Abuffer is prepared by combining 25 ml of 0.5o mnh(aq) with 25 ml of 0.20 m hci. what is the ph of the buffer? (ka (nh4) = 5.6 x 10 ) a. 8.86 b. 9.65 c. 8.00 d. 7.76 e. 9.43

 e) 9.43

Explanation: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid and the pH of the buffer is calculated using Handerson equation:

There are 25 mL of 0.50 M which is a weak base. 25 mL of 0.20 M HCl, a strong acid are added. Ammonia reacts with HCl to form its conjugate acid, ammonium ion. The net ionic equation will be:

From above reaction, ammonia and HCl react in 1:1 mol ratio. Let's calculate the moles of each we have before the reaction. There is also, 1:1 mol ratio between HCl and ammonium ion.

moles of ammonia =

= 0.0125 mol

moles of HCl =

= 0.005 mol

Excess moles of ammonia = 0.0125 - 0.005 = 0.0075 mol

moles of ammonium ion formed = 0.005 mol

Total volume of the solution = 0.025 mL + 0.025 mL = 0.050 L

concentration of ammonia in buffer =

= 0.15 M

concentration of ammonium ion in buffer =

= 0.10 M

pKa is calculated from given Ka as:

pKa = 9.25

Plug in the values in Handerson equation:

pH = 9.25 + 0.18

pH = 9.43

So, the correct choice is e) 9.43 .

The [H⁺] of the solution is 1.74*10⁻⁹ M

Explanation:

pH, short for Hydrogen Potential, is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance. The pH scale ranges from 0 to 14. Values less than 7 indicate the acidity range and those greater than 7 indicate alkalinity or basicity. Value 7 is considered neutral.

The pH is calculated as the negative logarithm (base 10) of the molar concentration of the hydrogen or proton ions (H⁺) or hydronium ions (H₃O⁺).

pH= - log [H⁺] = -log [H₃O⁺]

In this case, you know that pH= 8.76.  Replacing in the definition of pH:

8.76 = -log [H⁺]

Solving:

[H⁺]=  10⁽⁻⁸ ⁷⁶⁾

[H⁺]= 1.74*10⁻⁹ M

The [H⁺] of the solution is 1.74*10⁻⁹ M