a. How much solid NaNO2 should you add to a solution of 850. mL of 0.200...

Question

Question

Answer 1

Answer #1

a pH of base 0.166 M

b Base is added

c pH is 2.80

As per Henderson equation [Base + log PH = pka (feid log (base pHopka [Aeid (pH-pka) 10 [Base Anid Propka (Aeid]xio こ 0.235 M

Answer 2

Similar Homework Help Questions

What mass in grams of NaNO2 (69.0 g / mol) will it be necessary to add...

What mass in grams of NaNO2 (69.0 g / mol) will it be necessary to add to 250.0 ml of 0.200 M solution in HNO2 to produce a buffer of pH equal to 3.50
What mass in grams of NaNO2 (69.0 g / mol) will it be necessary to add...

What mass in grams of NaNO2 (69.0 g / mol) will it be necessary to add to 250.0 ml of 0.200 M solution in HNO2 to produce a buffer of pH equal to 3.50 ka = 7.1x10 ^ -4)
How many mL of 3 M NaOH solution should be added to 100 mL of 0.200...

How many mL of 3 M NaOH solution should be added to 100 mL of 0.200 M acetic acid to make acetate buffer, pH 5.00

3. You are asked to make a buffer solution with a pH of 3.40 by using...

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 addition of 0.100 M HNO2 to 0.100 M NaOH(aq) can result in the formation of a buffer solution. Include the net ionic equations for the reaction that occurs when you combine HNO2 (aq) and NaOH(aq). Determine the volume, in ml, of 0.100 NaOH(aq) the student should add to 100 mL of 0.100...
You have solutions of 0.200 M HF and 0.200 M KF (Ka for HF = 7.2...

You have solutions of 0.200 M HF and 0.200 M KF (Ka for HF = 7.2 × 10–4). A buffer of pH 3.00 is needed. What volumes of HNO2 and KNO2 are required to make 1 L of buffered solution? I am really confused about how to do every step of this. Please write it out and explain EVERYTHING. Thank you
Does the pH of the solution increase, decrease, or stay the same when you add solid...

Does the pH of the solution increase, decrease, or stay the same when you add solid sodium hydrogen oxalate, NaHC2O4 to a dilute aqueous solution of oxalic acid, H2C2O4? Explain your answer using the equation below. H2C2O4 (aq) + H2O (l)⇌ HC2O41– (aq) + H3O+ (aq) 2)Why a solution of sodium chloride and hydrochloric acid cannot act as a buffer? (b) Propose a conjugate acid/base pair which can function as a buffer. 3) (a) Calculate the pH of a buffer...

Question 4 20 points Saved You add 10.00 mL of 0.200 M NaOH to 25.00 mL...

Question 4 20 points Saved You add 10.00 mL of 0.200 M NaOH to 25.00 mL of pure water, and to this mixture you then add 5.00 mL of 0.100 M HCI. What will be the pH of the resulting solution? 13.00 Question 4 of 5 Moving to another question will save this response.
Question 4 20 points Save Answer You add 10.00 mL of 0.200 M NaOH to 25.00...

Question 4 20 points Save Answer You add 10.00 mL of 0.200 M NaOH to 25.00 mL of pure water, and to this mixture you then add 5.00 ml of 0.100 M HCI. What will be the pH of the resulting solution? 7.00 OOOOO
wo 1015 Question 1 20 points You add 5.00 mL of 0.200 M NaOH to 50.00...

wo 1015 Question 1 20 points You add 5.00 mL of 0.200 M NaOH to 50.00 mL of pure water, and to this mixture you then add 14,00 ml. of 0.700 M HCI. What will be the pH of the resulting solution? Moving to another question will save this response Question of

12. You are asked to prepare 500. mL of a 0.200 M acetate buffer at pH...

12. You are asked to prepare 500. mL of a 0.200 M acetate buffer at pH 4.90 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76), 3.00 M NaOH, and water. Answer the following questions regarding the preparation of the buffer. a) How many grams of acetic acid will you need to prepare the 500 mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. g=? B) What volume of 3.00 M...