ZuoTi.Pro
Question

Question 3 1 pts If you start with 80.0 mL of 0.445 M HNO3, calculate the [H] concentration following addition of 23.4 mL of
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

DATE holes a concentration & volume. moles of and And ) 4 20.44580.08 -0.0356 mol moles of base kolt) = on = 0.8488 0.0234 =

0 0
Add a comment
Know the answer?
Add Answer to:
Question 3 1 pts If you start with 80.0 mL of 0.445 M HNO3, calculate the...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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

  • Please explain the correct answer for both questions. Thank you! Incorrect Question 5 0/1 pts A...

    Please explain the correct answer for both questions. Thank you! Incorrect Question 5 0/1 pts A 25.0 mL sample of 0.723 M HCIO4 is titrated with 0.27 M KOH solution. The H30* concentration after the addition of 80.0 mL of KOH is M. (Cl is chlorine, not carbon and iodine) 0.4 3x10-13 1x107 0.7 4x10-2 Incorrect Question 6 0/1 pts What could be the pKof this weak acid according to the titration curve below? Weak Acid Titration Curve PH 10...

  • 1) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 16.0 mL of KOH....

    1) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 16.0 mL of KOH.Express your answer numerically.   pH=_______ 2) A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3.Express your answer numerically.   pH=_______ 3) A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x10-5 ) is titrated with 0.40 M NaOH. Calculate...

  • A 36.80-mL sample of 0.250 M HNO3 solution is titrated with 0.221 M KOH. Calculate the pH of the solution a before the...

    A 36.80-mL sample of 0.250 M HNO3 solution is titrated with 0.221 M KOH. Calculate the pH of the solution a before the addition of KOH pH= b after the addition of 6.45 mL KOH pH Cafter the addition of 13.20 mL KOH pH dafter the addition of 26.74 mL KOH pH e after the addition of 38.63 mL KOH pH f after the addition of 42.23 mL KOH pH К, - 1.8 х10-5 К 7.4 х 10-5 К, 5.0...

  • Question 3 2 pts How many mL of 0.233 M. HNO3(aq) are needed to neutralize 56.90...

    Question 3 2 pts How many mL of 0.233 M. HNO3(aq) are needed to neutralize 56.90 mL of a 0.1368 M solution of barium hydroxide, Ba(OH)2? 0 33.4 O 100.2 0 66.8 O 16.7 O 53.9

  • Question 4 5 pts Given the following reaction, calculate the electrical potential after adding 10ml of...

    Question 4 5 pts Given the following reaction, calculate the electrical potential after adding 10ml of cesium. Assume the analyte initially is present at a concentration of 0.0100 M and that a 25.0-ml sample is taken for analysis. The titrant, which is the underlined species, has a concentration of 0.0100 M. V2+(aq) + Ce4#lag) → V3+(aq) + Ce3+(ag) O 0.245 V 0 -0.265 V O 0.265 V 0 -0.245 V

  • A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the...

    A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 MM CH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 15.0 mL of NaOH. and Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pH of 2.80. You have in front...

  • Please help and explain the solutions! 1. A 25.0 mL sample of 0.300 M  HNO3 is titrated...

    Please help and explain the solutions! 1. A 25.0 mL sample of 0.300 M  HNO3 is titrated with 0.300 M NaOH. Calculate the pH before the addition of base 2. A 25.0 mL sample of 0.300 M  HNO3 is titrated with 0.300 M NaOH. Calculate the  pH after the addition of 24.0 mL of 0.300 M NaOH 3. A 25.0 mL sample of 0.300 M  HNO3 is titrated with 0.300 M NaOH. Calculate the  pH after the addition of 26 mL of 0.300 M NaOH...

  • Soln. 2.5x10-3 M Fe(NO3)3 mL 2.5X10-3 M KSCN mL 0.5 M HNO3 mL Absorbance A 5...

    Soln. 2.5x10-3 M Fe(NO3)3 mL 2.5X10-3 M KSCN mL 0.5 M HNO3 mL Absorbance A 5 1 4 0.020 B 5 2 3 0.034 C 5 3 2 0.037 D 5 4 1 0.056 E 5 5 0 0.066 Calibrated at max wavelength of FeSCN2+ = 485.80nm Final concentration of Fe3+ = 5.56*10-5 Using M1V1=M2V2, calculate the initial concentrations of the reactant Fe3+, (m) and SCN- (n) in each solution A-E.

  • ml O2.02L QUESTION 15 Calculate the new molarity if 45.0 mL of 3.2 M HNO3 is...

    ml O2.02L QUESTION 15 Calculate the new molarity if 45.0 mL of 3.2 M HNO3 is diluted to 125 ml. Report your answer rounded to 3 significant figures and only give a numerical value. QUESTION 16 Consider the following unbalanced equation: Na2SiF6(s) + Na(s) → Si(s) + NaF(s) How many grams of Na will be produced if 3.75 g of Na reacts with excess Na2SiF6? Report your answer rounded to 3 significant figures. Do not report any units, only a...

  • Question 1: In the laboratory you dilute 3.33 mL of a concentrated 6.00 M hydrochloric acid...

    Question 1: In the laboratory you dilute 3.33 mL of a concentrated 6.00 M hydrochloric acid solution to a total volume of 75.0 mL. What is the concentration of the dilute solution? M Question 2: You wish to make a 0.153 M hydroiodic acid solution from a stock solution of 3.00 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Thank-you!

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