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Based on your description, I would suggest to add $\displaystyle\frac{\pu{321 g}}{\pu{1.1998 g cm^{-3}}} = \pu{267.5 mL}$ of saturated salt solution (assuming approx. $\pu{25 °C},$ ambient temperature).
A report The Densities of Saturated Solutions of
NaCl and KCl from 10° to 105 °C by U.S. Geological Survey (PDF) contains a collection of density values for ...
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This question and the one referenced by Mithoron address NH$_4$HF$_2$ as an entity in itself which must be examined as a whole.
It is easier conceptually to rewrite the formula for the compound as NH$_4$F.HF. Consider adding NH$_4$F to water: you get a pH near 7. In a separate container, add HF to water (~0.1 M); you get a pH ~1 https://ehs.princeton.edu/...
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You need to write out all the possible equilibria just like you do in the case of a multiprotic acid like Phosphoric acid. You will also need to have a pKa for every equation. The bifluoride ion will obviously dissociate in water
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We happen to be measuring aqueous solutions instead, so I am trying to identify useful reference solutions we can prepare.
This experiment is really problematic. mid-IR is not meant for aqueous solutions. Water is a no-no in infrared spectroscopy. Look at the low transmittance of water in mid IR range. Liquid water is going to swamp everything. What will be ...
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Both your paragraphs are valid, as all present components are balanced by 3, mutually linked equilibrium reactions, with the respective equilibrium constants:
$\ce{HF + H2O <=> F- + H3O+}$, $K_\mathrm{a}$
$\ce{F- + H2O <=> HF + OH-}$, $K_\mathrm{b}$
$\ce{2 H2O <=> H2O+ + OH-}$, $K_\mathrm{w}$
with the relation $K_\mathrm{a} \cdot K_\mathrm{...
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