Consider the titration of 30.0 mL of 0.100 M HC 2 H 3 O 2 with 0.100 M NaNH 2 . Which volume of NaNH 2 would take place within the buffer region? a) 30.0 mL b) 50.0 mL c) 10.0 mL d) 100.0 mL e) 1.5 L

Here it says, consider the titration of 30 ml's of 0.100 molar acetic acid with 0.100 molar sodium amide. Which volume of sodium amide would take place within the buffer region? Alright, so remember the buffer region occurs before we get to the equivalence point in our titration curve. So we would need to determine what our equivalence volume is first. So we're gonna say m acid times v acid equals m base times v base. Here this will be 0.100 molar, This is 30 ml equals 0.100 molar times volume of our base. Divide both sides by 0.100 molar, and we'd have the volume of our base to reach the equivalence point, which would be 30 ml. So it takes 30 ml to reach the equivalence point, but we want to find the buffer region. So we just need to find a volume less than 30 ml. Less than 30 ml's would mean that we haven't got to the equivalence point and a buffer can still exist. When we take a look, it has to be less than 30, still doesn't work. C is an answer, not less than 30. And this is 1.5 liters, which translates to 1,500 milliliters. So definitely not less than 30 amounts. So here, the answer would have to be option C. Just remember, before the equivalence point has been reached we can have a buffer region existing. Okay. So all we have to do is calculate the equivalence volume and then look for a volume less than that. That would ensure that we could have a buffer region.

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18. Aqueous Equilibrium

Weak Titrate-Strong Titrant Curves

General Chemistry

18. Aqueous Equilibrium

Weak Titrate-Strong Titrant Curves

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Multiple Choice

Consider the titration of 30.0 mL of 0.100 M HC₂H₃O₂ with 0.100 M NaNH₂. Which volume of NaNH₂ would take place within the buffer region?
a) 30.0 mL b) 50.0 mL c) 10.0 mL d) 100.0 mL e) 1.5 L

30.0 mL

50.0 mL

10.0 mL

100.0 mL

1.5 L

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Verified step by step guidance

Identify the chemical reaction involved in the titration: HC2H3O2 (acetic acid) reacts with NaNH2 (sodium amide) to form C2H3O2^- (acetate ion) and NH3 (ammonia).

Understand that the buffer region in a titration curve is where the pH changes gradually, typically occurring when the amounts of acid and its conjugate base are comparable.

Calculate the initial moles of acetic acid (HC2H3O2) using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Here, \( \text{moles of HC2H3O2} = 0.100 \text{ M} \times 0.030 \text{ L} \).

Determine the volume of NaNH2 needed to reach the buffer region. This occurs when the moles of NaNH2 added are approximately half the initial moles of HC2H3O2, as this will create a significant amount of both the acid and its conjugate base.

Calculate the volume of NaNH2 required using the stoichiometry of the reaction and the concentration of NaNH2. Use the formula: \( \text{volume} = \frac{\text{moles}}{\text{concentration}} \) to find the volume that corresponds to half the initial moles of HC2H3O2.