A 25.0 mL solution of 0.817 mol L-1 NH3 is titrated using 0.669 mol L-1 HCl. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment?
find the volume of HCl used to reach equivalence point
M(NH3)*V(NH3) =M(HCl)*V(HCl)
0.817 M *25.0 mL = 0.669 M *V(HCl)
V(HCl) = 30.5 mL
Answer: 30.5 mL
A 25.0 mL solution of 0.817 mol L-1 NH3 is titrated using 0.669 mol L-1 HCl....
A 29.3 mL solution of 0.588 mol L-1 HCl is titrated using 0.507 mol L-1NaOH. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment?
1.A) A 29.8 mL solution of 0.298 mol L-1 HCl is titrated using 0.173 mol L-1 NaOH.What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or KB values in your textbook in chapter 15. B) A 10.1 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What will be the pH of the solution after 4.07 mL of the HCl solution is added?...
ng: A 28.6 ml solution of 0.582 mol L NaOH is titrated using 0.683 mol L HC. What volume of HCl (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or KB values in your textbook in chapter 15. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". zion
A 17.6 mL solution of 0.493 mol L-1 HCOOH is titrated using 0.230 mol L-1 NaOH. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or KB values in your textbook in chapter 15. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
What is the pH of a solution containing 0.342 mol L-1 NH3 and 0.140 mol L-1NH4? Round your answer to 2 decimal places. Remember you can find KA and/or Kg values in your textbook in chapter 15. Answer: Check A 45.3 mL solution of 0.283 mol L-1 HCl is titrated using 0.820 mol L-'NaOH. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or Ke values in your...
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
E. Titration calculations 1. A 25.0-ml sample of 0.100 M HCl is titrated with 0.125 M NaOH. How many milliliters of the titrant will be need to reach the equivalence point? 2. A 25.0-ml sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCI. How many milliliters of the titrant will be need to reach the equivalence point? 3. For the following titrations, determine if the equivalence points will be acidic, basic, or neutral i. NH3 titrated with HCI...
A 13.3 mL solution of 0.100 mol L-1 HCl is titrated using 0.150 mol L-1 NaOH. What is the pH of the solution after 4.59 mL of the NaOH solution is added?
A 15.0 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What is the pH of the solution after 1.33 mL of the HCl solution is added? Express your answer to 2 decimal places
The sample of 20.00 mL of 0.015 M NH3 is titrated with 0.030 M HCl. (a) Show the reaction between NH3 and H+. (1 point) (b) Find the volume of 0.030 M HCl needed to reach the equivalence point. (1 point) (c) Show the reaction of hydrolysis of product from the step (a). (1 point) (d) Calculate the pH at the equivalence point (Ka of NH4+ is 5.6 x 10–10). (1 point) Hint: Use Tables. Example of answer: (a) [show...