[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Acid/Base Reactions > Quantitative Analysis >
[/cs_text][cs_text]Calculation of pKa for strong and weak acids:
- For HCl, which is a strong acid, the Ka value is 1.3 x 106. Hence,
pKa = -log10(Ka)
= -log10(1.3 x 106)
= -6.1
- For HCOOH, which is a weak acid, the Ka value is 1.8 x 10-4. Hence,
pKa = -log10(Ka)
= -log10(1.8 x 10-4)
= 3.7
- Strong acids have a higher Ka value because they dissociate completely in aqueous solution. Since pKa is the negative logarithm of Ka, it tends to be lower. The opposite scenario is for weak acids which have a lower Ka value and a higher pKa value.
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