C) What additional volume of 10.0 M HCl would be needed to exhaust the remaining capacity...

C) What additional volume of 10.0 M HCl would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? THE CORRECT ANSWER IS 1.8 ML BUT PLEASE PROVIDE YOUR WORK TO SHOW HOW YOU ARRIVED AT THIS ANSWER.

B) To provide some context, the question from part B was The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0150 mol of hydrogen ions without changing the volume. What is the pH of the final solution? and the answer was 7.44.

A) The question from part A was What volume of 10.0 M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl? and the ANSWER was 6.7mL.

Again, I only need help arriving to the answer of 1.8 mL for Part C.

Expert Solution

queen_honey_blossom answered 2 years ago

what volume of 0.200 m HCl solution is needed to neutralize 0.400 g of NaHCO3

Find the volume (mL) and the pH of 0.135 M HCl needed to reach the equivalence...

Find the volume (mL) and the pH of 0.135 M HCl needed to reach the equivalence point(s) in titrations of the following. (You need to find the pH at the equivalence point, not the initial pH of the solution. (a) 50.8 mL of 0.272 M NH3 (b) 11.8 mL of 1.76 M CH3NH2

Find the pH at the equivalence point(s) and the volume (mL) of 0.125 M HCl needed...

Find the pH at the equivalence point(s) and the volume (mL) of 0.125 M HCl needed to reach the point(s) in titrations of the following. (See this table.) (a) 69.0 mL of 0.225 M NH3 volume to reach equivalence point pH at equivalence point

1. What is the change in pH when 10.0 mL of 0.010 M HCl is added...

1. What is the change in pH when 10.0 mL of 0.010 M HCl is added to 500 mL of pure water. 2. What is the change in pH when 10.0 mL of 0.010 M NaOH is added to 500 mL of pure water.

What is the pH after adding 10.0 mL of 0.10 M HCl to a 90.0 mL...

What is the pH after adding 10.0 mL of 0.10 M HCl to a 90.0 mL buffer solution of 0.60 M CH3COOH and 0.40 M CH3COONa at 25 °C? (Ka = 1.8 x 10−5)? What reaction will occur when HCl is added to the above buffer? 1) How many moles of acetic acid are present after the reaction? 2) How many moles of acetate ion are present after the reaction? 3) What is the concentration (in M) of acetic acid...

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution....

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution. (potentially useful info: Ka of NH4+ = 5.6 x 10−10)

What is the buffer capacity for a solution that requires 3.35 mL of 0.10 M HCl...

What is the buffer capacity for a solution that requires 3.35 mL of 0.10 M HCl to change the pH by 1 unit?

What volume of 0.496 M HCl is required to neutralize 20.0 mL of 0.809 M sodium...

What volume of 0.496 M HCl is required to neutralize 20.0 mL of 0.809 M sodium hydroxide? b.) If you added 35.0 mL of hydrochloric acid solution to the sodium hydroxide, will the resulting solution be acidic or basic? Explain your reasoning. c.) Describe how you would neutralize the new solution using amounts (in volume) of either 0.496 M HCl or 0.809 M sodium hydroxide.

What volume of 6.00 M HNO3 is needed to make 500.0 mL of a 0.250 M...

What volume of 6.00 M HNO3 is needed to make 500.0 mL of a 0.250 M solution?

A 10.0−mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate...

A 10.0−mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate the pH after the following additions of the HCl solution a)0mL b)10ml c)30mL d)40mL

Question