tritrations below, calculate the molarity of the NaOH Solution in each of the following? Make sure to balance the equation. a) NaOH + HCl > NaCl + H2O  32 ml of NaOH is required to completely react with 25.00ml of 0.150m HCl b) NaOH + H2SO4 > Na2SO4 + H2O 42 ml of NaOH is required to completely react with 18.00 ml of 0.10m H2SO4

What percent of a 0.0138 M NaCN solution undergoes hydrolysis? [K, for HCN-3.98E-10] 0.182 4.27 0.0000309 0.000234 4.57 6:51 PM