Why is the normal boiling point of #HF# (#19.5# #""^@C#), so high compared to that of #HCl# (#-85.0# #""^@C#)?
For the same reason that water is a liquid at room temperature and pressure, whereas
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The higher normal boiling point of HF compared to HCl is due to the stronger hydrogen bonding present in HF molecules, which requires more energy to break compared to the weaker dipole-dipole interactions in HCl molecules.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- When a weak acid, for which #K_a=6,2xx10^-5# is titrated with a strong base, what is the #pH# at half-equivalence?
- What are some common mistakes students make with acids and bases?
- According to the equations below, what is the conjugate base of #HCO_3^-# ?
- Why do bases feel slick in nature?
- A certain sample of #"HClO"_2# has a concentration of #"0.125 M"#. Calculate the pH at equilibrium. Why can we not treat #"HClO"_2# as a strong acid, even though #K_a > 1#?

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