Calculate the pH of a solution that is 0.239 M acetic acid and 0.190 M sodium acetate. The Ka of acetic acid is 1.76×10–5 at 25°C. What is the pH of this mixture at 0°C? (At 0°C, Ka = 1.64x10-5)

The pH of the mixture at 0°C is 4.68

Explanation:

To calculate the pH at 0°C, we use the equation given by Henderson Hasselbalch:

We are given:

= negative logarithm of acid dissociation constant of acetic acid at 0°C = 4.78

pH = ?

Putting values in above equation, we get:

Hence, the pH of the mixture at 0°C is 4.68

- calcium has greater affinity to bond with electron receptors than hydrogen does and hence, it has the ability to replace hydrogen in most of its compounds.

- lithium has 2 valence electrons in the product because it can make only 1 bond with hydrogen. beryllium has 4 valence electrons in the product because it can only make 2 bonds. it has fewer electrons than neon and can react with electron donors. each hydrogen has 2 valence electrons, the same as helium.

- the covalent bond formed between carbon and hydrogen is polar because carbon is more electronegative than hydrogen and it attracts the bonded electron pair closer to itself, thus giving hydrogen a partial positive charge.

- a hydrogen bond is a relatively weak bond that hydrogen atoms make with the electronegative atoms nitrogen, oxygen or fluorine.

so the best choice is a.) 2 calcium (ca) atoms

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