Question

Exatnp ml of 0.20 M calculate the pH in the titratio NH, by 0.1 M HCI (NH, 1.8 Before any acid is added After the addition of 20 ml of At equivalence point After 90 ml of HCl
0 0
Add a comment Improve this question Transcribed image text
Answer #1

2. (4-7447 ㅢ업 o-20) 2-72, ns.rf mmmol.f HU 6-1 X 20-2 mrno, 2 ム、F447 + 0.06 M

no.of mm sl dt HU 0、, a 90 9 γη,n.丿 t2o6 6 final 3

Add a comment
Know the answer?
Add Answer to:
Exatnp ml of 0.20 M calculate the pH in the titratio NH, by 0.1 M HCI...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine whic...

    Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...

  • A student performs the titration of 25.0 mL of HCI with 0.1 M NaOH. If the...

    A student performs the titration of 25.0 mL of HCI with 0.1 M NaOH. If the acid concentration is 0.1 M and 35.0 mL of base are added, the hydroxide concentration and the pH are: [OH-] = 1.67 times 10^-2 M, pH = 12.22 [OH-] = 3.5 M, pH = 13.46 [OH-] = 1.67 times 10^-2 M, pH = 1.78 [OH-] = 2.58 times 10^-3 M, pH = 13.51 the pH at the equivalence point when a 0.20 M weak...

  • 3) A 5000 ml solution of 0.50 M NH (K-18210) sted with 0.35 M HCl solution...

    3) A 5000 ml solution of 0.50 M NH (K-18210) sted with 0.35 M HCl solution a) Calculate the pll before any HCl has been added.) b) Calculate the ph when 160 ml. HCI bave been let peines How many mit of Hcl must be added to reach the equivalence point? Et points) Page 2 4) What is the pit at the equivalence point?(3 p c) What is the pH afer 1200 mL of Hawe benadept)

  • Using the standardized concentrations for M(OH)2 and HCl determined in this investigation, calculate the pH for...

    Using the standardized concentrations for M(OH)2 and HCl determined in this investigation, calculate the pH for a strong acid + strong base titration in which 5.00 mL of the M(OH)2 was transferred via pipet to a beaker and HCl was added from the buret. concentration M(OH)2 .07 concentration HCl .0512 Calculate the pH: a) before any HCl is added b) after the addition of 4.00 mL HCl c) after the addition of 9.00 mL HCl d) 4.00 mL beyond the...

  • The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc-...

    The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc- is a weak base. Ka for acetic acid = 1.75 * 10^-5. a) Calculate the pH of the 50.0 mL of 0.1 M OAc- solution before the addition of any HCl. b) Calculate the pH of the resulting solution after the addition of 5.0 mL of 0.2 M HCl to the 50.0 mL of 0.1 M OAc- solution. c)  Calculate the pH of the resulting...

  • 7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate...

    7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate the pH of the following and sketch the titration curve. Kb 1.8 x 10 f. Before the titration starts g. After addition of 2.5 ml of HCl h. After addition of 5.0 ml of HCI i. After addition of 10.0 ml of HC

  • A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3

    1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is   [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...

  • In the titration of 100 ml of a 0.1 M H3PO4 with 0.5 M NAOH, calculate...

    In the titration of 100 ml of a 0.1 M H3PO4 with 0.5 M NAOH, calculate the pH of the solution at each of the following points: A) before any NaOH added B) After 10 mL of NaOH added C) at 1st equivalence point

  • Please help! For the titration of 50. mL of 0.10 M ammonia with 0.10 M HCl,...

    Please help! For the titration of 50. mL of 0.10 M ammonia with 0.10 M HCl, calculate the pH For ammonia, NH3, Kh = 1.8 x 105. (a) Before the addition of any HCl solution pH= The number of significant digits is set to 4; the tolerance is +/-2% (b) After 20. mL of the acid has been added pH = The number of siqnificant digits is set to 3; the tolerance is +/-2% (c) After half of the NH3...

  • 4) Calculate the pH at the equivalence point for the titration below: 150 mL 0.10 M HCI against 7...

    4) Calculate the pH at the equivalence point for the titration below: 150 mL 0.10 M HCI against 75 mL of 0.20 M NH3 4) Calculate the pH at the equivalence point for the titration below: 150 mL 0.10 M HCI against 75 mL of 0.20 M NH3

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT