Question

Sort the pH of the following mixtures from LOWEST (most acidic) to HIGHEST (most basic): (I)...

Sort the pH of the following mixtures from LOWEST (most acidic) to HIGHEST (most basic):

(I) 0.001 mol of HCl added to 1 L water

(II) 0.001 mol HCl added to a buffer solution of 0.1 M HCOOH and 0.1 M NaHCOO (pKa=3.75)

(III) 0.001 mol HCl added to a buffer solution of 0.1 M NH4Cl and NH3 (pKa=9.25)

Homework Answers

Answer #1

1) concentration of HCl = n/v = 0.001/1 = 0.001 M

   pH = -log(H3O+)

      = -log0.001

   = 3


2) pH of acidic buffer = pka+log(NaHCOO-HCl/HCOOH+HCl)

           pka of HCOOH = 3.75

pH = 3.75+log((0.1-0.001)/(0.1+0.001))

     = 3.74

3) pH of basic buffer =14 - ( pkb+log(NH4Cl+HCl/NH3-HCl))

pkb of NH3 = 14-9.25 = 4.75

      = 14 - (4.75+log((0.1+0.001)/(0.1-0.001))

      = 9.24

order of pH : III > II > I

Know the answer?
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
Similar Questions
Find the pH of a buffer solution that is 0.90 M NH3 and 0.80 M in...
Find the pH of a buffer solution that is 0.90 M NH3 and 0.80 M in NH4Cl. Find the pH of the solution after 0.10 mol of HCl has been added to 1.00 L of the solution. Please show clear/concise step by step instructions, thank you!
Which solution is most acidic (that is, which one has the lowest pH)? 1.0 M HF...
Which solution is most acidic (that is, which one has the lowest pH)? 1.0 M HF 0.50 M HF 0.50 M HCl
1. How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol) must...
1. How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol) must be added to 650. mL of 0.951-M solution of NH3 in order to prepare a pH = 10.50 buffer? 2. What volume (to the nearest 0.1 mL) of 4.40-M HCl must be added to 0.450 L of 0.150-M K2HPO4 to prepare a pH = 6.60 buffer?
PLEASE SHOW WORK 4. Calculate the [H+], pH and percent dissociation of a solution that is...
PLEASE SHOW WORK 4. Calculate the [H+], pH and percent dissociation of a solution that is 0.50 M in HOCl and 0.60 M in NaOCl. 5. Calculate the [H+], pH and percent dissociation of a solution that is 1.0 M in aniline (C6H5NH2) and 1.2 M in C6H5NH3Cl. 6. A solution contains 0.60 mol of NH4Cl and 0.30 mol of NH3 in 1.5 L. What is the pH if 0.070 mol of HCl is added to this buffer?  
1 a. How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol)...
1 a. How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol) must be added to 900. mL of 0.923-M solution of NH3 in order to prepare a pH = 8.90 buffer? b. What volume (to the nearest 0.1 mL) of 6.70-M NaOH must be added to 0.550 L of 0.250-M HNO2 to prepare a pH = 3.00 buffer c. What volume (to the nearest 0.1 mL) of 6.20-M HCl must be added to 0.400 L...
a) What volume (to the nearest 0.1 mL) of 6.60-M HCl must be added to 0.450...
a) What volume (to the nearest 0.1 mL) of 6.60-M HCl must be added to 0.450 L of 0.200-M K2HPO4 to prepare a pH = 7.40 buffer? b) How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol) must be added to 400. mL of 0.964-M solution of NH3 in order to prepare a pH = 8.75 buffer? pKb = 4.75
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH...
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH change when 0.085 mol NaOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = 2.) Determine the pH change when 0.044 mol HNO3 is added to 1.00 L of a buffer solution that is 0.462 M in HF and 0.218 M in F-. pH after addition − pH before addition = pH change =
1) Calculate the pH of a 100 ml solution containing 0.6 grams of NaH2PO4 and 0.142...
1) Calculate the pH of a 100 ml solution containing 0.6 grams of NaH2PO4 and 0.142 grams of Na2HPO4 The pKa of NaH2PO4 = 7.2 Mol. Wt. of NaH2PO4 = 120 Mol. Wt. Of Na2HPO4 = 142 2) Calculate the pH of a solution obtained when 1.0 ml of 0.1 M HCL is added to 99.0 ml pure water. 3) Calculate the pH of the solution obtained by adding 1.0 ml of 0.1 M HCl to 99 ml of buffer...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl and 0.2 M NH3 (Ka for NH4Cl = 5.6 x 10-10). Assume 2 significant figures in all of the given concentrations so that you should calculate all of the following pH values to two decimal places. 1. Calculate the pH of this solution. 2. Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on...
Calculate the pH of the solution that results from each of the following mixtures. 1) 55.0...
Calculate the pH of the solution that results from each of the following mixtures. 1) 55.0 mL of 0.15 M HCHO2 with 80.0 mL of 0.13 M. Express your answer using two decimal places. 2) 135.0 mL of 0.13 M NH3 with 260.0 mL of 0.13 M NH4Cl. Express your answer using two decimal places.