A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Part A Determine whether or not 250 mgNaOH would exceed the capacity of the buffer to neutralize it. Determine whether or not 250 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part B Determine whether or not 350 mgKOH would exceed the capacity of the buffer to neutralize it. Determine whether or not 350 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part C Determine whether or not 1.25 gHBr would exceed the capacity of the buffer to neutralize it. Determine whether or not 1.25 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part D Determine whether or not 1.35 gHI would exceed the capacity of the buffer to neutralize it. Determine whether or not 1.35 would exceed the capacity of the buffer to neutralize it. yes no

THIS USER ASKED 👇

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Part A Determine whether or not 250 mgNaOH would exceed the capacity of the buffer to neutralize it. Determine whether or not 250 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part B Determine whether or not 350 mgKOH would exceed the capacity of the buffer to neutralize it. Determine whether or not 350 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part C Determine whether or not 1.25 gHBr would exceed the capacity of the buffer to neutralize it. Determine whether or not 1.25 would exceed the capacity of the buffer to neutralize it. yes no Request Answer Part D Determine whether or not 1.35 gHI would exceed the capacity of the buffer to neutralize it. Determine whether or not 1.35 would exceed the capacity of the buffer to neutralize it. yes no

THIS IS THE BEST ANSWER 👇

Neither of them will neutralize the buffer solution.

Explanation:

The buffer solution of HNO₂ and KNO₂ is neutralized when all the base acid of the buffer solution reacts and eats or when the added base reacts and consumes all the acid of the buffer solution.

First, we need to calculate the number of moles of the acid mole and the bottom of the buffer:

Now, let’s consider each case.

A) 250 mg of NaOH:

We need to calculate the number of moles of NaOH

For m: is the mass = 250 mg, and M: is the recommended mass = 39.99 g / mol

The number of moles of HNO₂ acid after reaction with NaOH – added base is:

After the reaction of HNO₂ with the NaOH, 0.044 moles of acid remain, so 250 mg of NaOH would not exceed the buffer’s ability to neutralize it.

B) 350 mg KOH:

The number of KOH moles is:

Now the number of moles of HNO₂ remaining in the solution is:

Therefore, 350 mg of KOH would not exceed the buffer capacity to neutralize it.

C) 1.25 g of HBr:

The number of HBr moles is:

Now the number of moles of the KNO₂ base remaining in solution after the reaction with HBr is:

Thus, 1.25 g of HBr would not exceed the buffer’s ability to neutralize it.

D) 1.35 g of HI:

The number of HI moles is:

Now the number of moles of the KNO₂ base remaining in solution after the reaction with HI is:

Accordingly, 1.35 g of HI would not exceed the buffer capacity to neutralize it.

Therefore, neither of them will neutralize the buffer solution.

I hope it helps you!