HaileyChristiansen20
11.03.2020 •
Chemistry
A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid
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Ответ:
The value of for the given acid is
Explanation:
To calculate the molarity of solution, we use the equation:
Initial mass of weak monoprotic acid = 1.00 g
Molar mass of weak monoprotic acid = 180 g/mol
Volume of solution = 300 mL
Putting values in above equation, we get:
To calculate the hydrogen ion concentration for given pH of the solution, we use the equation:
We are given:
pH = 2.62
Putting values in above equation, we get:
The chemical equation for the dissociation of weak monoprotic acid (HA) follows:
Initial: 0.0185
At eqllm: 0.0185-x x x
Evaluating the value of 'x'
So, equilibrium concentration of HA = (0.0185 - 0.0024) = 0.0161 M
Equilibrium concentration of = x = 0.0024 M
The expression of for above equation follows:
Putting values in above equation, we get:
Hence, the value of for the given acid is
Ответ:
Hope this helps :)
Explanation:
Phase changes are physical changes that take place when matter changes energy states, but chemical bonds are not broken or formed. ... The phase of a substance depends on the amount of energy the atoms contain. All atoms are in motion. :)