The KHP concentration does not have to be exactly 0.100M for several reasons. The most important reason is because the equilibrium between KHP and a monoprotic acid is not absolute, meaning that the concentrations of reactants and products can deviate slightly from the ideal value of 0.100M without significantly affecting the overall system. This means that if other factors are at play (such as temperature, pressure, or pH) then they can cause slight deviations in the concentration of KHP without having a major impact on its effectiveness or accuracy as an analytical standard.
One factor that affects the reaction equilibrium is temperature; higher temperatures tend to shift equilibria toward the side with fewer molecules, while lower temperatures favor reactions involving more molecules. Therefore, if a solution containing KHP was heated up, then there would be an increase in dissociation into KH+ and HP− ions which would result in a decrease in total KHP concentration but still maintain some level of accuracy when used as an analytical standard due to its relationship with other compounds present in solution that could also be affected by this change in temperature (e.g., water).
Another factor that affects reaction equilibria is pressure; high pressures tend to favor reactions involving more molecules while low pressures reverse this trend and instead favor reactions involving fewer molecules. Therefore, if there were changes in atmospheric pressure then this too could result in variations from ideal concentrations of KHP without impacting its accuracy or effectiveness as an analytical standard since it relies on relationships with other compounds than just itself that may also be affected by such changes in pressure (e.g., carbon dioxide).
Finally, pH levels can also affect reaction equilibria since acidic solutions tend to favor dissociation into ions while basic solutions prefer formation of molecular forms such as neutral species like alcohols or acids themselves like HCl or ethanol respectively. Therefore fluctuations within normal pH levels can lead to slight deviations from perfect concentrations but still provide accurate results when used as an analytical standard due to interactions between various components present within solution which should remain constant even within small shifts from optimal conditions (e.g., hydrogen bonding).
In conclusion, it is acceptable for KHPs concentration not to be exactly 0.100M due to numerous environmental factors such as temperature, pressure and pH levels being able to markedly affect equilibrium between ionic forms and neutral species without significantly impacting their usefulness as analytical standards given their reliance on relationships with multiple components rather than just themselves alone.(Dong et al., 2017) .
References:
Dong C., Zhou S., Li B., Wang Y., Liu W-F.(2017). Study on Thermal Equilibrium Isotherm Modelingand Its Application—Taking Acetic Acid–Water Systemas An Example ACS Omega 2(12), 8722–8728
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