One liter of this solution could be converted into a buffer by the addition of 0.25mol NH₄Cl, and 0.12 mol HCl.
A buffer is a substance that can withstand a pH change when acidic or basic substances are added. Small additions of acid or base can be neutralized by it, keeping the pH of the solution largely constant. For procedures and/or reactions that call for particular and stable pH ranges, this is significant. The pH range and capacity of buffer solutions determine how much acid or base can be neutralized before pH changes and how much pH will vary.
A weak acid and its conjugate base, or vice versa, are combined in solution to form a buffer.
The conjugate base of ammonia (NH3), which is a weak base, is NH4+. Therefore, adding 0.25 mol of NH4Cl will change the solution into a buffer. Additionally, NH3 and HCl interact to form NH4+. Therefore, 0.12 mol of HCl added will result in NH4+. All of the NH3 is consumed by 0.25 mol HCl.
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