Question

3. You are asked to make a buffer solution with a pH of 3.40 by using 0.100 M HNO, and 0.100 M NaOH (aq). a. Explain why the
0 0
Add a comment Improve this question Transcribed image text
Answer #1

addition of Naot converts Some amount of HNO into NaNOL. HNO A +++ NO3 Nandy - Nat H NG commanian effect The above mechanism

Add a comment
Know the answer?
Add Answer to:
3. You are asked to make a buffer solution with a pH of 3.40 by using...
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
  • A buffer solution consists of 0.10 M HNO2 and 0.20 M NaNO2. If 0.010 moles of...

    A buffer solution consists of 0.10 M HNO2 and 0.20 M NaNO2. If 0.010 moles of sodium hydroxide are added to 200. ml the solution , what is the new pH of the solution (pKa (HNO2) = 3.40)?

  • 18. Consider a buffer solution containing HNO, and KNO, where the concentration of HNO2 is double...

    18. Consider a buffer solution containing HNO, and KNO, where the concentration of HNO2 is double the concentration of KNO,. Which statement about the buffer solution is true? a) The nitrite ion concentration will increase if a strong base is added Xb) The pH of this solution is equal to the pKa value of the HNO2. c) The pK, value of HNO, will decrease if a strong acid is added. R. is a cons d) The buffer capacity of this...

  • Your research adviser asks you to prepare 1 L of a 0.100 M buffer solution at...

    Your research adviser asks you to prepare 1 L of a 0.100 M buffer solution at pH 8.3, using your choice in (a). You begin by dissolving 0.100 moles of the compound in ~800 mL of water (you will fill it up to the 1 L mark after adding base). What volume (in mL) of 8 M NaOH must you add to your diluted buffer molecule to make the final solution pH 8.3

  • 5. You need to make 500.0 mL of a buffer with a pH of 2.20. You...

    5. You need to make 500.0 mL of a buffer with a pH of 2.20. You have the following substances to work with: 0.100 M NH3 Solid NaN3 Solid NaClO2 0.100 M HClO2 Solid NH4Cl Solid Na2SO3 0.100 M HN3 Solid NaHSO3 Ka for HClO2 = 1.1x10-2 Kb for NH3 = 1.8x10-5 Ka for HN3 = 1.9x10-5 Ka1 for H2SO3 = 1.7x10-2 Ka2 for H2SO3 = 6.4x10-8 (Assume that the addition of solid does not change the volume of the...

  • Calculate the pH of the buffer that results from mixing 90.0 mL of 0.350 M HNO2...

    Calculate the pH of the buffer that results from mixing 90.0 mL of 0.350 M HNO2 and 75.0 mL of 0.500 M NaNO2. (Ka = 4.60 x 10-4) a. Using the above initial buffer, calculate the new pH of the buffer when 15.0 mL of a 1.0 M solution of HCl is added. b. Using the above initial buffer, calculate the new pH of the buffer when 0.500 g of NaOH is added.

  • To make a buffer, a student mixes H2CO3 with NaHCO3 to form a solution which is 0.012 M carbonic acid (H2CO3) and 0.012...

    To make a buffer, a student mixes H2CO3 with NaHCO3 to form a solution which is 0.012 M carbonic acid (H2CO3) and 0.012 M (NaHCO3). The pH of the buffer solution is 6.37 The student adds 10.0 mL of 0.100 M NaOH to a fresh solution of his buffer. Calculate the pH after the addition of NaOH.

  • You are working in a lab and need to make a buffer with a pH =...

    You are working in a lab and need to make a buffer with a pH = 5.50. You have 5.00 M NaOH and 5.00 M HCl available. You observe that malonic acid (HO2CCH2CO2H or H2A) has pK1 = 2.847 and pK2 = 5.696. Given the mass of malonic acid needed from the last problem, how many mL of NaOH solution is needed to give a pH of 5.50 in the buffer solution? Assume that you will make 500. mL of...

  • pH of a buffer solution pH and Buffers IV pH of a Buffer Solution A.2019 Mass of sodium acetate, CH,COONa, g Mea...

    pH of a buffer solution pH and Buffers IV pH of a Buffer Solution A.2019 Mass of sodium acetate, CH,COONa, g Measured pH Calculated pH buffer solution prepared with dissolved CH,COONa +8.5 mL CH,COOH (aq) 5.54 40 mL buffer + 1.0 mL of 6.0 M HCI (aq) 4/.ces 40 mL buffer + 1.0 mL of 6.0 M NaOH (aq) 5.02 Calculated pH Measured pH 5,54 deionized water 40 mL DI water +1.0 mL of 6.0 M HCI (aq) 1.C03 40...

  • A solution of nitrous acid and potassium nitrite acts as a buffer due to reactions that...

    A solution of nitrous acid and potassium nitrite acts as a buffer due to reactions that occur within the solution when a strong acid or a strong base is added. Write the net ionic equation for the reaction that occurs in this buffer to react away any added HCl (aq). Write the net ionic equation for the reaction that occurs in this buffer to react away any added NaOH (aq). 3. A solution of nitrous acid and potassium nitrite acts...

  • A student must make a buffer solution with a pH of 2.00. Determine which weak acid...

    A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...

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