Explain why the addition of a small amount of base to an acidic buffer solution causes...

Explain why the addition of a small amount of base to an acidic buffer solution causes only a small change in the pH of the buffer solution. You should use any appropriate chemical and/or mathematical equations to substantiate your arguments

Expert Solution

queen_honey_blossom answered 2 years ago

pH of the Buffer after the addition of strong base Original buffer solution= 50.0 mL of...

pH of the Buffer after the addition of strong base Original buffer solution= 50.0 mL of 1.0 M CH3COOH 50.0 mL of 1.0 M NaCH3COO Take 50.0 mL of this buffer solution and add 2.0 mL of 1.0 M NaOH Calculate the expected pH of this solution.

1. If a small amount of strong base were added to a buffer made of a...

1. If a small amount of strong base were added to a buffer made of a weak acid HA and the lithium salt of its conjugate base, LiA, the pH does not change very much because.... a. No reaction occurs b. The strong base reacts with A- to give HA c. Adding a strong base changes the pKa of the base d. The strong base reacts with HA to give A- e. The strong base reacts with the Li+ to...

The addition of a small amount of a salt, such as (NH4)2SO4 to a solution containing...

The addition of a small amount of a salt, such as (NH4)2SO4 to a solution containing a charged protein increases the solubility of the protein in water. This observation is called the salting-in effect. However, the addition of large amounts of salt can decrease the solubility of the protein to such an extent that the protein precipitates from solution. This observation is called the salting-out effect and is widely used by biochemists to isolate and purify proteins. Consider the equilibrium...

For an acidic component, after treatment of a strong base the solution is then treated with...

For an acidic component, after treatment of a strong base the solution is then treated with a strong acid. Why is this step perfromed?

A) Why does a buffer solution require a weak acid/base conjugate pair, as opposed to a...

A) Why does a buffer solution require a weak acid/base conjugate pair, as opposed to a strong acid, and its conjugate? A strong acid will completely dissociate, suggesting that the conjugate base is really weak and will not neutralize any additional H+ ions. A strong acid will completely dissociate, suggesting that the conjugate base is really strong and will not neutralize any additional H+ ions. A strong acid will only partially dissociate, suggesting that the conjugate base is really weak...

2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without...

2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without a significant pH change. It is governed by the concentrations of the conjugate acid and base forms of the buffer. A 0.5 M buffer will require five times as much acid or base as a 0.1 M buffer for given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity...

An acidic buffer solution can be prepared from phosphoric acid and dihydrogen phosphate. a. What is...

An acidic buffer solution can be prepared from phosphoric acid and dihydrogen phosphate. a. What is the pH of solution prepared by mixing 23.5g of NaH 2 PO 4 and 15.0mL of concentrated phosphoric acid (14.7M) in enough water to give 1.25L of solution? b. By how much does the pH of this buffer solution change on the addition of 3.50 mL of 6.0M HCl?

a) Calculate the pH of 75 mL of the undiluted buffer solution after the addition of...

a) Calculate the pH of 75 mL of the undiluted buffer solution after the addition of 1 mL of 3 M HCl. b) Calculate the pH of 75 mL of the undiluted buffer solution after the addition of 15 mL of 3 M HCl. Buffer solution was made from 1 M of sodium acetate, and 1.1005 M of acetic acid. (pKa of acetic acid 4.75). pH of buffer = 4.79.

Calculate the pH of a buffer solution after the addition of 20.0 mL of 0.200 M...

Calculate the pH of a buffer solution after the addition of 20.0 mL of 0.200 M NaOH to 80.0 mL of 0.0500 M HC3H5O2 and 0.0250 M NaC3H5O2. (Ka = 1.4 x 10^-5)

Describe the buffer capacity of the acetic acid buffer solution in relation to the addition of both concentrated and dilute acids and bases

Data Table 1. Adding 0.1 M HCl from D1 into A1. Number of Drops pH of Solution 0 6 2 6 4 6 6 6 8 6 10 6 12 6 14 6 16 6 Data Table 2. Adding 0.1 M NaOH from D6 into A6. Drop Number pH of Solution 0 6 2 6 4 6 6 6 8 6 10 6 12 6 14 6 16 6 Data Table 3. Adding 6 M HCl from Pipet into...

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