calculate pH of 50.0 mL of a .100 M solution of the weak monoprotic acid HX
HX ==> H^+ + X^-
Set up an ICE chart and substitute into the expression for Ka for HX. Solve.
To calculate the pH of a weak monoprotic acid solution, we need to know the concentration (in moles per liter) and the dissociation constant (Ka) of the acid.
Given that the concentration of the weak acid HX is 0.100 M, we still need to know the Ka value of the acid to calculate its pH. The Ka value represents the extent of the acid dissociation in water.
Once we have the Ka value, we can use the Henderson-Hasselbalch equation to calculate the pH of the weak acid solution:
pH = pKa + log([A-]/[HA])
Where:
- pH is the measure of acidity or alkalinity on a logarithmic scale (0-14)
- pKa is the logarithmic form of Ka (negative logarithm of Ka)
- [A-] is the concentration of the conjugate base of the acid
- [HA] is the concentration of the acid itself
Since we don't have the Ka value of the weak acid, we cannot proceed with the calculation of pH without this information.