If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and...

Question

Question

If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and...

If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and 0.0600 mol HC6H5O72-, what would be the new concentration of HC6H5O72- after 25.0 mL of 0.125 M NaOH is added to the buffer?'

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

des) Stef & find males of Naon. Males - Molarity & Volume in L Poles = 00 125 M X 0.025L Mnaoy² 0.003 mal Step 6. Rxn of naon

Add a comment

Answer 2

Similar Homework Help Questions

If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and...

If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and 0.0600 mol HC6H5O72- , what would be the new concentration of HC6H5O72- after 25.0 mL of 0.125 M NaOH is added to the buffer?
2.a (0.5 pts) Open Response Question: Citric acid, H:CHO, is a triprotic acid. Consider a buffer...

2.a (0.5 pts) Open Response Question: Citric acid, H:CHO, is a triprotic acid. Consider a buffer system comprising H-CH:0," and HC,H,O, ions. What is the net ionic equation for the reaction that occurs when NaOH is added to a buffer containing HC.H.O.and HCHO? WRITE THE EQUATION CLEARLY IN THE ANSWER BOX. ANSWER: BALANCED NET IONIC EQUATION Score: 10,5 2.b (1.5 pts) Open Response Question: If a 250. mL sample of the above buffer solution initially has 0.0800 mol H.C.H.O., and...
=Assume you have prepared 100.0 mL of a buffer solution using 0.400 mol of acetic acid...

=Assume you have prepared 100.0 mL of a buffer solution using 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate. The pH of this buffer solution is initially 4.74. After preparing this buffer solution, you added 55.0 mL of a 1.10 M NaOH solution to your buffer to see what would happen. What will the pH of this new solution be?

a) A 25.00-mL sample of monoprotic acid was titrated with 0.0800 M potassium hydroxide solution. The...

a) A 25.00-mL sample of monoprotic acid was titrated with 0.0800 M potassium hydroxide solution. The equivalence point was reached after 18.75 mL of base was added. Calculate the concentration of the acid. b) A 15.00-mL sample of 0.120 M nitric acid was titrated with 0.0800 M potassium hydroxide. Calculate the pH of the sample when 10.00 mL of the base has been added.
A 87.0 mL sample of 0.0400 M HBrO4 is titrated with 0.0800 M NaOH solution.

37. A 87.0 mL sample of 0.0400 M HBrO4 is titrated with 0.0800 M NaOH solution. Calculate the pH after the following volumes of base have been added.
#1. If you have 250. mL of a buffer that is 0.12 M in H2PO4- and...

#1. If you have 250. mL of a buffer that is 0.12 M in H2PO4- and 0.12 M HPO42- , what will be the pH after 27.77 mL of 0.193 M NaOH is added? Ka2 is 6.21 x 10-8 . #2. Given 1000. mL of a 0.434 M solution of C2H5NH2 (pKb = 3.19), what is the pH if 26.45 g of C2H5NH3Cl (81.5446 g/mol) are added?

A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125...

A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125 M NaOH solution. Ka of HCOOH = 1.7 x 10−4. a. Calculate the pH of the solution after 50 mL of NaOH solution has been added. b. How many mL of 0.125 M NaOH need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of...

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
1. A buffer is prepared using 0.20 mol of H2PO4 and 0.10 mol of HPO42 in 500 mL of solution. Will...

1. A buffer is prepared using 0.20 mol of H2PO4 and 0.10 mol of HPO42 in 500 mL of solution. Will the buffer capacity be exceeded if 5.6 g of KOH is added to it? What is the pH of the original solution and the pH of the new solution? (Kb 1.6 x 10-7) 2. How many milliliters of 0.113M HBr should be added to 52.2 ml of 0.0134 M morpholine to give a pH of 8? (The pKa of...

A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI.

Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.

If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7- and...

Homework Answers